At constant pressure, the combustion of 5.00 g of c2h6(g) releases 259 kj of heat. what is δh for the reaction given below? 2 c2h6(g) + 7 o2(g) → 4 co2(g) + 6 h2o(l).

3120 kJ

Given:

At constant pressure, the combustion of 5.00 g of C₂H₅  releases 259 kJ of heat.

Question:

What is ΔH for the reaction given below?

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The Process:

Step-1

Step-2

Let us convert mass to mol of 5 g of C₂H₅.

Remember, the combustion of 0.166 moles of C₂H₅ releases 259 kJ of heat.

Step-3

Combustion reactions that release heat into the environment, including the type of exothermic reaction. The exothermic reaction has a negative ΔH because the product enthalpy is lower than the reactant enthalpy of the system.

And now, we will solve the problem of what is ΔH for the reaction given below.

Notice that 2 moles of C₂H₅ take part in this reaction.

Thus, the combustion of C₂H₅ based on the equation of reaction above releases heat of 3120 kJ.

l dont know l am s sorry

the answer is a! (2.9 x 10^-18 j) hope i could someone. : )