1. A strip of silver foil has a uniform width of 1.00 cm and a uniform thickness of 0.0119 cm. If the density of silver is 10.5 g/cm³, how long a strip should be cut to obtain 1.00 g of the metal?

(A) 9.52 x 10¯² cm
(B) 1.19 cm
(C) 8.00 cm
(D) 12.5 cm

2. A car traveling at 10 miles per hour emits about 0.15 kg of carbon monoxide (CO) gas per mile. How many moles of CO are emitted per mile under theses conditions?

(A) 1.5 x 10¯¹
(B) 5.4
(C) 9.4
(D) 12.5

3. You need to fertilize an area with the equivalent of 25.0 pounds of nitrogen, N. How much urea, CON₂H₄, should be used?

(A) 46.7 lb
(B) 53.6 lb
(C) 107 lb
(D) 127 lb

4. A sample of a conpound contains 0.100 g of hydrogen and 4.20 g of nitrogen. The simplest formula for the compound is

(A) HN₂
(B) HN₃
(C) NH₃
(D) NH₂

5. If the hydrocarbon C₂H₄ is burned in oxygen gas, carbon dioxide and water are formed as described by the unbalanced chemical equation

C₂H₄ + O₂ ----> CO₂ + H₂O

When this equation is balanced properly, we predict that one mole of C₂H₄ will

(A) react with one mole of O₂
(B) form two moles of CO₂.
(C) form three moles of water.
(D) react with four moles of O₂.

6. A human patient suffering from a duodenal ulcer may show a hydrochloric acid concentration of 0.080 mol/liter in his gastric juice. It is possible to neutralize this acid with aluminum hydroxide, Al(OH)₃, which reacts with HCl according to the balanced chemical equation

Al(OH)₃ + 3 HCl ----> AlCl₃ + 3 H₂O

If the patient's stomach receives 3.0 liters of gastric juice per day, how much aluminum hydroxide must he consume per day to counteract the acid?

(A) 6.2 g
(B) 19 g
(C) 26 g
(D) 78 g

7. The correct molecular formula of a compound that has an empirical formula of C₂H₂O and a molecular weight of 168 is

(A) C₂HO
(B) C₄H₂₄O₆
(C) C₈H₈O₄
(D) C₈H₁₂O₅

8. Given the reaction

Na₂O(s) + H₂O(l) -----> 2 NaOH(aq)

what is the molarity of the solution formed if 1.35 g of Na₂O is mixed with water such that the final volume is 100 mL?

(A) 0.0435 M
(B) 0.108 M
(C) 0.217 M
(D) 0.435 M

9. When ignited in air, magnesium burns with a bright flame to form magnesium oxide. The standard heat of formation of solid MgO is -1203 kJ/mol. How much heat is evolved when sufficient magnesium meal is burned in oxygen to form 1.0 g of MgO?

(A) 0.025 kJ
(B) 30 kJ
(C) 40 kJ
(D) 1203 kJ

10. ⁴⁰Ca, ³⁹K, and ⁴¹Sc all have the same

(A) number of electrons.
(B) atomic number.
(C) mass number.
(D) number of neutrons.

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