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The enthalpy change \mathrm{(\Delta H^{\circ})}for the combustion of methane \mathrm{CH_{4}} at constant pressure is -890.3 kJ/mol. Calculate the heat released when 4 moles of methane are completely combusted at constant pressure.

Option: 1

-3561.2 kJ
 


Option: 2

3561.2 kJ
 


Option: 3

2200 kJ
 


Option: 4

-2200 kJ


Answers (1)

The heat (q) released in a reaction at constant pressure is given by:

\mathrm{q=n \times \Delta H^{\circ}}

where n is the number of moles of the substance and \mathrm{\Delta H^{\circ}} is the standard enthalpy change for the reaction.
Given:

\mathrm{\begin{aligned} n & =4 \text { moles } \\ \Delta H^{\circ} & =-890.3 \mathrm{~kJ} / \mathrm{mol} \end{aligned}}

Substituting the values:

\mathrm{q=4 \times-890.3 \mathrm{~kJ} / \mathrm{mol}=-3561.2 \mathrm{~kJ}}

Therefore, the heat released when 4 moles of methane are completely com-
busted at constant pressure is -3561.2 kJ.

So, the correct option is A

Posted by

Ramraj Saini

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