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tresset_1 [31]
3 years ago
14

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 tak

es 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
Chemistry
1 answer:
worty [1.4K]3 years ago
6 0

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

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