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

Answer:

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 - $0.0821 \frac{L \cdot atm}{mol \cdot K}$
• T is temperature (in Kelvins)

Explanation:

Step 1: Define

10.0 L

3.00 mol H₂

4.50 atm

Step 2: Find Temperature

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

Step 3: Check

Round to the nearest whole number.

182.704 K ≈ 183 K