A sample of N2 O3(g) has a pressure of 0.017 atm. The...

A sample of $\mathrm{N}_{2} \mathrm{O}_{3}(g)$ has a pressure of 0.017 atm. The temperature (in K) is doubled, and the $\mathrm{N}_{2} \mathrm{O}_{3}$ undergoes complete decomposition to $\mathrm{NO}_{2}(g)$ and $\mathrm{NO}(g) .$ Find the total pressure of the mixture of gases assuming constant volume and no additional temperature change.

A sample of $\mathrm{N}_{2} \mathrm{O}_{3}(g)$ has a pressure of 0.017 atm. The temperature
(in K) is doubled, and the $\mathrm{N}_{2} \mathrm{O}_{3}$ undergoes complete decomposition to $\mathrm{NO}_{2}(g)$ and $\mathrm{NO}(g) .$ Find the total pressure of the mixture of gases
assuming constant volume and no additional temperature change.

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Key Concepts

Reaction Stoichiometry in Gaseous Systems

Stoichiometry in gas-phase reactions involves using the balanced chemical equation to determine how the amount of reactants converts into products. This is crucial because the reaction can change the total number of moles of gas, which, under constant volume conditions, directly affects the overall pressure of the system.

Ideal Gas Law

The ideal gas law (PV = nRT) links the pressure, volume, amount, and temperature of a gas. It is essential for understanding how a gas responds to changes in temperature or number of moles while maintaining constant volume, since pressure is directly proportional to both the number of gas particles and the temperature.

Temperature Effects on Gas Pressure

When the volume of a gas is held constant, any change in temperature results in a proportional change in pressure according to the ideal gas law. Understanding this relationship is important for predicting how doubling the temperature can lead to an increase in pressure in a system where reactions alter the mole count of the gas.

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