Question

Values of R, the ideal gas constant, and the ideal gas equation are given below. Use these to solve the problems.

PV = nRT
A 10.0-L rigid container holds 3.00 mol H2 gas at a pressure of 4.50 atm. What is the temperature of the gas? (Round to the nearest whole number)
K

Answer 1

183 K

General Formulas and Concepts:

Chemistry - Gas Laws

Combined Gas Law: PV = nRT

• P is pressure
• V is volume (in Liters)
• n is amount of moles
• R is gas constant -
  `0.0821 (L \cdot atm)/(mol \cdot K)`
• T is temperature (in Kelvins)

Step-by-step explanation:

Step 1: Define

10.0 L

3.00 mol H₂

4.50 atm

Step 2: Find Temperature

1. Substitute [CGL]:
   `(4.50 \ atm)(10.0 \ L) = (3.00 \ mol)(0.0821 (L \cdot atm)/(mol \cdot K))(x \ K)`
2. Isolate temperature x:
   `((4.50 \ atm)(10.0 \ L))/((3.00 \ mol)(0.0821 (L \cdot atm)/(mol \cdot K))) = x \ K`
3. Rewrite:
   `x \ K = ((4.50 \ atm)(10.0 \ L))/((3.00 \ mol)(0.0821 (L \cdot atm)/(mol \cdot K)))`
4. Evaluate:
   `x = 182.704 \ K`

Step 3: Check

Round to the nearest whole number.

182.704 K ≈ 183 K