Department of Chemistry

Chemistry 11a/15a Placement Exam

Question #1: 

Evaluate (0.04)1/2

Question #2: 

If 2 + (4 + x)1/2 = 10, what is the value of x?

Question #3: 

Evaluate (6 × 10–6)(4 × 10–4) / (3 × 10–3)

Question #4: 

How many moles of carbon are present in 6 moles of Al2(C2O4)3?

Question #5: 

If (V2/V1) = (M1/M2)1/2, what is the expression for M2 in terms of the other three variables?

Question #6: 

Suppose that (1/V) = (A/B) (1/S) + (1/B), where V and S are variables and A and B are constants. If (1/V) is plotted on the y-axis versus (1/S) on the x-axis,

  1. What is the expression for the y-intercept?

  2. What is the expression for the x-intercept?

Question #7: 

Evaluate [log(100) – antilog(2)]

Question #8: 

You are given 1 liter of 1 M glucose. You dilute it by adding to it 9 liters of distilled water. What is the final concentration?

Question #9: 

Given that 1 cm3 = 1 mL, how many liters are there in a cubic meter?

Question #10: 

If the atomic mass of Br is 80. g/mol, what mass of Br2 is required to prepare 500. mL of 0.010 M aqueous Br2?

Question #11: 

If the density of a liquid is 0.80 g/mL, what is the volume of 2.4 grams of the liquid?

Question #12: 

If 24 g of a compound synthesized in the laboratory represents a yield of 75%, what is the maximum (100%) yield?

Question #13: 

If x + y = 2 and 2x + 4y = 5

  1. What is the value of x?

  2. What is the value of y

Question #14:

Apples cost $1.50 per pound, and bananas cost $0.60 per pound. If a student buys 8.00 pounds of fruit (apples and bananas) for $9.30, how many pounds of apples did the student buy?

Question #15:

Hydrogen atoms have a mass of 1.00 g/mol, and oxygen atoms have a mass of 16.0 g/mol. Liquid water has a density of 1.00 g/mL. Hydrogen and oxygen gases are burned to produce water, which is then condensed into a liquid. If this reaction produces 90.0 mL water, how many grams of oxygen gas were consumed?