Answer to Question #256921 in Chemistry for kevin

Question

1. We are given the initial pressure of 1.5 atm and temperature of 25⁰C of the gas and asked for the pressure at a higher temperature of 450⁰C 

Answer 1

Let's assume that the volume of gas remains unchanged.

P₁ = 1.5 atm

T₁ = 25⁰C = 298 K

V₁ = V₂ = constant

P₂ = unknown

T₂ = 450⁰C = 723 K

Solution:

Since the volume doesn't change, Gay-Lussac's law can be used.

Gay-Lussac's law can be expressed as: P₁/T₁ = P₂/T₂

P₁T₂ = P₂T₁

To find the final pressure, solve the equation for P₂:

P₂ = P₁T₂/T₁

P₂ = (1.5 atm × 723 K) / (298 K) = 3.6393 atm = 3.6 atm

P₂ = 3.6 atm

Answer: The final pressure of gas is 3.6 atm