The decomposition of water can be represented by the chemical equation
$$2H_2O(l) \rightleftharpoons 2H_2(g) + O_2(g)\quad \Delta H = +571.8 \text{ kJ mol}^{-1}$$
From this equation, it can be concluded that the formation of two moles of liquid water from gaseous hydrogen and oxygen is an
A - VCE - SSCE Chemistry - Question 13 - 2002 - Paper 1
Question 13
The decomposition of water can be represented by the chemical equation
$$2H_2O(l) \rightleftharpoons 2H_2(g) + O_2(g)\quad \Delta H = +571.8 \text{ kJ mol}^{-1}$$
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Worked Solution & Example Answer:The decomposition of water can be represented by the chemical equation
$$2H_2O(l) \rightleftharpoons 2H_2(g) + O_2(g)\quad \Delta H = +571.8 \text{ kJ mol}^{-1}$$
From this equation, it can be concluded that the formation of two moles of liquid water from gaseous hydrogen and oxygen is an
A - VCE - SSCE Chemistry - Question 13 - 2002 - Paper 1
Step 1
Identify the Process Type
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Answer
To determine if the process is exothermic or endothermic, we look at the sign of the enthalpy change, ( \Delta H ). Since ( \Delta H = +571.8 \text{ kJ mol}^{-1} ), this indicates that heat is absorbed during the formation of water, which makes it an endothermic process.
Step 2
Determine Heat Absorption
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Answer
The positive value of ( \Delta H ) indicates that for the formation of 2 moles of water, 571.8 kJ of energy is absorbed. Therefore, the correct conclusion is that this process involves absorbing 571.8 kJ of heat energy.
Step 3
Select the Correct Answer
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Answer
Given the analysis, the answer is C. endothermic process absorbing 571.8 kJ of heat energy.
