Question

Calculate the work done during the reaction represented by the following thermochemical equation at 300K :
CH4 + 2O2 ➡️ CO2 + 2H20
(g). (g). (g). (L)
(R= 8.314 J/Kmol)

Answer 1

Work Done Comes 4.988 kJ

Explanation:

Work is done during any chemical reaction that can be calculated with the help of a Chemical equation.

The Chemical Equation says -  

• Work Done = $- \Delta n_g \times R \times T$ """(1)

where,

Where $\Delta$ is the change in the number of moles of gas.

$\Delta n_g$ = -(-2) = 2

The Universal gas Constant, R = 8.314 $\frac {J}{Kmol}$

Temperature, T = 300 K

Applying Equation (1) we get -  

W = $- \Delta n_g \times R \times T$

= $-(-2) \times 8.314 \times 300$

= 4988.4 J

or

4.9884 kJ is the Work Done

Answer 2

The work done during the reaction is 4.988 KJ

Explanation:

The chemical reaction given is:

CH₄ + 2O₂ → CO₂ + 2H₂O

Now, the work done of the chemical reaction is given by the formula:

W = -Δng RT

Where,

Δng = Changes in number of gas moles

R = Gas constant = 8.314 J/Kmol (constant)

T = Temperature = 300 K (given)

Δng = Product - Reactant = 1 - 3 = -2

Now, the work done is given as:

W = -(-2) × 8.314 × 300

∴ W = 4.988 KJ