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2 years ago

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Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial ch

emist studying this reaction fills a flask with of sulfur dioxide gas and of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be . Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to significant digits.

1 answer:

Inessa [10]2 years ago

8 0

Answer:

The answer is " $\bold{4.97 \times 10^{-2}}$ "

Explanation:

Please find the complete question in the attached file.

Equation:

$2SO_2+O_2 \leftrightharpoons 2SO_3$

at $t=0 3.3 \ \ \ \ \ \ \ \ \ \ 0.79$

at equilibrium $3.3-p \ \ \ \ \ \ \ \ \ \ 0.79 - \frac{P}{2} \ \ \ \ \ \ \ \ \ \ \ \ P$

$p= 0.47 \ \ atm\\\\SO_2=3.3-0.47 = 2.83 \ \ atm\\\\O_2= 0.74 -\frac{0.47}{2}=0.74-0.235=0.555 \ atm\\\\K_P=\frac{[PSO_3]^2}{[PSO_2]^2[PO_2]}\\\\$

$=\frac{0.47^2}{2.83^2\times 0.555}\\\\=4.97 \times 10^{-2}$

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<u>Answer:</u> The unknown salt is NaF

<u>Explanation:</u>

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<u>At eqllm:</u> 0.1-x x x

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The expression of $K_b$ for above equation follows:

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Putting values in above expression, we get:

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Putting values in above equation, we get:

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So, the calculated $K_a$ is approximately equal to the $K_a$ of HF

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