Question

A sample of gas contains 0.1100 mol of N2(g) and 0.3300 mol of H2(g) and occupies a volume of 20.5 L. The following reaction takes place: N2(g) 3 H2(g) 2 NH3(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. g

Answer 1

Answer:

20.5 L

Explanation:

-The stoichiometric reaction of the 2 gases is:

$N_2_{(g)}+3H_2_{(g)}->2NH_3_{(G)}$

-We apply the combined gas law to determine the resultant volume of the ammonia gas formed:

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}\\\\\#But\\\\\frac{P_1}{T_1}=\frac{P_2}{T_2}\\\\\therefore V_1=V_2$

Since, the temperature and pressure remain constant, the volume of the ammonia gas formed is equal to the volume of the reactants.

Hence, the volume after the reaction is 20.5 L