# Can someone explain how to do this? Consider the following equation: #"2ZnS"# + #"3O"_2# #rarr# #"2ZnO"# + #"2SO"_2# , ΔH° = - 878.2kJ. What is the enthalpy change when 0.96 g ZnO is produced?

The enthalpy change in the production of 0.96g of zinc oxide is

-5.15 kJ.

A total of 878.2 kJ of energy are released into the environment when 2 moles of ZnS and 2 moles of ZnO are produced.

Moles to grams conversion:

Ar (O) = 16 and Ar (Zn) = 65.28 and Ar (S) = 32.06.

Thus

Thus, 878.2 kJ of energy are produced by 162.56 g of ZnO.

Thus, 872.8/162.56 = 5.37 kJ of energy are produced by 1g of ZnO.

Thus, 5.37 x 0.96 = 5.15 kJ of energy will be produced by 0.96 g of ZnO.

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Use the given enthalpy change and the balanced equation to find the enthalpy change for the given mass of ZnO.

- Calculate moles of ZnO produced.
- Apply the stoichiometric coefficients from the balanced equation.
- Multiply moles of ZnO by the given enthalpy change.

[ \text{Enthalpy change} = \left( \frac{\text{moles of ZnO}}{\text{coefficient of ZnO}} \right) \times \text{ΔH°} ]

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