SSCE HSC Chemistry Alcohols: Question 32 (iii) In most respo

Question 32 (iii) In most responses, candidates correctly stated that temperature alone could change the value of the equilibrium constant - HSC - SSCE Chemistry - Question 32 - 2012 - Paper 1

Question 32

Question 32 (iii) In most responses, candidates correctly stated that temperature alone could change the value of the equilibrium constant. (c)(i) In better respon... show full transcript

Worked Solution & Example Answer:Question 32 (iii) In most responses, candidates correctly stated that temperature alone could change the value of the equilibrium constant - HSC - SSCE Chemistry - Question 32 - 2012 - Paper 1

Step 1

(iii) In most responses, candidates correctly stated that temperature alone could change the value of the equilibrium constant.

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Answer

The temperature is a crucial factor that influences the position of equilibrium in a chemical reaction. According to Le Chatelier's principle, if the temperature of a reaction is changed, the system will adjust to counteract the change and establish a new equilibrium state. Specifically, if a reaction is exothermic, increasing the temperature will shift the equilibrium to the left, favoring the reactants and thus changing the equilibrium constant (K). Conversely, decreasing the temperature will favor the production of products and will increase the equilibrium constant.

Step 2

(c)(i) In better responses, candidates correctly described the two-step process for making sulphuric acid from SO₃, and supported this description with correctly balanced equations that included appropriate states, showing oleum as a liquid.

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Answer

The two-step process for synthesizing sulphuric acid (H₂SO₄) from sulfur trioxide (SO₃) includes the following steps:

Sulfur Trioxide to Oleum: The first step involves the reaction of SO₃ with sulfuric acid (H₂SO₄) to produce oleum (H₂S₂O₇).

$\text{SO}_3 (g) + \text{H}_2\text{SO}_4 (l) \rightarrow \text{H}_2\text{S}_2\text{O}_7 (l)$
Conversion of Oleum to Sulfuric Acid: The oleum can then be mixed with water to produce concentrated sulfuric acid:

$\text{H}_2\text{S}_2\text{O}_7 (l) + \text{H}_2\text{O} (l) \rightarrow 2 \text{H}_2\text{SO}_4 (l)$

This two-step process is essential for producing sulfuric acid in a controlled manner, ensuring optimal conditions and high yields.

Question 32 (iii) In most responses, candidates correctly stated that temperature alone could change the value of the equilibrium constant - HSC - SSCE Chemistry - Question 32 - 2012 - Paper 1

Worked Solution & Example Answer:Question 32 (iii) In most responses, candidates correctly stated that temperature alone could change the value of the equilibrium constant - HSC - SSCE Chemistry - Question 32 - 2012 - Paper 1

(iii) In most responses, candidates correctly stated that temperature alone could change the value of the equilibrium constant.

(c)(i) In better responses, candidates correctly described the two-step process for making sulphuric acid from SO₃, and supported this description with correctly balanced equations that included appropriate states, showing oleum as a liquid.

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