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4 votes
Given:

CH4 + 2O2 → CO2 + 2H2O, ΔH = -890 kJ/mol

How much energy is released when 59.7 grams of methane (CH4) reacts with oxygen?

The combustion of 59.7 grams of methane releases ____ kilojoules of energy

User Sean Kilb
by
8.1k points

2 Answers

5 votes

Answer:

The combustion will release -3,321 KJ/mol of energy

Step-by-step explanation:

User Nguyen Viet Cuong
by
8.3k points
2 votes

Answer:

The combustion of 59.7 grams of methane releases 3320.81 kilojoules of energy

Step-by-step explanation:

Given;

CH₄ + 2O₂ → CO₂ + 2H₂O, ΔH = -890 kJ/mol

From the combustion reaction above, it can be observed that;

1 mole of methane (CH₄) released 890 kilojoules of energy.

Now, we convert 59.7 grams of methane to moles

CH₄ = 12 + (1x4) = 16 g/mol

59.7 g of CH₄
= (59.7)/(16) = 3.73125 \ moles

1 mole of methane (CH₄) released 890 kilojoules of energy

3.73125 moles of methane (CH₄) will release ?

= 3.73125 moles x -890 kJ/mol

= -3320.81 kJ

Therefore, the combustion of 59.7 grams of methane releases 3320.81 kilojoules of energy

User Apolo
by
8.3k points
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