Consider the reaction C₂H₅OH(l) + 3O₂(g) $\rightarrow$ 2CO₂(g) + 3H₂O(l) , $\Delta$ H = -1.37 * 10³ kJ
When a 15.4-g sample of ethyl alcohol (molar mass = 46.1 g/mol) is burned, how much energy is released as heat?

Name: Consider the reaction C 2 H 5 OH(l) + 3O 2 (g) $\rightarrow$2CO 2 (g) + 3H 2 O(l), $\Delta$H = -1.37 * 10 3 kJ When a 15.4-g sample of ethyl alcohol (molar mass = 46.1 g/mol) is burned, how much energy is released as heat?
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Question

Consider the reaction C₂H₅OH(l) + 3O₂(g)

\rightarrow

2CO₂(g) + 3H₂O(l) ,

\Delta

H = -1.37 * 10³ kJ
When a 15.4-g sample of ethyl alcohol (molar mass = 46.1 g/mol) is burned, how much energy is released as heat?

Quizplus · Accepted Answer

The Answer is B

Consider the Reaction C2H5OH(l) + 3O2(g) →\rightarrow→ 2CO2(g) + 3H2O(l) Δ\DeltaΔ H = -137 * 103 KJ When a 15

Consider the Reaction C₂H₅OH(l) + 3O₂(g) $\rightarrow$ 2CO₂(g) + 3H₂O(l) $\Delta$ H = -137 * 10³ KJ
When a 15