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natka813 [3]
3 years ago
12

11. Assuming that the gases are ideal, calculate the amount of work done (joules) in each of the following reactions at 25 degre

es Celsius. a. 4 HCl(g) + Ox(9) + 2Cl(g) + 2 H2O(g) b. 2 NO(g) → Na(g) + O2(g)
Chemistry
1 answer:
gayaneshka [121]3 years ago
3 0

<u>Answer:</u>

<u>For a:</u> Work done for the given reaction is 2477.572 J.

<u>For b:</u> Work done for the given reaction is 0 J

<u>Explanation:</u>

To calculate the work done for the reaction, we use the equation:

W=-P\Delta V

Ideal gas equation follows:

PV=nRT

Relating both the above equations, we get:

W=-\Delta n_gRT     ......(1)

where,

\Delta n_g = difference in number of moles of products and reactants = n_g_{(products)}-n_g_{(reactants)}

R = Gas constant = 8.314 J/K.mol

T = temperature = 25^oC=[273+25]K=298K

  • <u>For a:</u>

The chemical reaction follows:

4HCl(g)+O_2(g)\rightarrow 2Cl_2(g)+2H_2O(g)

\Delta n_g=4-5=-1

Putting values in equation 1, we get:

W=-(-1mol)\times (8.314J/K.mol)\times 298K=2477.572J

Hence, work done for the given reaction is 2477.572 J.

  • <u>For b:</u>

The chemical reaction follows:

2NO(g)\rightarrow N_2(g)+O_2(g)

\Delta n_g=2-2=0

Putting values in equation 1, we get:

W=-(0mol)\times (8.314J/K.mol)\times 298K=0J

Hence, work done for the given reaction is 0 J.

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