Question

A sample of (N2O3 ,(g)) has a pressure of 0.020 atm. The temperature (in K) is then doubled, and the (N2O3) undergoes complete decomposition to (NO2 ,(g)) and (NO, (g)).

What is the new pressure?
- A) 0.010 atm
- B) 0.020 atm
- C) 0.040 atm
- D) 0.080 atm

Answer 1

The new pressure after the complete decomposition of N2O3 to NO2 and NO when the temperature is doubled would be 0.040 atm, as the number of moles of gas increases and the pressure doubles according to the ideal gas law.

Step-by-step explanation:

The question is about the chemical decomposition of dinitrogen trioxide (N2O3) to nitrogen dioxide (NO2) and nitric oxide (NO) when the temperature is doubled, and how it affects the pressure of the system. Given that the initial pressure of N2O3 is 0.020 atm and assuming the ideal gas law applies, the decomposition reaction can be represented as:

N2O3 (g) → NO2 (g) + NO (g)

Since one mole of N2O3 produces two moles of gas (one mole of NO2 and one mole of NO), there is a net increase in the number of moles of gas. If the temperature is doubled and the volume remains constant, according to the combined gas law (P1/T1 = P2/T2), the pressure would also double. Therefore, the new pressure after the decomposition and doubling of temperature would be 0.020 atm × 2 = 0.040 atm, which corresponds to option C.