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Over [174]
3 years ago
12

A sample of gas contains 0.1300 mol of N2(g) and 0.2600 mol of O2(g) and occupies a volume of 23.9 L. The following reaction tak

es place: N2(g) + 2O2(g)2NO2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.
Chemistry
1 answer:
AlekseyPX3 years ago
6 0

Answer : The volume of the sample after the reaction takes place is, 15.93 liters.

Explanation : Given,

Moles of N_2 = 0.13 mole

Moles of O_2 = 0.26 mole

Initial volume of gas = 23.9 L

First we have to calculate the moles of NO_2 gas.

The balanced chemical reaction is :

N_2(g)+2O_2(g)\rightarrow 2NO_2(g)

From the balanced reaction, we conclude that

As, 1 mole of N_2 react with 2 moles of O_2 to give 2 moles of NO_2.

So, 0.13 mole of N_2 react with 2\times 0.13=0.26 moles of O_2 to give 2\times 0.13=0.26 moles of NO_2.

According to the Avogadro's Law, the volume of the gas is directly proportional to the number of moles of the gas at constant pressure and temperature.

V\propto n

or,

\frac{V_1}{V_2}=\frac{n_1}{n_2}

where,

V_1 = initial volume of gas = 23.9 L

V_2 = final volume of gas = ?

n_1 = initial moles of gas = 0.13 + 0.26 = 0.39 mole

n_2 = final moles of gas = 0.26 mole

Now put all the given values in the above formula, we get the final temperature of the gas.

\frac{23.9L}{V_2}=\frac{0.39mole}{0.26mole}

V_2=15.93L

Therefore, the volume of the sample after the reaction takes place is, 15.93 liters.

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