How many moles of CO2 are produced when 3 moles of pentane react with excess oxygen? C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(l) 5 moles 3/5 moles 15 moles 3 moles Answer: c

How many moles of CO2 are produced when 3 moles of pentane react with excess oxygen? C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(l) 5 moles 3/5 moles 15 moles 3 moles Answer: c

The overall equation involved in photosynthesis is The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2. How many grams of glucose (C6H12O6, 180.1 g/mol) form when 4.40 g of CO2 react? 18.0 g 3.00 g 108 g 0.0167 g Answer: b

The overall equation involved in photosynthesis is The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2. How many grams of glucose (C6H12O6, 180.1 g/mol) form when 4.40 g of CO2 react? 18.0 g 3.00 g 108 g 0.0167 g Answer: b

The rapid decomposition of sodium azide, NaN3, to its elements is one of the reactions used to inflate airbags: 2 NaN3 (s)  2 Na (s) + 3 N2 (g) How many grams of N2 are produced from 6.00 g of NaN3? 3.88 g 1.72 g 0.138 g 2.59 g Answer: a

The rapid decomposition of sodium azide, NaN3, to its elements is one of the reactions used to inflate airbags: 2 NaN3 (s)  2 Na (s) + 3 N2 (g) How many grams of N2 are produced from 6.00 g of NaN3? 3.88 g 1.72 g 0.138 g 2.59 g Answer: a

The overall equation involved in photosynthesis is The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2. How many grams of carbon dioxide (CO2) are required to produce 18.0 g of C6H12O6? 18.0 g 3.00 g 54.0 g 26.4 g 4.40 g Answer: d

The overall equation involved in photosynthesis is The overall equation involved in photosynthesis is 6 CO2 + 6 H2O  C6H12O6 + 6 O2. How many grams of carbon dioxide (CO2) are required to produce 18.0 g of C6H12O6? 18.0 g 3.00 g 54.0 g 26.4 g 4.40 g Answer: d

Ammonia is produced using the Haber process: Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 Calculate the mass of ammonia produced when 35.0 g of nitrogen react with 12.5 g of hydrogen. 47.5 g 42.6 g 35.0 g 63.8 g 70.5 g Answer: b

Ammonia is produced using the Haber process: Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 Calculate the mass of ammonia produced when 35.0 g of nitrogen react with 12.5 g of hydrogen. 47.5 g 42.6 g 35.0 g 63.8 g 70.5 g Answer: b

Ammonia is produced using the Haber process: Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 What percent yield of ammonia is produced from 15.0 kg each of H2 and N2, if 13.7 kg of product are recovered? Assume the reaction goes to completion. 7.53 × 10–2 % 1.50 × 10–1 % 75.3% 15.0% 16.2% Answer: c

Ammonia is produced using the Haber process: Ammonia is produced using the Haber process: 3 H2 + N2  2 NH3 What percent yield of ammonia is produced from 15.0 kg each of H2 and N2, if 13.7 kg of product are recovered? Assume the reaction goes to completion. 7.53 × 10–2 % 1.50 × 10–1 % 75.3% 15.0% 16.2% Answer: c

What mass of TiCl4 is needed to produce 25 What mass of TiCl4 is needed to produce 25.0 g of Ti if the reaction proceeds with an 82% yield? TiCl4 + 2Mg  Ti + 2 MgCl2 30.5 g 121 g 99.1 g 81.2 g Answer: b

What mass of TiCl4 is needed to produce 25 What mass of TiCl4 is needed to produce 25.0 g of Ti if the reaction proceeds with an 82% yield? TiCl4 + 2Mg  Ti + 2 MgCl2 30.5 g 121 g 99.1 g 81.2 g Answer: b

What is the molarity of an aqueous solution containing 22 What is the molarity of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution? 0.0657 M 1.85 × 10–3 M 1.85 M 3.52 M 0.104 M Answer: c

What is the molarity of an aqueous solution containing 22 What is the molarity of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution? 0.0657 M 1.85 × 10–3 M 1.85 M 3.52 M 0.104 M Answer: c

Sulfuric acid is found in some types of batteries. What volume of 3 Sulfuric acid is found in some types of batteries. What volume of 3.50 M H2SO4 is required to prepare 250.0 mL of 1.25 M H2SO4? 17.5 mL 700. mL 89.3 mL 109 mL None of the above Answer: c

Sulfuric acid is found in some types of batteries. What volume of 3 Sulfuric acid is found in some types of batteries. What volume of 3.50 M H2SO4 is required to prepare 250.0 mL of 1.25 M H2SO4? 17.5 mL 700. mL 89.3 mL 109 mL None of the above Answer: c

A 45.0 mL solution is 0.500 M HCl. What is the concentration after 25.0 mL of water is added to the solution? Assume volumes are additive. 0.321 M 0.179 M 0.900 M 0.278 M Answer: a

A 45.0 mL solution is 0.500 M HCl. What is the concentration after 25.0 mL of water is added to the solution? Assume volumes are additive. 0.321 M 0.179 M 0.900 M 0.278 M Answer: a

Which of the following aqueous solutions would conduct electricity? AgNO3 C11H22O11 (sucrose) CH3CH2OH (ethanol) All of the above None of the above Answer: a

Which of the following aqueous solutions would conduct electricity? AgNO3 C11H22O11 (sucrose) CH3CH2OH (ethanol) All of the above None of the above Answer: a

What is the maximum number of grams of PbI2 precipitated upon mixing 25.0 mL of 0.150 M KI with 15.0 mL of 0.175 M Pb(NO3)2? 0.864 g 1.73 g 1.21 g 2.07 g None of the above Answer: a

What is the maximum number of grams of PbI2 precipitated upon mixing 25.0 mL of 0.150 M KI with 15.0 mL of 0.175 M Pb(NO3)2? 0.864 g 1.73 g 1.21 g 2.07 g None of the above Answer: a

A 25. 0 mL sample of H2SO4 is neutralized with NaOH A 25.0 mL sample of H2SO4 is neutralized with NaOH. What is the concentration of the H2SO4 if 35.0 mL of 0.150 M NaOH are required to completely neutralize the acid? 0.210 M 0.105 M 0.150 M 0.420 M None of the above Answer: b

A 25. 0 mL sample of H2SO4 is neutralized with NaOH A 25.0 mL sample of H2SO4 is neutralized with NaOH. What is the concentration of the H2SO4 if 35.0 mL of 0.150 M NaOH are required to completely neutralize the acid? 0.210 M 0.105 M 0.150 M 0.420 M None of the above Answer: b

What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize 1000.0 L of 0.350 M H2SO4? 2.94 × 104 g 1.47 × 104 g 5.88 × 104 g 3.50 × 103 g 1.75 × 103 g Answer: c

What mass, in grams, of sodium bicarbonate, NaHCO3, is required to neutralize 1000.0 L of 0.350 M H2SO4? 2.94 × 104 g 1.47 × 104 g 5.88 × 104 g 3.50 × 103 g 1.75 × 103 g Answer: c