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Wittaler [7]
3 years ago
13

2 SO2(g) + O2(g) 2 SO3(g) Assume that Kc = 0.0680 for the gas phase reaction above. Calculate the corresponding value of Kp for

this reaction at 84.5°C.
Chemistry
1 answer:
son4ous [18]3 years ago
6 0

Answer: The corresponding value of K_p for this reaction at 84.5°C is 0.00232

Explanation:

2SO_2(g)+O_2(g)\rightarrow 2SO_3(g)

Relation of with is given by the formula:

K_p=K_c(RT)^{\Delta ng}

where,

= equilibrium constant in terms of partial pressure = ?

K_c = equilibrium constant in terms of concentration = 0.0680

R = Gas constant = 0.0821\text{ L atm }mol^{-1}K^{-1}

T = temperature  =84.5^0C=(273+84.5)K=357.5K

\Delta n_g = change in number of moles of gas particles = n_{products}-n_{reactants}=2-3=-1

Putting values in above equation, we get:

K_p=0.0680\times (0.0821\times 357.5)^{-1}\\\\K_p=0.00232

Thus the corresponding value of K_p for this reaction at 84.5°C is 0.00232

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Answer:

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Explanation:

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Using Henderson equation to find pH of this buffer

            pH = pKa + log\frac{[Conjugate base]}{[Acid]}

or,               = 7.53  + log\frac{60 X 0.103}{8 X 0.296}

or,               = 7.53 + 0.4

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