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ArbitrLikvidat [17]

3 years ago

12

When the reaction 2H₂S(g) ↔️2H₂(g) + S2(g) is carried out at 1065°C, Kp = 0.012. Starting with pure H₂S at 1065°C, what must the

initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g)?

1 answer:

mario62 [17]3 years ago

8 0

Answer:

Answer is in the attachment.

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Read 2 more answers

Convert 150 kPa to atmospheres. *

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Answer: 1.48 atmosphere

Explanation:

Pressure in kilopascal = 150

Pressure in atmosphere = ?

Recall that 1 atmosphere = 101.325 kilopascal

Hence, 1 atm = 101.325 kPa

Z atm = 150 kPa

To get the value of Z, cross multiply

150 kPa x 1 atm = 101.325 kPa x Z

150 kPa•atm = 101.325 kPa•Z

Divide both sides by 101.325 kPa

150 kPa•atm/101.325 kPa = 101.325 kPa•Z/101.325 kPa

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Consider the insoluble compound nickel(II) hydroxide , Ni(OH)2 . The nickel ion also forms a complex with cyanide ions . Write a

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Answer: Equilibrium constant for this reaction is $2.8 \times 10^{15}$ .

Explanation:

Chemical reaction equation for the formation of nickel cyanide complex is as follows.

$Ni(OH)_{2}(s) + 4CN^{-}(aq) \rightleftharpoons [Ni(CN)_{4}^{2-}](aq) + 2OH^{-}(aq)$

We know that,

K = $K_{f} \times K_{sp}$

We are given that, $K_{f} = 1.0 \times 10^{31}$

and, $K_{sp} = 2.8 \times 10^{-16}$

Hence, we will calculate the value of K as follows.

K = $K_{f} \times K_{sp}$

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= $2.8 \times 10^{15}$

Thus, we can conclude that equilibrium constant for this reaction is $2.8 \times 10^{15}$ .

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