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a. 252 g<br />
b. 63.0 g<br />
c. 116 g<br />
d. 84.0 g<br />
e. 76.0 g<br />
____ 66. The reaction of 5.0 g of fluorine with excess chlorine produced 5.6 g of ClF3. What percent yield of ClF3 was<br />
obtained?<br />
Cl2 + 3F2 2ClF3<br />
a. 58%<br />
b. 69%<br />
c. 76%<br />
d. 86%<br />
e. 92%<br />
____ 67. If a reaction of 5.0 g of hydrogen with 5.0 g of carbon monoxide produced 4.5 g of methanol, what was the<br />
percent yield?<br />
2H2 + CO CH3OH<br />
a. 11%<br />
b. 79%<br />
c. 96%<br />
d. 24%<br />
e. 63%<br />
____ 68. What mass of water is contained in 160. grams of 22.0% KCl solution?<br />
a. 125 g<br />
b. 86.8 g<br />
c. 35.2 g<br />
d. 130 g<br />
e. 112 g<br />
____ 69. Calculate the molarity of a solution that contains 70.0 g of H2SO4 in 280. mL of solution.<br />
a. 2.55 M<br />
b. 6.84 M<br />
c. 8.62 M<br />
d. 9.78 M<br />
e. 11.84 M<br />
____ 70. What is the molarity of 175 mL of solution containing 2.18 grams of Na2SO4•10H2O?<br />
a. 3.77 10 -3 M<br />
b. 6.44 10 -1 M<br />
c. 8.78 10 -3 M<br />
d. 1.18 10 -3 M<br />
e. 3.87 10 -2 M<br />
____ 71. The specific gravity of commercial nitric acid solution is 1.42 and it is 70.0% HNO3 by mass. Calculate its<br />
molarity.<br />
a. 18.0 M