In the following reaction, what is the quantity of heat (in kJ) released when 5.87 moles of CH₄ are burned?
1 answer:
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?
<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.
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Answer: 3.024 g grams of hydrogen are needed to convert 76 grams of chromium(III) oxide,
Explanation:
The reaction equation for given reaction is as follows.
Here, 1 mole of reacts with 3 moles of
.
As mass of chromium (III) oxide is given as 76 g and molar mass of chromium (III) oxide is 152 g/mol.
Number of moles is the mass of substance divided by its molar mass. So, moles of is calculated as follows.
Now, moles of .given by 0.5 mol of
is calculated as follows.
As molar mass of is 2.016 g/mol. Therefore, mass of
is calculated as follows.
Thus, we can conclude that 3.024 g grams of hydrogen are needed to convert 76 grams of chromium(III) oxide, .