The anaesthetic, nitrous oxide, N2O, decomposes to form an equilibrium mixture of N2O, N2 and O2 according to the following equation - VCE - SSCE Chemistry - Question 6 - 2009 - Paper 1
Question 6
The anaesthetic, nitrous oxide, N2O, decomposes to form an equilibrium mixture of N2O, N2 and O2 according to the following equation.
2N2O(g) ⇌ 2N2(g) + O2(g)
At 2... show full transcript
Worked Solution & Example Answer:The anaesthetic, nitrous oxide, N2O, decomposes to form an equilibrium mixture of N2O, N2 and O2 according to the following equation - VCE - SSCE Chemistry - Question 6 - 2009 - Paper 1
Step 1
A. The equilibrium concentrations of N2 and O2 are equal at 25°C.
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Answer
This statement is not supported by the information given. The equilibrium constant K does not indicate that the concentrations of N2 and O2 are equal.
Step 2
B. The equilibrium concentration of N2O is higher at 25°C than at 40°C.
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Answer
This is true based on the shift in equilibrium. Since K is significantly higher at 25°C compared to 40°C, it indicates that more N2O is present at the lower temperature.
Step 3
C. N2O is less stable at the higher temperature.
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Answer
This statement can be inferred from the equilibrium constant values. A decrease in K at a higher temperature suggests that N2O is less stable at 40°C.
Step 4
D. The forward reaction is exothermic.
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The decrease in K with an increase in temperature provides evidence that the forward reaction is exothermic, as increasing temperature favors the endothermic reverse reaction.
