Adapted by Nelson Nuñez-Rodriguez
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By David W. Ball
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| QUESTION | ANSWER |
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1. How many molecules of O2 will react with 6.022 × 1023 molecules of H2 to make water? The reaction is 2H2(g) + O2(g) → 2H2O(ℓ). |
1. 1.2044 × 1024 molecules |
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3. How many moles are present in 6.411 kg of CO2? How many molecules is this? |
3. 145.7 mol; 8.77 × 1025 molecules |
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5. What is the mass in milligrams of 7.22 × 1020 molecules of CO2?
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5. 52.8 mg
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7. What is the mass in grams of 1 molecule of H2O?
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7. 2.99 × 10−23 g
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9. What is the volume of 3.44 mol of Ga if the density of Ga is 6.08 g/mL? |
9. 39.4 mL
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11. For the chemical reaction 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(ℓ) assume that 13.4 g of C4H10 reacts completely to products. The density of CO2 is 1.96 g/L. What volume in liters of CO2 is produced? |
11. 20.7 L |
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13. Calculate the mass of each product when 100.0 g of CuCl react according to the reaction 2CuCl(aq) → CuCl2(aq) + Cu(s)
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13. 67.91 g of CuCl2; 32.09 g of Cu. The two masses add to 100.0 g, the initial amount of starting material, demonstrating the law of conservation of matter. |
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15. What mass of CO2 is produced from the combustion of 1 gal of gasoline? The chemical formula of gasoline can be approximated as C8H18. Assume that there are 2,801 g of gasoline per gallon. |
15. 8,632 g |
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17. A chemical reaction has a theoretical yield of 19.98 g and a percent yield of 88.40%. What is the actual yield? |
17. 17.66 g |
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19. Given the initial amounts listed, what is the limiting reagent, and how much of the other reactants are in excess?
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19. The limiting reagent is NaOH; 21.9 g of P4 and 3.61 g of H2O are left over. |
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21. Verify that it does not matter which product you use to predict the limiting reagent by using both products in this combustion reaction to determine the limiting reagent and the amount of the reactant in excess. Initial amounts of each reactant are given.
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21. Both products predict that O2 is the limiting reagent; 20.3 g of C3H8 are left over. |