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natima [27]
2 years ago
9

In the following reaction, what is the quantity of heat (in kJ) released when 5.87 moles of CH₄ are burned?

Chemistry
1 answer:
IRISSAK [1]2 years ago
5 0

Taking into account the definition of enthalpy of a chemical reaction, the quantity of heat released when 5.87 moles of CH₄ are burned is 4,707.74 kJ.

The enthalpy of a chemical reaction as the heat absorbed or released in a chemical reaction when it occurs at constant pressure. That is, the heat of reaction is the energy that is released or absorbed when chemicals are transformed into a chemical reaction.

The enthalpy is an extensive property, that is, it depends on the amount of matter present.

In this case, the balanced reaction is:

CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g)

and the enthalpy reaction ∆H° has a value of -802 kJ/mol.

This equation indicates that when 1 mole of CH₄ reacts with 2 moles of O2, 802 kJ of heat is released.

When 5.87 moles of CH₄ are burned, then you can apply the following rule of three: if 1 mole of CH₄ releases 802 kJ of heat, 5.87 moles of CH₄ releases how much heat?

heat=\frac{5.87 molesof CH_{4}x802 kJ}{1 mol of CH_{4} }

<u><em>heat= 4,707.74 kJ</em></u>

Finally, the quantity of heat released when 5.87 moles of CH₄ are burned is 4,707.74 kJ.

Learn more:

  • brainly.com/question/15355361?referrer=searchResults
  • brainly.com/question/16982510?referrer=searchResults
  • brainly.com/question/13813185?referrer=searchResults
  • brainly.com/question/19521752
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