Question

A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to 475 K at constant volume

Answer 1

Answer:

1.20 × 10³ torr

Explanation:

Step 1: Given data

• Initial pressure (P₁): 822 torr

• Initial temperature (T₁): 325 K

• Final pressure (P₂): ?

• Final temperature (T₂): 475 K

• Constant volume: 750 mL

Step 2: Calculate the final pressure of the gas

Considering the constant volume, if we assume the gas behaves ideally, we can calculate its final pressure using Gay-Lussac's law.

P₁/T₁ = P₂/T₂

P₂ = P₁ × T₂/T₁

P₂ = 822 torr × 475 K/325 K = 1.20 × 10³ torr