EXPERIMENT 13: PRE-LABORATORY Ideal Gas Law: Determination of the Molar Mass of

Question

EXPERIMENT 13: PRE-LABORATORY Ideal Gas Law: Determination of the Molar Mass of a Volatile Compound Name: Section: Pre-Laboratory Review Questions and Exercises DUE BEFORE LAB BEGINS. ANSWER IN THE SPACE PROVIDED. 1. How many moles of gas are contained in 500.0 mL at 22.0 °C and 710.0 mm Hg pressure? 2. What volume will 2.00 moles of neon gas occupy at STP? 3. At what temperature will 5.00 moles of helium gas occupy 50.0 liters at 1,20 atmospheres? 0.514 g of a gas occupies 150.0 mL at 23.0 "C and 75S torr. What is its molar mass? What gas is it? 4. 5. A 75.0 L vessel contains 4.00 g of H, and 30.00 g of O gases at 50.0 °C. What is the partial pressure of each gas?

Explanation / Answer

Ans 1 :

Number of moles of gas can be calculated using the ideal gas law , pV = nRT

p = 710 mmHg = 0.934211 atm

V = 0.500 L

T = 22oC = 295.15 K

R = 0.0821 L.atm / mol. K

So putting all the values we get :

0.934211 x 0.500 = n x 0.0821 x 295.15

n = 0.0193 moles

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