N2O3(g) → NO2(g) + NO(g)
P1 = 0.018 atm
initial temperature = T1
final temperature = 2 T1
initial amount = 1 mole of gas
final amount = 2 moles of gas
Ideal Gas Law:
A sample of N2O3(g) has a pressure of 0.018 atm . The temperature (in K) is then doubled and the N2O3 undergoes complete decomposition to NO2(g) and NO(g).
Find the total pressure of the mixture of gases assuming constant volume and no additional temperature change.
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