Based on the thermochemical equation 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O...

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Question

Based on the thermochemical equation 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O...

Based on the thermochemical equation 2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O ΔH = -5316 kJ,

if (5.81x10^1) g of C₄H₁₀ (MM = 58.14 g/mol) reacted with excess oxygen, how many kJ of heat would be released?

NOTE: The word "released" means that NO NEGATIVE SIGN IS NEEDED in your answer.

Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer.

Do not round any intermediate calculations.

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Answer 1

Answer #1

Since the heat released in this reaction corresponds to 1 mole of C4H10 which is -5316 KJ...Now 1 mole of C4H10 has molar mass 58.14g and again in the statement the heat released by combustion of 58.1g of C4H10 is asked...so it will be same i.e. -5316 KJ

So, the final answer is -5316 KJ

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Answer 2

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Add Answer to: Based on the thermochemical equation 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O...

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Based on the thermochemical equation 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O...