$course$/Chemistry Common Assessments/Semester 2/Quarter 3/Unit 6: Stoichiometry/6A: stoichiometry problems stoic1 Use this balanced equation to solve the following problem:

2 H2O2 (aq) → 2 H2O (l) + O2 (g)

How many grams of oxygen gas is produced by the decomposition of {g} grams of H2O2?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {g}*.4703 0.01 1 1 3 0 0.1000000 3 0 private g calculated uniform 0.1 2 1 100 1 1.88 2 1.21 3 0.19 4 0.73 5 1.65 6 1.06 7 1.97 8 1.28 9 1.19 10 1.91 11 1.49 12 0.34 13 1.04 14 1.37 15 1.01 16 1.41 17 1.06 18 1.68 19 0.36 20 1.10 21 0.67 22 1.78 23 0.99 24 1.80 25 0.25 26 1.74 27 1.80 28 0.89 29 1.48 30 1.83 31 1.98 32 1.82 33 0.92 34 0.51 35 1.80 36 0.25 37 0.51 38 1.94 39 1.97 40 1.94 41 1.50 42 0.34 43 0.84 44 0.91 45 0.28 46 2.00 47 1.60 48 0.90 49 1.82 50 1.70 51 0.75 52 0.34 53 0.21 54 1.00 55 0.92 56 0.81 57 0.11 58 0.71 59 1.25 60 1.86 61 0.96 62 1.47 63 1.21 64 1.08 65 0.91 66 0.70 67 0.65 68 1.07 69 1.71 70 0.20 71 1.35 72 0.18 73 1.50 74 1.09 75 1.76 76 0.75 77 1.41 78 1.19 79 0.51 80 0.47 81 1.27 82 1.77 83 0.61 84 0.93 85 1.81 86 1.87 87 0.67 88 1.03 89 1.93 90 1.77 91 0.58 92 0.51 93 0.19 94 1.51 95 1.91 96 0.45 97 0.56 98 1.98 99 0.61 100 1.91 100 stoic10 Use this balanced equation to solve the following problem:

2 HCl (aq) + Mg (s) → MgCl2 (aq) + H2 (g)

How many liters (at STP) of hydrogen gas would be produced by the reaction of {g} grams of magnesium?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {g}*.9218 0.02 1 1 4 0 0.1000000 3 0 private g calculated uniform 1 5 2 100 1 1.88 2 1.21 3 0.19 4 0.73 5 1.65 6 1.06 7 1.97 8 1.28 9 1.19 10 1.91 11 1.49 12 0.34 13 1.04 14 1.37 15 1.01 16 1.41 17 1.06 18 1.68 19 0.36 20 1.10 21 0.67 22 1.78 23 0.99 24 1.80 25 0.25 26 1.74 27 1.80 28 0.89 29 1.48 30 1.83 31 1.98 32 1.82 33 0.92 34 0.51 35 1.80 36 0.25 37 0.51 38 1.94 39 1.97 40 1.94 41 1.50 42 0.34 43 0.84 44 0.91 45 0.28 46 2.00 47 1.60 48 0.90 49 1.82 50 1.70 51 0.75 52 0.34 53 0.21 54 1.00 55 0.92 56 0.81 57 0.11 58 0.71 59 1.25 60 1.86 61 0.96 62 1.47 63 1.21 64 1.08 65 0.91 66 0.70 67 0.65 68 1.07 69 1.71 70 0.20 71 1.35 72 0.18 73 1.50 74 1.09 75 1.76 76 0.75 77 1.41 78 1.19 79 0.51 80 0.47 81 1.27 82 1.77 83 0.61 84 0.93 85 1.81 86 1.87 87 0.67 88 1.03 89 1.93 90 1.77 91 0.58 92 0.51 93 0.19 94 1.51 95 1.91 96 0.45 97 0.56 98 1.98 99 0.61 100 1.91 100 stoic11 Use this balanced equation to solve the following problem:

2 HCl (aq) + Mg (s) → MgCl2 (aq) + H2 (g)

How many moles of hydrogen gas would be produced by the reaction of {mol} moles of hydrochloric acid (HCl)?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {mol}*.5 0.03 1 2 3 0 0.1000000 3 0 private mol calculated uniform 0.01 0.1 3 100 1 0.049 2 0.075 3 0.095 4 0.098 5 0.044 6 0.062 7 0.027 8 0.050 9 0.093 10 0.053 11 0.030 12 0.073 13 0.019 14 0.027 15 0.067 16 0.088 17 0.054 18 0.084 19 0.084 20 0.024 21 0.050 22 0.033 23 0.052 24 0.083 25 0.012 26 0.053 27 0.024 28 0.056 29 0.058 30 0.050 31 0.054 32 0.079 33 0.067 34 0.055 35 0.063 36 0.067 37 0.059 38 0.045 39 0.022 40 0.029 41 0.051 42 0.064 43 0.072 44 0.061 45 0.083 46 0.082 47 0.044 48 0.028 49 0.072 50 0.087 51 0.018 52 0.089 53 0.033 54 0.088 55 0.024 56 0.073 57 0.092 58 0.089 59 0.064 60 0.077 61 0.013 62 0.081 63 0.069 64 0.026 65 0.087 66 0.055 67 0.027 68 0.045 69 0.028 70 0.098 71 0.015 72 0.030 73 0.080 74 0.045 75 0.033 76 0.084 77 0.040 78 0.045 79 0.010 80 0.094 81 0.054 82 0.033 83 0.041 84 0.063 85 0.035 86 0.029 87 0.028 88 0.049 89 0.073 90 0.012 91 0.052 92 0.051 93 0.010 94 0.092 95 0.055 96 0.092 97 0.053 98 0.052 99 0.099 100 0.062 100 stoic12 Use this balanced equation to solve the following problem:

2 HCl (aq) + Mg (s) → MgCl2 (aq) + H2 (g)

How many liters (at STP) of hydrogen gas would be produced by the reaction of {mol} moles of hydrochloric acid (HCl)?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {mol}*11.2 0.01 2 1 2 0 0.1000000 3 0 private mol calculated uniform 0.01 0.1 3 100 1 0.049 2 0.075 3 0.095 4 0.098 5 0.044 6 0.062 7 0.027 8 0.050 9 0.093 10 0.053 11 0.030 12 0.073 13 0.019 14 0.027 15 0.067 16 0.088 17 0.054 18 0.084 19 0.084 20 0.024 21 0.050 22 0.033 23 0.052 24 0.083 25 0.012 26 0.053 27 0.024 28 0.056 29 0.058 30 0.050 31 0.054 32 0.079 33 0.067 34 0.055 35 0.063 36 0.067 37 0.059 38 0.045 39 0.022 40 0.029 41 0.051 42 0.064 43 0.072 44 0.061 45 0.083 46 0.082 47 0.044 48 0.028 49 0.072 50 0.087 51 0.018 52 0.089 53 0.033 54 0.088 55 0.024 56 0.073 57 0.092 58 0.089 59 0.064 60 0.077 61 0.013 62 0.081 63 0.069 64 0.026 65 0.087 66 0.055 67 0.027 68 0.045 69 0.028 70 0.098 71 0.015 72 0.030 73 0.080 74 0.045 75 0.033 76 0.084 77 0.040 78 0.045 79 0.010 80 0.094 81 0.054 82 0.033 83 0.041 84 0.063 85 0.035 86 0.029 87 0.028 88 0.049 89 0.073 90 0.012 91 0.052 92 0.051 93 0.010 94 0.092 95 0.055 96 0.092 97 0.053 98 0.052 99 0.099 100 0.062 100 stoic2 Use this balanced equation to solve the following problem:

2 H2O2 (aq) → 2 H2O (l) + O2 (g)

How many grams of water would be produced by the decomposition of {g} grams of H2O2?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {g}*.5297 0.01 1 1 3 0 0.1000000 3 0 private g calculated uniform 0.1 2 1 100 1 1.88 2 1.21 3 0.19 4 0.73 5 1.65 6 1.06 7 1.97 8 1.28 9 1.19 10 1.91 11 1.49 12 0.34 13 1.04 14 1.37 15 1.01 16 1.41 17 1.06 18 1.68 19 0.36 20 1.10 21 0.67 22 1.78 23 0.99 24 1.80 25 0.25 26 1.74 27 1.80 28 0.89 29 1.48 30 1.83 31 1.98 32 1.82 33 0.92 34 0.51 35 1.80 36 0.25 37 0.51 38 1.94 39 1.97 40 1.94 41 1.50 42 0.34 43 0.84 44 0.91 45 0.28 46 2.00 47 1.60 48 0.90 49 1.82 50 1.70 51 0.75 52 0.34 53 0.21 54 1.00 55 0.92 56 0.81 57 0.11 58 0.71 59 1.25 60 1.86 61 0.96 62 1.47 63 1.21 64 1.08 65 0.91 66 0.70 67 0.65 68 1.07 69 1.71 70 0.20 71 1.35 72 0.18 73 1.50 74 1.09 75 1.76 76 0.75 77 1.41 78 1.19 79 0.51 80 0.47 81 1.27 82 1.77 83 0.61 84 0.93 85 1.81 86 1.87 87 0.67 88 1.03 89 1.93 90 1.77 91 0.58 92 0.51 93 0.19 94 1.51 95 1.91 96 0.45 97 0.56 98 1.98 99 0.61 100 1.91 100 stoic3 Use this balanced equation to solve the following problem:

2 H2O2 (aq) → 2 H2O (l) + O2 (g)

How many liters (at STP) of oxygen gas would be produced by the decomposition of {g} grams of H2O2?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {g}*.329 0.01 1 1 3 0 0.1000000 3 0 private g calculated uniform 0.1 2 1 100 1 1.88 2 1.21 3 0.19 4 0.73 5 1.65 6 1.06 7 1.97 8 1.28 9 1.19 10 1.91 11 1.49 12 0.34 13 1.04 14 1.37 15 1.01 16 1.41 17 1.06 18 1.68 19 0.36 20 1.10 21 0.67 22 1.78 23 0.99 24 1.80 25 0.25 26 1.74 27 1.80 28 0.89 29 1.48 30 1.83 31 1.98 32 1.82 33 0.92 34 0.51 35 1.80 36 0.25 37 0.51 38 1.94 39 1.97 40 1.94 41 1.50 42 0.34 43 0.84 44 0.91 45 0.28 46 2.00 47 1.60 48 0.90 49 1.82 50 1.70 51 0.75 52 0.34 53 0.21 54 1.00 55 0.92 56 0.81 57 0.11 58 0.71 59 1.25 60 1.86 61 0.96 62 1.47 63 1.21 64 1.08 65 0.91 66 0.70 67 0.65 68 1.07 69 1.71 70 0.20 71 1.35 72 0.18 73 1.50 74 1.09 75 1.76 76 0.75 77 1.41 78 1.19 79 0.51 80 0.47 81 1.27 82 1.77 83 0.61 84 0.93 85 1.81 86 1.87 87 0.67 88 1.03 89 1.93 90 1.77 91 0.58 92 0.51 93 0.19 94 1.51 95 1.91 96 0.45 97 0.56 98 1.98 99 0.61 100 1.91 100 stoic4 Use this balanced equation to solve the following problem:

2 H2O2 (aq) → 2 H2O (l) + O2 (g)

How many grams of H2O2 are needed to produce {L} liters of oxygen gas at STP?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {L}*3.038 0.01 1 1 3 0 0.1000000 3 0 private L calculated uniform 1 10 1 100 1 4.6 2 9.3 3 5.3 4 8.5 5 5.6 6 7.5 7 7.2 8 8.4 9 2.5 10 8.8 11 1.9 12 7.7 13 7.5 14 4.7 15 9.7 16 9.1 17 3.3 18 1.3 19 8.8 20 3.7 21 2.8 22 3.6 23 1.8 24 2.2 25 8.1 26 2.0 27 8.6 28 4.6 29 3.7 30 7.5 31 5.1 32 9.6 33 6.1 34 8.1 35 2.5 36 2.7 37 4.4 38 4.5 39 7.2 40 3.2 41 1.3 42 1.1 43 7.6 44 7.0 45 6.5 46 1.4 47 8.6 48 3.1 49 6.3 50 4.6 51 3.6 52 7.5 53 6.7 54 3.0 55 1.0 56 6.8 57 4.3 58 7.3 59 8.3 60 9.9 61 7.2 62 7.2 63 6.0 64 3.7 65 7.9 66 4.7 67 9.6 68 4.4 69 9.0 70 4.2 71 9.4 72 1.5 73 6.2 74 2.7 75 7.9 76 5.6 77 3.9 78 7.7 79 1.9 80 8.1 81 10.0 82 6.2 83 1.6 84 3.4 85 7.8 86 6.8 87 5.4 88 5.8 89 7.6 90 7.3 91 1.9 92 4.1 93 2.8 94 7.5 95 7.3 96 9.9 97 1.6 98 3.7 99 9.2 100 5.7 100 stoic5 Use this balanced equation to solve the following problem:

2 HCl (aq) + CaCO3 (s) → CaCl2 (aq) + H2O (l) + CO2 (g)

How many grams of carbon dioxide gas would be produced by the reaction of {g} grams of CaCO3?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {g}*.4397 0.01 2 1 2 0 0.1000000 3 0 private g calculated uniform 0.1 2 2 100 1 1.88 2 1.21 3 0.19 4 0.73 5 1.65 6 1.06 7 1.97 8 1.28 9 1.19 10 1.91 11 1.49 12 0.34 13 1.04 14 1.37 15 1.01 16 1.41 17 1.06 18 1.68 19 0.36 20 1.10 21 0.67 22 1.78 23 0.99 24 1.80 25 0.25 26 1.74 27 1.80 28 0.89 29 1.48 30 1.83 31 1.98 32 1.82 33 0.92 34 0.51 35 1.80 36 0.25 37 0.51 38 1.94 39 1.97 40 1.94 41 1.50 42 0.34 43 0.84 44 0.91 45 0.28 46 2.00 47 1.60 48 0.90 49 1.82 50 1.70 51 0.75 52 0.34 53 0.21 54 1.00 55 0.92 56 0.81 57 0.11 58 0.71 59 1.25 60 1.86 61 0.96 62 1.47 63 1.21 64 1.08 65 0.91 66 0.70 67 0.65 68 1.07 69 1.71 70 0.20 71 1.35 72 0.18 73 1.50 74 1.09 75 1.76 76 0.75 77 1.41 78 1.19 79 0.51 80 0.47 81 1.27 82 1.77 83 0.61 84 0.93 85 1.81 86 1.87 87 0.67 88 1.03 89 1.93 90 1.77 91 0.58 92 0.51 93 0.19 94 1.51 95 1.91 96 0.45 97 0.56 98 1.98 99 0.61 100 1.91 100 stoic6 Use this balanced equation to solve the following problem:

2 HCl (aq) + CaCO3 (s) → CaCl2 (aq) + H2O (l) + CO2 (g)

How many moles of hydrochloric acid (HCl) would be needed to completely react with {g} grams of CaCO3?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {g}*.01998 0.01 1 1 5 0 0.1000000 3 0 private g calculated uniform 0.1 2 2 100 1 1.69 2 1.91 3 1.74 4 1.90 5 0.81 6 0.46 7 1.43 8 0.83 9 0.42 10 1.28 11 1.99 12 0.19 13 0.18 14 1.26 15 1.69 16 1.51 17 1.48 18 0.42 19 1.85 20 1.42 21 1.51 22 0.67 23 1.13 24 0.23 25 0.18 26 1.45 27 1.56 28 0.52 29 0.24 30 1.70 31 1.09 32 0.72 33 0.81 34 0.36 35 0.96 36 1.26 37 1.31 38 0.81 39 1.24 40 1.17 41 0.32 42 1.27 43 1.28 44 1.21 45 1.21 46 1.29 47 1.85 48 0.48 49 1.77 50 1.63 51 0.70 52 1.40 53 0.91 54 1.29 55 0.66 56 1.32 57 0.62 58 0.76 59 1.49 60 1.12 61 0.96 62 1.77 63 1.32 64 1.17 65 0.99 66 0.76 67 1.77 68 0.72 69 1.38 70 0.44 71 1.07 72 0.68 73 1.16 74 0.38 75 0.32 76 0.97 77 1.62 78 1.77 79 0.39 80 0.95 81 0.34 82 0.62 83 1.41 84 0.41 85 1.69 86 1.75 87 1.16 88 1.97 89 0.31 90 0.30 91 1.76 92 0.36 93 0.91 94 1.47 95 0.75 96 0.57 97 1.90 98 0.84 99 1.41 100 0.50 100 stoic7 Use this balanced equation to solve the following problem:

2 HCl (aq) + CaCO3 (s) → CaCl2 (aq) + H2O (l) + CO2 (g)

{mol} moles of HCl were needed to react completely with a sample of CaCO3. How many grams were in that sample?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {mol}*50.045 0.01 1 1 3 0 0.1000000 3 0 private mol calculated uniform 0.01 0.1 3 100 1 0.021 2 0.047 3 0.034 4 0.084 5 0.021 6 0.058 7 0.057 8 0.044 9 0.062 10 0.083 11 0.085 12 0.038 13 0.054 14 0.092 15 0.028 16 0.087 17 0.080 18 0.013 19 0.036 20 0.090 21 0.074 22 0.025 23 0.066 24 0.060 25 0.085 26 0.093 27 0.094 28 0.066 29 0.020 30 0.042 31 0.056 32 0.012 33 0.054 34 0.073 35 0.072 36 0.016 37 0.013 38 0.074 39 0.046 40 0.031 41 0.076 42 0.068 43 0.075 44 0.092 45 0.012 46 0.011 47 0.097 48 0.037 49 0.087 50 0.044 51 0.091 52 0.026 53 0.062 54 0.084 55 0.060 56 0.025 57 0.038 58 0.018 59 0.027 60 0.053 61 0.036 62 0.068 63 0.095 64 0.035 65 0.034 66 0.077 67 0.049 68 0.073 69 0.068 70 0.010 71 0.040 72 0.093 73 0.073 74 0.011 75 0.083 76 0.063 77 0.054 78 0.022 79 0.042 80 0.024 81 0.026 82 0.035 83 0.020 84 0.059 85 0.073 86 0.076 87 0.070 88 0.061 89 0.044 90 0.069 91 0.040 92 0.053 93 0.090 94 0.013 95 0.084 96 0.035 97 0.096 98 0.023 99 0.021 100 0.042 100 stoic8 Use this balanced equation to solve the following problem:

2 HCl (aq) + CaCO3 (s) → CaCl2 (aq) + H2O (l) + CO2 (g)

How many grams of CaCO3 would be needed to produce {L} liters of carbon dioxide (at STP)?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {L}*4.468 0.01 1 1 2 0 0.1000000 3 0 private L calculated uniform 1 10 2 100 1 7.86 2 6.61 3 4.62 4 3.21 5 9.85 6 7.18 7 3.78 8 4.03 9 3.99 10 5.31 11 2.71 12 1.77 13 2.21 14 5.13 15 3.48 16 7.28 17 7.03 18 8.90 19 5.42 20 3.91 21 9.53 22 5.24 23 6.72 24 6.01 25 1.43 26 6.72 27 2.99 28 8.06 29 5.83 30 8.98 31 2.68 32 9.85 33 4.22 34 4.10 35 9.51 36 3.17 37 9.36 38 3.85 39 5.97 40 1.15 41 4.19 42 2.19 43 7.67 44 8.88 45 8.34 46 8.45 47 4.21 48 3.96 49 2.90 50 2.41 51 9.75 52 7.31 53 6.61 54 8.38 55 4.80 56 4.47 57 7.96 58 2.48 59 1.12 60 8.70 61 7.68 62 4.35 63 2.38 64 9.92 65 8.22 66 4.80 67 2.38 68 1.83 69 8.33 70 5.59 71 7.03 72 3.01 73 5.83 74 9.46 75 1.27 76 6.09 77 2.57 78 4.97 79 3.99 80 6.44 81 4.33 82 1.74 83 2.99 84 9.40 85 7.33 86 8.37 87 7.39 88 2.43 89 3.39 90 4.51 91 3.54 92 2.67 93 2.41 94 3.89 95 6.51 96 1.31 97 1.07 98 2.87 99 6.60 100 2.05 100 stoic9 Use this balanced equation to solve the following problem:

2 HCl (aq) + Mg (s) → MgCl2 (aq) + H2 (g)

How many grams of hydrogen gas would be produced by the reaction of {g} grams of magnesium?

Do not include units in your answer.

]]> 2.0000000 0.3333333 0 0 0 abc 1 {g}*.0833 0.03 1 1 4 0 0.1000000 3 0 private g calculated uniform 1 5 2 100 1 1.88 2 1.21 3 0.19 4 0.73 5 1.65 6 1.06 7 1.97 8 1.28 9 1.19 10 1.91 11 1.49 12 0.34 13 1.04 14 1.37 15 1.01 16 1.41 17 1.06 18 1.68 19 0.36 20 1.10 21 0.67 22 1.78 23 0.99 24 1.80 25 0.25 26 1.74 27 1.80 28 0.89 29 1.48 30 1.83 31 1.98 32 1.82 33 0.92 34 0.51 35 1.80 36 0.25 37 0.51 38 1.94 39 1.97 40 1.94 41 1.50 42 0.34 43 0.84 44 0.91 45 0.28 46 2.00 47 1.60 48 0.90 49 1.82 50 1.70 51 0.75 52 0.34 53 0.21 54 1.00 55 0.92 56 0.81 57 0.11 58 0.71 59 1.25 60 1.86 61 0.96 62 1.47 63 1.21 64 1.08 65 0.91 66 0.70 67 0.65 68 1.07 69 1.71 70 0.20 71 1.35 72 0.18 73 1.50 74 1.09 75 1.76 76 0.75 77 1.41 78 1.19 79 0.51 80 0.47 81 1.27 82 1.77 83 0.61 84 0.93 85 1.81 86 1.87 87 0.67 88 1.03 89 1.93 90 1.77 91 0.58 92 0.51 93 0.19 94 1.51 95 1.91 96 0.45 97 0.56 98 1.98 99 0.61 100 1.91 100 $course$/Chemistry Common Assessments/Semester 2/Quarter 3/Unit 6: Stoichiometry/6C: percent yield yield1

Use this balanced equation to solve the following problem:

NH4NO3 (s) → N2O (g) + 2 H2O (g) 

{an} grams of ammonium nitrate are decomposed. If the reaction actually produces {w} grams of water vapor, what is the percent yield?

(Do not type a percent sign with your answer.)


]]> 2.0000000 0.3333333 0 0 0 abc 1 100*{w}/(({an}/80.04)*2*18.02) 0.01 1 1 2 0 0.1000000 3 0 private w calculated uniform 2 4 2 100 1 3.95 2 3.26 3 2.55 4 2.33 5 3.25 6 2.90 7 4.00 8 2.68 9 2.49 10 2.24 11 3.61 12 2.98 13 3.30 14 3.40 15 3.36 16 2.44 17 2.97 18 3.87 19 3.84 20 2.57 21 2.66 22 3.55 23 2.18 24 3.77 25 2.00 26 3.67 27 3.85 28 2.99 29 2.13 30 3.66 31 2.30 32 2.62 33 2.16 34 2.34 35 2.09 36 3.26 37 3.49 38 2.30 39 3.31 40 3.89 41 3.68 42 3.07 43 3.14 44 2.13 45 3.63 46 2.41 47 2.58 48 2.61 49 2.83 50 2.68 51 2.73 52 3.98 53 3.27 54 2.89 55 3.22 56 3.75 57 3.97 58 3.08 59 2.31 60 2.94 61 3.88 62 3.34 63 3.96 64 2.58 65 3.36 66 3.45 67 2.66 68 3.05 69 3.03 70 2.43 71 3.76 72 3.76 73 3.73 74 2.36 75 3.52 76 2.69 77 2.68 78 2.63 79 3.10 80 3.39 81 3.84 82 2.49 83 2.52 84 3.27 85 2.24 86 2.78 87 3.77 88 3.29 89 3.08 90 3.82 91 3.62 92 2.25 93 2.26 94 2.07 95 3.80 96 3.42 97 2.73 98 2.12 99 3.49 100 3.80 100 private an calculated uniform 8 10 2 100 1 8.08 2 8.03 3 8.45 4 8.87 5 8.51 6 8.05 7 9.48 8 8.83 9 8.71 10 8.35 11 9.97 12 8.56 13 9.37 14 8.70 15 8.44 16 9.30 17 9.07 18 9.26 19 8.79 20 9.59 21 8.45 22 9.57 23 8.48 24 9.29 25 8.67 26 8.09 27 8.53 28 9.88 29 8.29 30 9.93 31 9.17 32 8.76 33 9.74 34 9.32 35 9.76 36 9.22 37 8.85 38 9.31 39 9.03 40 9.51 41 9.04 42 8.92 43 9.36 44 9.94 45 9.43 46 9.32 47 9.63 48 8.64 49 8.67 50 9.09 51 8.69 52 9.91 53 8.61 54 8.78 55 9.09 56 9.87 57 8.42 58 9.26 59 8.02 60 9.98 61 9.49 62 9.52 63 9.15 64 9.16 65 8.36 66 8.53 67 9.73 68 8.61 69 8.63 70 8.45 71 8.15 72 8.53 73 9.84 74 8.27 75 8.26 76 9.66 77 8.63 78 9.62 79 8.30 80 9.51 81 9.43 82 8.80 83 9.51 84 9.77 85 9.64 86 9.45 87 8.81 88 9.09 89 8.65 90 8.07 91 8.93 92 9.08 93 8.46 94 9.38 95 9.85 96 9.12 97 9.44 98 8.64 99 8.15 100 8.30 100 yield2

Use this balanced equation to solve the following problem:

Ba(OH)2 (s) + 2 NH4Cl (s) → 2 NH3 (g) + 2 H2O (g) + BaCl2 (aq)

{b} grams of barium hydroxide react with an excess of ammonium chloride. If the reaction actually produces {a} grams of NH3, what is the percent yield?

(Do not type a percent sign with your answer.)

]]> 2.0000000 0.3333333 0 0 0 abc 1 100*{a}/(({b}/171.34)*2*17.03) 0.01 1 1 2 0 0.1000000 3 0 private a calculated uniform 3 4 2 100 1 3.63 2 3.77 3 3.15 4 3.66 5 3.77 6 3.58 7 3.18 8 3.68 9 3.53 10 3.17 11 3.22 12 3.92 13 3.93 14 3.98 15 3.45 16 3.79 17 3.44 18 3.03 19 3.44 20 3.97 21 3.37 22 3.66 23 3.62 24 3.94 25 3.37 26 3.49 27 3.29 28 3.21 29 3.87 30 3.54 31 3.82 32 3.33 33 3.24 34 3.75 35 3.04 36 3.46 37 3.22 38 3.90 39 3.33 40 3.53 41 3.46 42 3.05 43 3.98 44 3.25 45 3.74 46 3.78 47 3.09 48 3.26 49 3.75 50 3.73 51 3.22 52 3.25 53 3.10 54 3.40 55 3.50 56 3.89 57 3.18 58 3.02 59 3.89 60 3.27 61 3.81 62 3.79 63 3.80 64 3.86 65 3.65 66 3.35 67 3.73 68 3.82 69 3.76 70 3.28 71 3.13 72 3.97 73 3.82 74 3.36 75 3.69 76 3.46 77 3.08 78 3.34 79 3.88 80 3.56 81 3.73 82 3.44 83 3.12 84 3.09 85 3.46 86 3.12 87 3.09 88 3.08 89 3.63 90 3.81 91 3.34 92 3.39 93 3.94 94 3.65 95 3.06 96 3.94 97 3.53 98 3.12 99 3.25 100 3.73 100 private b calculated uniform 20 25 2 100 1 19.63 2 19.94 3 17.13 4 19.88 5 17.58 6 17.13 7 19.60 8 17.50 9 16.29 10 19.96 11 19.70 12 17.30 13 19.39 14 17.04 15 17.09 16 18.60 17 16.36 18 18.35 19 17.07 20 19.30 21 16.96 22 16.17 23 17.69 24 19.49 25 17.06 26 16.57 27 16.46 28 16.63 29 19.35 30 19.44 31 17.23 32 19.77 33 19.63 34 17.82 35 16.84 36 19.06 37 19.99 38 19.89 39 19.13 40 16.35 41 19.85 42 19.85 43 17.42 44 17.41 45 18.12 46 18.38 47 16.47 48 16.87 49 16.46 50 18.32 51 16.40 52 19.18 53 17.88 54 17.62 55 19.38 56 19.40 57 17.54 58 16.49 59 17.31 60 16.24 61 16.27 62 16.95 63 17.87 64 18.30 65 19.78 66 19.13 67 16.88 68 17.06 69 17.59 70 17.10 71 16.87 72 17.23 73 16.39 74 17.55 75 18.78 76 18.62 77 17.14 78 17.28 79 16.21 80 18.11 81 16.22 82 16.63 83 16.47 84 18.52 85 17.24 86 16.82 87 18.16 88 18.39 89 18.13 90 19.25 91 16.88 92 16.22 93 16.69 94 18.08 95 17.76 96 19.79 97 19.64 98 19.75 99 18.31 100 16.80 100 $course$/Chemistry Common Assessments/Semester 2/Quarter 3/Unit 6: Stoichiometry/6B: limiting reagent limiting1 Use this balanced equation to solve the following problem:

Na2CO3 (s) + 2 HCl (aq) → H2O (l) + CO2 (g) + 2 NaCl (aq)

{g} grams of sodium carbonate are added to {mol} moles of hydrochloric acid. How many grams of carbon dioxide will be produced? What is the limiting reactant?

]]> 4.0000000 0.3333333 0 0 0 none 1 Your answer is correct. Your answer is partially correct. Your answer is incorrect. hydrochloric acid is limiting 0.01 1 1 2 sodium carbonate is limiting 0.01 1 1 2 both reactants are limiting 0.01 1 1 2 there is no limiting reactant 0.01 1 1 2 {=({mol}/2)*44.01} g carbon dioxide 0.01 1 1 2 {=({mol})*44.01} g carbon dioxide 0.01 1 1 2 {=({g}/105.99)*44.01} g carbon dioxide 0.01 1 1 2 {=({g}/53)*44.01} g carbon dioxide 0.01 1 1 2 {=({g}/300)*44.01} g carbon dioxide 0.01 1 1 2 {={g}*{mol}} g carbon dioxide 0.01 1 1 2 {={mol}*7.7} g carbon dioxide 0.01 1 1 2 private mol calculatedsimple uniform 0.01 0.099 3 100 1 0.052 2 0.045 3 0.093 4 0.084 5 0.033 6 0.016 7 0.071 8 0.065 9 0.060 10 0.025 11 0.063 12 0.021 13 0.085 14 0.022 15 0.041 16 0.035 17 0.063 18 0.035 19 0.028 20 0.015 21 0.076 22 0.069 23 0.070 24 0.037 25 0.014 26 0.082 27 0.028 28 0.030 29 0.060 30 0.089 31 0.091 32 0.039 33 0.046 34 0.092 35 0.089 36 0.051 37 0.021 38 0.021 39 0.015 40 0.043 41 0.022 42 0.010 43 0.011 44 0.077 45 0.074 46 0.031 47 0.065 48 0.024 49 0.064 50 0.073 51 0.052 52 0.064 53 0.045 54 0.074 55 0.043 56 0.092 57 0.031 58 0.037 59 0.041 60 0.096 61 0.045 62 0.042 63 0.091 64 0.032 65 0.021 66 0.053 67 0.081 68 0.065 69 0.092 70 0.090 71 0.073 72 0.056 73 0.083 74 0.086 75 0.064 76 0.050 77 0.062 78 0.066 79 0.046 80 0.017 81 0.089 82 0.062 83 0.025 84 0.075 85 0.011 86 0.015 87 0.081 88 0.015 89 0.069 90 0.026 91 0.057 92 0.060 93 0.057 94 0.071 95 0.096 96 0.071 97 0.045 98 0.059 99 0.022 100 0.025 100 private g calculatedsimple uniform 5.23 9.53 2 100 1 8.95 2 7.87 3 9.22 4 6.73 5 9.18 6 5.24 7 6.45 8 6.22 9 7.25 10 5.46 11 8.96 12 8.28 13 5.86 14 8.67 15 9.00 16 6.59 17 6.08 18 7.47 19 5.26 20 6.21 21 7.12 22 9.27 23 7.01 24 7.82 25 9.46 26 8.50 27 6.74 28 6.15 29 7.32 30 5.72 31 7.27 32 5.68 33 8.52 34 6.40 35 6.01 36 7.45 37 6.63 38 7.75 39 7.29 40 5.96 41 7.99 42 8.67 43 7.22 44 7.56 45 8.62 46 6.40 47 6.21 48 9.35 49 7.21 50 8.97 51 6.13 52 5.48 53 5.98 54 7.37 55 7.80 56 6.27 57 6.28 58 5.90 59 8.29 60 8.86 61 8.72 62 6.72 63 9.24 64 8.21 65 7.05 66 6.91 67 9.00 68 9.13 69 7.75 70 6.55 71 6.95 72 5.82 73 8.00 74 8.09 75 7.53 76 8.58 77 6.99 78 6.14 79 6.28 80 5.80 81 9.15 82 8.94 83 5.44 84 6.37 85 7.03 86 8.13 87 8.37 88 9.53 89 9.18 90 8.34 91 5.66 92 8.20 93 7.17 94 6.47 95 5.60 96 6.08 97 8.71 98 7.85 99 6.63 100 6.49 100 limiting2 Use this balanced equation to solve the following problem:

Na2CO3 (s) + 2 HCl (aq) → H2O (l) + CO2 (g) + 2 NaCl (aq)

{g} grams of sodium carbonate are added to {mol} moles of hydrochloric acid. How many grams of carbon dioxide will be produced? What is the limiting reactant?

]]> 4.0000000 0.3333333 0 0 0 none 1 Your answer is correct. Your answer is partially correct. Your answer is incorrect. hydrochloric acid is limiting 0.01 1 1 2 sodium carbonate is limiting 0.01 1 1 2 both reactants are limiting 0.01 1 1 2 there is no limiting reactant 0.01 1 1 2 {=({mol}/2)*44.01} g carbon dioxide 0.01 1 1 2 {=({mol})*44.01} g carbon dioxide 0.01 1 1 2 {=({g}/105.99)*44.01} g carbon dioxide 0.01 1 1 2 {=({g}/53)*44.01} g carbon dioxide 0.01 1 1 2 {=({g}/300)*44.01} g carbon dioxide 0.01 1 1 2 {={g}*{mol}} g carbon dioxide 0.01 1 1 2 {={mol}*105.99} g carbon dioxide 0.01 1 1 2 private mol calculatedsimple uniform 0.01 0.099 3 100 1 0.090 2 0.054 3 0.044 4 0.082 5 0.066 6 0.024 7 0.096 8 0.099 9 0.093 10 0.032 11 0.013 12 0.070 13 0.055 14 0.077 15 0.046 16 0.094 17 0.042 18 0.011 19 0.083 20 0.070 21 0.057 22 0.025 23 0.012 24 0.096 25 0.064 26 0.063 27 0.079 28 0.082 29 0.083 30 0.035 31 0.022 32 0.058 33 0.048 34 0.072 35 0.079 36 0.088 37 0.024 38 0.094 39 0.098 40 0.073 41 0.081 42 0.055 43 0.078 44 0.031 45 0.047 46 0.036 47 0.043 48 0.098 49 0.032 50 0.056 51 0.058 52 0.043 53 0.068 54 0.047 55 0.032 56 0.070 57 0.012 58 0.085 59 0.043 60 0.021 61 0.053 62 0.037 63 0.087 64 0.091 65 0.033 66 0.051 67 0.093 68 0.098 69 0.013 70 0.071 71 0.090 72 0.018 73 0.050 74 0.020 75 0.037 76 0.033 77 0.016 78 0.061 79 0.070 80 0.039 81 0.054 82 0.033 83 0.037 84 0.086 85 0.025 86 0.060 87 0.039 88 0.044 89 0.016 90 0.055 91 0.018 92 0.071 93 0.015 94 0.097 95 0.075 96 0.096 97 0.047 98 0.036 99 0.065 100 0.036 100 private g calculatedsimple uniform 0.11 0.52 2 100 1 0.24 2 0.48 3 0.31 4 0.35 5 0.44 6 0.22 7 0.52 8 0.49 9 0.14 10 0.15 11 0.47 12 0.19 13 0.29 14 0.39 15 0.21 16 0.37 17 0.25 18 0.43 19 0.24 20 0.41 21 0.48 22 0.23 23 0.51 24 0.19 25 0.46 26 0.48 27 0.42 28 0.22 29 0.42 30 0.48 31 0.26 32 0.21 33 0.48 34 0.48 35 0.24 36 0.31 37 0.33 38 0.44 39 0.45 40 0.49 41 0.19 42 0.12 43 0.23 44 0.38 45 0.43 46 0.24 47 0.41 48 0.18 49 0.38 50 0.17 51 0.17 52 0.47 53 0.17 54 0.32 55 0.29 56 0.47 57 0.39 58 0.19 59 0.24 60 0.47 61 0.33 62 0.32 63 0.41 64 0.49 65 0.27 66 0.39 67 0.50 68 0.40 69 0.52 70 0.40 71 0.16 72 0.48 73 0.23 74 0.49 75 0.27 76 0.40 77 0.43 78 0.36 79 0.32 80 0.50 81 0.50 82 0.22 83 0.21 84 0.29 85 0.22 86 0.50 87 0.52 88 0.12 89 0.26 90 0.37 91 0.26 92 0.30 93 0.18 94 0.28 95 0.39 96 0.34 97 0.46 98 0.12 99 0.48 100 0.23 100