(Solved): 1. How many moles are present in 100.0g of sulfur dioxide? A) 1.561 B) 0.6406 C) 64.06 D) 2.083 2 ...

1. How many moles are present in $$100.0\mathrm{g}$$ of sulfur dioxide? A) $$1.561$$ B) $$0.6406$$ C) $$64.06$$ D) $$2.083$$ 2. What is the mass of $$3.612$$ moles of $$\mathrm{HCl}$$ ? A) $$0.09907\mathrm{g}$$ B) $$131.7\mathrm{g}$$ C) $$202.2\mathrm{g}$$ D) $$3.612\mathrm{g}$$ 3. How many molecules are present in $$1.60$$ moles of water? A) $$9.63\times 10^{23}$$ B) $$9.63\times 10^{24}$$ C) $$3.75\times 10^{23}$$ D) $$3.75\times 10^{24}$$ 4. How many moles are present in $$1.40\times 10^{22}$$ molecules of carbon monoxide? A) $$43.0$$ B) $$0.0233$$ C) $$8.43\times 10^{45}$$ D) $$8.43\times 10^{47}$$ 5. What is the mass of $$1.60\times 10^{23}$$ molecules of $$\mathrm{HCl}$$ ? A) $$9.69\mathrm{g}$$ B) $$137\mathrm{g}$$ C) $$0.729\mathrm{g}$$ D) $$36.5\mathrm{g}$$ 6. How many molecules are present in $$56.0\mathrm{g}$$ of $${\mathrm{MgSO}}_4$$ ? A) $$2.80\times 10^{23}$$ B) $$2.80\times 10^{24}$$ C) $$1.29\times 10^{24}$$ D) $$1.29\times 10^{25}$$ 7. How many moles of HF will be produced by the complete reaction of $$1.42$$ moles of $${\mathrm{H}}_2$$ in the following equation? $${\mathrm{H}}_2+{\mathrm{F}}_2?2\mathrm{HF}$$ A) $$0.710$$ B) $$1.42$$ C) $$2.00$$ D) $$2.84$$ 8. How many moles of $${\mathrm{N}}_2$$ will be consumed when $$1.60$$ moles of $${\mathrm{H}}_2$$ react completely in the following equation? $${\mathrm{N}}_2+3{\mathrm{H}}_2?2{\mathrm{NH}}_3$$ A) $$0.533$$ B) $$1.60$$ C) $$3.20$$ D) $$4.80$$ 9. How many moles of $${\mathrm{Cl}}_2$$ are consumed when $$0.500$$ moles of $${\mathrm{AlCl}}_1$$ are produced in the following equation? $$2\mathrm{Al}+3{\mathrm{Cl}}_2?2{\mathrm{AlCl}}_3$$ A) $$0.333$$ B) $$0.500$$ C) $$0.750$$ D) $$1.00$$ 10. How many moles of $${\mathrm{CO}}_2$$ are produced when $$3.01\times 10^{23}$$ molecules of $${\mathrm{C}}_3{\mathrm{H}}_6$$ react completely in the following equation? $$2{\mathrm{C}}_3{\mathrm{H}}_6+9{\mathrm{O}}_2?6{\mathrm{CO}}_2+6{\mathrm{H}}_2\mathrm{O}$$ A) $$0.167$$ B) $$1.50$$ C) $$1.51\times 10^{23}$$ D) $$2.01\times 10^{23}$$ 11. How many moles of $${\mathrm{H}}_2\mathrm{O}$$ are produced when $$1.60\times 10^{22}$$ molecules of $${\mathrm{O}}_2$$ react completely in the following equation? $$2{\mathrm{C}}_2{\mathrm{H}}_2+5{\mathrm{O}}_2?4{\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}$$ A) 0,0106 B) $$0.0664$$ C) $$2.41\times 10^{23}$$ D) $$1.51\times 10^{24}$$ 12. How many moles of $$\mathrm{HOH}$$ are produced when $$1.12\mathrm{X}10^{2\mathrm{x}}$$ molecule of $${\mathrm{H}}_3{\mathrm{PO}}_4$$ are consumed in the following equation? $$3\mathrm{Ca}(\mathrm{OH}{)}_2+2{\mathrm{H}}_3{\mathrm{PO}}_4?{\mathrm{Ca}}_3{\left({\mathrm{PO}}_4\right)}_2+6\mathrm{HOH}$$ A) $$0.0620$$ B) $$0.558$$ C) $$0.667$$ D) $$3.00$$ 13. How many molecules of $${\mathrm{NH}}_3$$ are produced when $$3.00$$ moles of $${\mathrm{H}}_2$$ react completely in the following equation? $${\mathrm{N}}_2+3{\mathrm{H}}_2?2{\mathrm{NH}}_3$$ A) $$0.667$$ B) $$1.50$$ C) $$1.20\times 10^{24}$$ D) $$2.71\times 10^{24}$$ 14. How many molecules of water are produced when $$3.00$$ moles of copper react completely in the following equation? $$\mathrm{Cu}+2{\mathrm{H}}_2{\mathrm{SO}}_4?{\mathrm{CuSO}}_4+2{\mathrm{H}}_2\mathrm{O}+{\mathrm{SO}}_2$$ A) $$9.03\times 10^{23}$$ B) $$3.61\times 10^{24}$$ C) $$1.20\times 10^{24}$$ D) $$2.71\times 10^{24}$$ 15. How many molecules of chlorine are produced when $$2.00$$ moles of carbon react completely in the following equation? $$\mathrm{C}+2{\mathrm{Cl}}_2?{\mathrm{CCl}}_4$$ A) $$3.01\times 10^{23}$$ B) $$6.02\times 10^{23}$$ C) $$1.20\times 10^{24}$$ D) $$2.41\times 10^{24}$$ 16. What mass of $$\mathrm{HCl}$$ is produced when $$3.00$$ moles of $${\mathrm{H}}_2$$ react completely in the following equation? $${\mathrm{H}}_2+{\mathrm{Cl}}_2?2\mathrm{HCl}$$ A) $$54.7\mathrm{g}$$ B) $$72.9\mathrm{g}$$ C) $$109\mathrm{g}$$ D) $$219\mathrm{g}$$ 17. What mass of carbon monoxide is produced when $$1.50$$ moles of oxygen react completely in the following equation? $$2\mathrm{C}+{\mathrm{O}}_2?2\mathrm{CO}$$ A) $$84.0\mathrm{g}$$ B) $$42.0\mathrm{g}$$ C) $$28.0\mathrm{g}$$ D) $$21.0\mathrm{g}$$ 18. What mass of carbon dioxide is produced when $$3.00$$ moles of oxygen react completely in the following equation? $$2\mathrm{CO}+{\mathrm{O}}_2?2{\mathrm{CO}}_2$$ A) $$88.0\mathrm{g}$$ B) $$44.0\mathrm{g}$$ C) $$29.3\mathrm{g}$$ D) $$264\mathrm{g}$$ 15. How many molecules of chlorine are produced when $$2.00$$ moles of carbon react completely in the following equation? $$\mathrm{C}+2{\mathrm{Cl}}_2?{\mathrm{CCl}}_4$$ A) $$3.01\times 10^{23}$$ B) $$6.02\times 10^{23}$$ C) $$1.20\times 10^{24}$$ D) $$2.41\times 10^{24}$$ 16. What mass of $$\mathrm{HCl}$$ is produced when $$3.00$$ moles of $${\mathrm{H}}_2$$ react completely in the following equation? $${\mathrm{H}}_2+{\mathrm{Cl}}_2?2\mathrm{HCl}$$ A) $$54.7\mathrm{g}$$ B) $$72.9\mathrm{g}$$ C) $$109\mathrm{g}$$ D) $$219\mathrm{g}$$ 17. What mass of carbon monoxide is produced when $$1.50$$ moles of oxygen react completely in the following equation? $$2\mathrm{C}+{\mathrm{O}}_2?2\mathrm{CO}$$ A) $$84.0\mathrm{g}$$ B) $$42.0\mathrm{g}$$ C) $$28.0\mathrm{g}$$ D) $$21.0\mathrm{g}$$ 18. What mass of carbon dioxide is produced when $$3.00$$ moles of oxygen react completely in the following equation? $$2\mathrm{CO}+{\mathrm{O}}_2?2{\mathrm{CO}}_2$$ A) $$88.0\mathrm{g}$$ B) $$44.0\mathrm{g}$$ C) $$29.3\mathrm{g}$$ D) $$264\mathrm{g}$$ 19. How many moles of carbon monoxide are produced when $$40.0\mathrm{g}$$ of oxygen react completely in the following equation? $$2\mathrm{C}+{\mathrm{O}}_2?2\mathrm{CO}$$ A) $$0.625$$ B) $$1.25$$ C) $$2.50$$ D) $$80.0$$ 20. How many moles of $${\mathrm{N}}_2{\mathrm{O}}_5$$ are produced when $$3,00\mathrm{g}$$ of $${\mathrm{O}}_2$$ react completely in the following equation? $$2{\mathrm{N}}_2+5{\mathrm{O}}_2?2{\mathrm{N}}_2{\mathrm{O}}_5$$ A) $$0.0375$$ B) $$0.0750$$ C) $$0.234$$ D) $$0.469$$ 21. How many moles of $${\mathrm{K}}_2\mathrm{S}$$ are consumed when $$14.0\mathrm{g}$$ of $$\mathrm{KBr}$$ react completely in the following equation? $${\mathrm{FeBr}}_2+{\mathrm{K}}_2\mathrm{S}?2\mathrm{KBr}+\mathrm{FeS}$$ A) $$0.0588$$ B) $$0.235$$ C) $$4.25$$ D) $$17.0$$ 22. What mass of $${\mathrm{CO}}_2$$ is produced when $$50.0\mathrm{g}$$ of $${\mathrm{C}}_2{\mathrm{H}}_4$$ reacts completely in the following equation? $${\mathrm{C}}_2{\mathrm{H}}_4+3{\mathrm{O}}_2?2{\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}$$ A) $$12.3\mathrm{g}$$ B) $$39.2\mathrm{g}$$ C) $$49.4\mathrm{g}$$ D) $$157\mathrm{g}$$ 23. What mass of $${\mathrm{H}}_2\mathrm{O}$$ is produced when $$12.0\mathrm{g}$$ of $$\mathrm{HCl}$$ react completely in the following equation? $$6\mathrm{HCl}+{\mathrm{Fe}}_2{\mathrm{O}}_3?2{\mathrm{FeCl}}_3+3{\mathrm{H}}_2\mathrm{O}$$ A) $$2.97\mathrm{g}$$ B) $$39.4\mathrm{g}$$ C) $$27.4\mathrm{g}$$ D) 110.g 24. What mass of $${\mathrm{H}}_2\mathrm{O}$$ is produced when $$60.0\mathrm{g}$$ of $${\mathrm{CH}}_4$$ reacts completely in the following. equation? $${\mathrm{CH}}_4+2{\mathrm{O}}_2?{\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}$$ A) $$2.41\mathrm{g}$$ B) $$9.64\mathrm{g}$$ C) $$33.7\mathrm{g}$$ D) $$135\mathrm{g}$$ 25. Which is the limiting reactant when $$12.0$$ moles of $${\mathrm{CH}}_t$$ are reacted with $$20.0$$ moles of $${\mathrm{O}}_2$$ in the following equation? $${\mathrm{CH}}_4+2{\mathrm{O}}_2?{\mathrm{CO}}_2+2{\mathrm{H}}_2\mathrm{O}$$ A) $${\mathrm{CH}}_4$$ B) $${\mathrm{O}}_2$$ C) $${\mathrm{CO}}_2$$ D) $${\mathrm{H}}_2\mathrm{O}$$ 26. Which is the limiting reactant when $$3.00$$ moles of copper are reacted with $$3.00$$ moles of silver nitrate in the following equation? $$\mathrm{Cu}+2{\mathrm{AgNO}}_3?\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2+2\mathrm{Ag}$$ A) $$\mathrm{Cu}$$ B) $${\mathrm{AgNO}}_3$$ C) $$\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2$$ D) $$\mathrm{Ag}$$ 27. Which substance is in excess when $$6.00$$ moles of aluminum are reacted with $$12.00$$ moles of oxygen in the following equation? $$4\mathrm{Al}+3{\mathrm{O}}_2?2{\mathrm{Al}}_2{\mathrm{O}}_3$$ A) $$\mathrm{Al}$$ B) $${\mathrm{O}}_2$$ C). $${\mathrm{Al}}_2{\mathrm{O}}_3$$ 28. In a reaction to produce sulfuric acid, the theoretical yield is $$300\mathrm{g}$$. What is the percent yield if the actual yield is $$280.\mathrm{g}$$ ? A) $$6.67\%$$ B) $$7.14\%$$ C) $$93.3\%$$ D) $$107\%$$ 29. In a reaction to produce iron the theoretical yield is $$340\mathrm{kg}$$. What is the percent yield if the actual yield is $$300,\mathrm{kg}$$ ? A) $$13.3\%$$ B) $$88.2\%$$ (C) $$11.8\%$$ D) $$113\%$$ 30. Dinitrogen tetroxide can be decomposed to form nitrogen dioxide. A. Write a balanced chemical equation for this reaction. B. What is the mass, in grams, of dinitrogen tetroxide needed to produce $$1.000\mathrm{kg}$$ of nitrogen dioxide? 31. When limestone (calcium carbonate) is heated it decomposes to form lime (calcium oxide) and carbon dioxide. A. Write a balanced chemical equation for this reaction. B. What mass of lime will be produced from the complete decomposition of $$100.\mathrm{g}$$ of limestone? C. What mass of carbon dioxide will be produced from the complete decomposition of 100.g of limestone? 32. The pollutant nitrogen monoxide can be reacted with ammonia to produce nitrogen gas and water. A. Write a balanced chemical equation for this reaction. B. In this equation, write the mole ratio of 1) Nitrogen monoxide to ammonia 2) Nitrogen monoxide to nitrogen gas 3) Nitrogen monoxide to water 4) Ammonia to nitrogen gas 5) Ammonia to water 6) Nitrogen gas to water 33. Nitrogen gas combines with hydrogen gas to produce ammonia. $$40.0\mathrm{g}$$ of nitrogen is reacted with $$10.0\mathrm{g}$$ of hydrogen. The reaction proceeds until one reactant is completely consumed. A. Write a balanced chemical equation for this reaction. B. What is the theoretical yield of ammonia? C. What is the percent yield of ammonia if $$45.3\mathrm{g}$$ is actually produced? 34. Sulfur dioxide reacts with oxygen to produce sulfur trioxide. $$150.\mathrm{g}$$ of sulfur dioxide is reacted with $$50.0\mathrm{g}$$ of oxygen. The reaction proceeds until one reactant is completely consumed. A. Write a balanced chemical equation for this reaction. B. What is the theoretical yield of sulfur trioxide? What is the percent yield of sulfur trioxide if $$180.\mathrm{g}$$ is actually produced.