Chemistry question please help

Question

A container of N2O3(g) has a pressure of 0.270 atm. When the absolute temperature of the N2O3(g) is tripled, the gas completely decomposes, producing NO2(g) and NO(g). Calculate the final pressure of the gas mixture, assuming that the container volume does not change.

Answer 1

N₂O₃(g) ==> NO₂(g) + NO(g) ... balanced equation for decomposition of N₂O₃

Constant volume & an increase in temperature means pressure will have to increase since you are going from 1 mole of gas on the reactant side to 2 moles of gas on the product side.

P₁/n₁T₁ = P₂/n₂T₂

P₁ = initial pressure = 0.270 atm

n₁ = initial # of moles = 1

T₁ = initial temperature

P₂ = final pressure = ?

n₂ = final moles = 2

T₂ = final temperature = 3T1

(0.270) / (1)(T₁) = P₂ / (2)(3T₁)

P₂ = (0.270)(2)(3T₁) / T₁

P₂ = 0.270 atm x 6 = 1.62 atm