$course$/Chemistry Common Assessments/Semester 2/Quarter 4/Unit 9: Kinetics and Equilibrium/9B: variables affecting reaction rate 1 Adding a catalyst will most likely [[1]] the rate of a chemical reaction.

]]> 1.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> increase 1 decrease 1 not effect 1 2 Stirring the reactants would probably [[1]] the rate of a chemical reaction.

]]> 1.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> increase 1 decrease 1 not effect 1 3 Placing the reactants in an ice bath would most likely [[2]] the rate of a chemical reaction.

]]> 1.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> increase 1 decrease 1 not effect 1 5 Grinding the reactants with a mortar and pestle would most likely [[1]] the rate of a chemical reaction.

]]> 1.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> increase 1 decrease 1 not effect 1 6 Using a lower concentration of reactants would most likely [[2]] the rate of a chemical reaction.

]]> 1.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> increase 1 decrease 1 not effect 1 7 Heating the reactants would most likely [[1]] the rate of a chemical reaction.

]]> 1.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> increase 1 decrease 1 not effect 1 9 When reactants are stirred or mixed, the reaction rate is expected to [[1]] because the [[6]] [[8]].

]]> 3.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> increase 1 decrease 1 stay the same 1 thermal energy 2 concentration 2 collision rate 2 catalysis 2 increases 3 decreases 3 $course$/Chemistry Common Assessments/Semester 2/Quarter 4/Unit 9: Kinetics and Equilibrium/9D: Le Chatelier le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the temperature is lowered, then [[1]] is favored because it [[10]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the temperature is raised, then [[2]] is favored because it [[9]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the pressure is raised, then [[1]] is favored because it [[12]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 reduces the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the pressure is lowered, then [[2]] is favored because it [[11]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the concentration of nitrogen is increased, then [[1]] is favored because it [[4]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the concentration of hydrogen is decreased, then [[2]] is favored because it [[5]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the concentration of hydrogen is increased, then [[1]] is favored because it [[6]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the concentration of ammonia is increased, then [[2]] is favored because it [[8]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the reaction

N_2(g) + 3 H_2(g) ⇌ 2 NH_3(g) + heat

If the concentration of ammonia is decreased, then [[1]] is favored because it [[7]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 produces nitrogen 2 consumes nitrogen 2 produces hydrogen 2 consumes hydrogen 2 produces ammonia 2 consumes ammonia 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 neither reaction 1 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the concentration of hydrogen is decreased, then [[2]] is favored because it [[7]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the temperature is increased, then [[2]] is favored because it [[10]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the temperature is decreased, then [[1]] is favored because it [[11]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the pressure is increased, then [[3]] is favored because it [[14]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the pressure is decreased, then [[3]] is favored because it [[14]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the concentration of HI is increased, then [[2]] is favored because it [[6]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the concentration of HI is decreased, then [[1]] is favored because it [[9]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the concentration of iodine is increased, then [[1]] is favored because it [[5]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the concentration of iodine is decreased, then [[2]] is favored because it [[8]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the equation for the synthesis of hydrogen iodide from hydrogen and iodine:

H_2(g) + I_2(g) ⇌ 2 HI_(g) + heat

If the concentration of hydrogen is increased, then [[1]] is favored because it [[4]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 consumes hydrogen 2 consumes iodine 2 consumes hydrogen iodide 2 produces hydrogen 2 produces iodine 2 produces hydrogen iodide 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the concentration of carbon is increased, then [[1]] is favored because it [[8]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the concentration of carbon is decreased, then [[2]] is favored because it [[4]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the concentration of water is increased, then [[1]] is favored because it [[9]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the concentration of water is decreased, then [[2]] is favored because it [[5]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the concentration of CO is increased, then [[2]] is favored because it [[10]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the concentration of CO is decreased, then [[1]] is favored because it [[6]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the concentration of hydrogen is increased, then [[2]] is favored because it [[11]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the concentration of hydrogen is decreased, then [[1]] is favored because it [[7]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the pressure is decreased, then [[1]] is favored because it [[14]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the pressure is increased, then [[2]] is favored because it [[15]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the temperature is decreased, then [[2]] is favored because it [[13]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 le chatelier Consider the following equation:

C_(s) + H₂O_(g) + heat ⇌ CO_(g) + H_2(g)

If the temperature is increased, then [[1]] is favored because it [[12]].

]]> 2.0000000 0.3333333 0 0 Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the forward reaction 1 the reverse reaction 1 neither reaction 1 produces carbon 2 produces water 2 produces CO 2 produces hydrogen 2 consumes carbon 2 consumes water 2 consumes CO 2 consumes hydrogen 2 absorbs heat 2 releases heat 2 increases the moles of gases 2 decreases the moles of gases 2 has no effect on the moles of gases 2 $course$/Chemistry Common Assessments/Semester 2/Quarter 4/Unit 9: Kinetics and Equilibrium/9C: equilibrium 1 A system at equilibrium is characterized by:

]]> 2.0000000 0.3333333 0 true true none Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> all the reactions stopping

]]> the forward and reverse reactions occurring at the same rate

]]> equal concentrations of reactants and products

]]> equal concentrations of all products

]]> rapid changes in concentration

]]> $course$/Chemistry Common Assessments/Semester 2/Quarter 4/Unit 9: Kinetics and Equilibrium/9B: variables affecting reaction rate 10 Why do gases react faster than liquids?

]]> 1.0000000 0.3333333 0 true true none Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> Gases have higher kinetic energy than liquids do

]]> Gases act as catalysts

]]> Activated complexes are usually gases

]]> Gases are more concentrated than liquids

]]> $course$/Chemistry Common Assessments/Semester 2/Quarter 4/Unit 9: Kinetics and Equilibrium/9C: equilibrium 2 Le Châtelier's principle states that

]]> 2.0000000 0.3333333 0 true true none Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> the reaction rate is proportional to the frequency of collisions between reactant molecules]]> all reactions will eventually go to completion]]> most reactions are reversible]]> when a system at equilibrium is subjected to a stress, it will respond in such a way as to counteract (undo) the stress]]> $course$/Chemistry Common Assessments/Semester 2/Quarter 4/Unit 9: Kinetics and Equilibrium/9B: variables affecting reaction rate 4 According to collision theory,

]]> 1.0000000 0.3333333 0 true true none Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> reactant particles must collide for the reaction to occur.

]]> every collision results in a reaction.

]]> the activated complex becomes the reactants.

]]> chemical reactions cause collisions.

]]> 8 At higher temperatures, reactant molecules would be expected to:

]]> 1.0000000 0.3333333 0 true true none Your answer is correct.

]]> Your answer is partially correct.

]]> Your answer is incorrect.

]]> collide with each other more often.

]]> decompose.

]]> form a catalyst.

]]> increase in activation energy.

]]>