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When {3.06}{g} of solid {N}{H}_{{{4}}}{H}{S} is introduced int

Question

When $3.06 g$ of solid $N H_{4} H S$ is introduced into a two-litre evacuated flask at $27^{\circ} C, 30 %$ of the solid decomposes into gaseous ammonia and hydrogen sulphide. (i) Calculate $K_{c}$ and $K_{p}$ for the reaction at $27^{\circ} C$ . (ii) What would happen to the equilibrium when more solid $N H_{4} H S$ is introduced into the flask?

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When

3.06 g

of solid

N H_{4} H S

is introduced into a two-litre evacuated flask at

27^{\circ} C, 30 %

of the solid decomposes into gaseous ammonia and hydrogen sulphide. (i) Calculate

K_{c}

and

K_{p}

for the reaction at

27^{\circ} C

. (ii) What would happen to the equilibrium when more solid

N H_{4} H S

is introduced into the flask?

12 mins ago

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Text solutionVerified

Answer: NA

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Question Text	When $3.06 g$ of solid $N H_{4} H S$ is introduced into a two-litre evacuated flask at $27^{\circ} C, 30 %$ of the solid decomposes into gaseous ammonia and hydrogen sulphide. (i) Calculate $K_{c}$ and $K_{p}$ for the reaction at $27^{\circ} C$ . (ii) What would happen to the equilibrium when more solid $N H_{4} H S$ is introduced into the flask?
Answer Type	Text solution:1
Upvotes	150