Question

Which of the following reactions will result in a reduced total pressure at constant

temperature in a rigid reaction vessel?
Hint: Look at the change in the number of moles of gas
O N₂O4(g) →2 NO₂(g)
O2 H₂(g) + O2(g) → 2 H₂O(l)
O CH4(g) + 2 O2(g) → CO₂(g) + 2 H₂O(g)
O 2 HI(g) → H₂(g) + 12(g)
O 2 N₂O(g) →2 N₂(g) + O₂(g)

Answer 1

The reaction that will result in a reduced total pressure at constant temperature in a rigid reaction vessel is 2 N₂O(g) → 2 N₂(g) + O₂(g).

Step-by-step explanation:

In a reaction vessel, the total pressure is determined by the number of gas moles present. According to the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

To reduce the total pressure at constant temperature, the number of moles of gas needs to decrease. Looking at the given reactions, the following reaction will result in a reduced total pressure: 2 N₂O(g) → 2 N₂(g) + O₂(g).

This reaction involves a decrease in the number of moles of gas by converting 2 moles of N₂O to 2 moles of N₂ and 1 mole of O₂. This reduction in gas moles will lead to a reduced total pressure in the reaction vessel.

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