Question

question 4 of 27
during a reaction, the enthalpy of formation of an intermediate is -286 kj/mol. during the reaction, 2 moles of the intermediate are produced. what is the enthalpy value for this step of the reaction?

a. -286 kj
b. 572 kj
c. 286 kj
d. -572 kj

Explanation:

Step1: Recall the formula for total enthalpy

The total enthalpy ($\Delta H_{total}$) is the enthalpy of formation per - mole ($\Delta H_f$) times the number of moles ($n$). The formula is $\Delta H_{total}=n\times\Delta H_f$.

Step2: Substitute the given values

We are given that $n = 2$ moles and $\Delta H_f=- 286$ kJ/mol. So, $\Delta H_{total}=2\ mol\times(-286\ kJ/mol)$.

Step3: Calculate the result

$\Delta H_{total}=-572$ kJ.

Answer:

D. -572 kJ