Question

The decomposition of ZnCO3(s) into ZnO(s) and CO2(g) at constant pressure requires the addition of 71.5 kJ of heat per mole of ZnCO3. You may want to reference (Pages 177 - 178) Section 5.4 while completing this problem. Part APart complete Write a balanced equation for the reaction. Express your answer as a chemical equation. Identify all of the phases in your answer. ZnCO3(s)→ZnO(s)+CO2(g) Previous Answers Correct The reactant and products of the decomposition reaction are given in the introduction. ZnCO3(s) is broken down into ZnO(s) and CO2(g). Part B What is the enthalpy of the reaction above?

Answer 1

Step-by-step explanation:

A) ZnCO3 (s) --> ZnO(s) + CO2(g)

B) ΔH = 71,5kJ/mole

The enthalpy is positive (ΔH > 0) because this reaction absorb heat to occur

Answer 2

For A: The chemical equation is
`ZnCO_3(s)\rightarrow ZnO(s)+CO_2(g)`

For B: The enthalpy of the reaction is 71.5 kJ/mol

Step-by-step explanation:

• For A:

Decomposition reaction is defined as the reaction in which a single chemical substance breaks down into two or more smaller substances.

The chemical equation for the decomposition of zinc carbonate follows:

`ZnCO_3(s)\rightarrow ZnO(s)+CO_2(g)`

• For B:

Endothermic reactions are defined as the reactions in which energy is absorbed in the reaction. The enthalpy change of the reaction is positive.

Exothermic reactions are defined as the reactions in which energy is released in the reaction. The enthalpy change of the reaction is negative.

In the above reaction, the heat is added. So, the reaction is endothermic in nature.

Amount of heat added per mole of zinc carbonate = 71.5 kJ

Hence, the enthalpy of the reaction is 71.5 kJ/mol