Question

Given reaction 2NH₃(g) + 3Cl₂(g) ⟶ N2(g) + 6HCl(g), you react 5.0 L of NH₃ with 5.0 L of Cl₂ measured at the same conditions in a closed container. Calculate the ratio of pressures in the container Pfinal : Pinitial.

a) 1:1
b) 3:2
c) 2:3
d) 4:3

Answer 1

To calculate the ratio of pressures in the container, use the ideal gas law equation and the stoichiometry of the reaction. Given that you initially have 5.0 L of NH₃ and 5.0 L of Cl₂, the ratio of pressures is 2:3.

Step-by-step explanation:

To calculate the ratio of pressures in the container, we need to use the ideal gas law equation: 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. Since the temperature, volume, and the number of moles of the gases are constant, we can simplify the equation to: Pfinal/Pinitial = (nfinal/ninitial). The ratio of moles can be calculated using the stoichiometry of the reaction, which is 2 moles of NH₃ react with 3 moles of Cl₂.

Given that you initially have 5.0 L of NH₃ and 5.0 L of Cl₂, the moles of NH₃ and Cl₂ will be equal.

To find the ratio of pressures, we substitute the number of moles into the equation: Pfinal/Pinitial = (nfinal/ninitial) = (2 moles of NH₃/5 L of NH₃) / (3 moles of Cl₂/5 L of Cl₂) = 2/3. Therefore, the ratio of pressures in the container is 2:3, option c).