(D) The decomposition reaction is: $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$Initial pressure: $P_{NH_3} = 0.50 \ atm$,$P_{H_2S} = 0 \ a

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(D) The decomposition reaction is: $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$Initial pressure: $P_{NH_3} = 0.50 \ atm$,$P_{H_2S} = 0 \ atm$At equilibrium,let the increase in pressure due to decomposition be $x \ atm$ for each gas.$P_{NH_3} = 0.50 + x$$P_{H_2S} = x$Total pressure $P_T = P_{NH_3} + P_{H_2S} = (0.50 + x) + x = 0.84 \ atm$$0.50 + 2x = 0.84$ $\Rightarrow 2x = 0.34$ $\Rightarrow x = 0.17 \ atm$Equilibrium pressures: $P_{NH_3} = 0.50 + 0.17 = 0.67 \ atm$ and $P_{H_2S} = 0.17 \ atm$$K_p = P_{NH_3} \times P_{H_2S} = 0.67 \times 0.17 = 0.1139 \approx 0.11$

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

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An amount of solid $NH_4HS$ is placed in a flask already containing ammonia gas at a certain temperature and $0.50 \ atm$ pressure. Ammonium hydrogen sulphide decomposes to yield $NH_3$ and $H_2S$ gases in the flask. When the decomposition reaction reaches equilibrium,the total pressure in the flask rises to $0.84 \ atm$. The equilibrium constant for $NH_4HS$ decomposition at this temperature is

AIEEE 2005 All AIEEE

A
$0.3$
B
$0.18$
C
$0.17$
D
$0.11$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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$4.0 \, mol$ of argon and $5.0 \, mol$ of $PCl_5$ are introduced into an evacuated flask of $100 \, L$ capacity at $610 \, K$. The system is allowed to equilibrate. At equilibrium,the total pressure of the mixture was found to be $6.0 \, atm$. The $K_p$ for the reaction is ...... [Given: $R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1}$]

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At $700 \, K$,the equilibrium constant $K_p$ for the reaction $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$ is $1.80 \times 10^{-3}$. The numerical value in $mol \, L^{-1}$ of $K_c$ for this reaction at the same temperature will be $(R = 8.314 \, J \, K^{-1} \, mol^{-1})$.

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For the reaction $P + Q \rightleftharpoons R + C$,the equilibrium constant $K_c$ is $10^{-2}$ and the forward rate constant $K_f$ is $10^{-1}$. The rate constant for the backward reaction $(K_b)$ will be:

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For the reaction $2Ag_2O_{(s)} \rightleftharpoons 4Ag_{(s)} + O_{2(g)}$,the partial pressure of $O_2$ is given by:

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For the chemical reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,$\Delta H^o$ of reaction can be determined from which one of the following plots?

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At $700 \, K$,the equilibrium constant $K_p$ for the reaction $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$ is $1.80 \times 10^{-3}$. The numerical value in $mol \, L^{-1}$ of $K_c$ for this reaction at the same temperature will be $(R = 8.314 \, J \, K^{-1} \, mol^{-1})$.

For the reaction $P + Q \rightleftharpoons R + C$,the equilibrium constant $K_c$ is $10^{-2}$ and the forward rate constant $K_f$ is $10^{-1}$. The rate constant for the backward reaction $(K_b)$ will be:

For the reaction $2Ag_2O_{(s)} \rightleftharpoons 4Ag_{(s)} + O_{2(g)}$,the partial pressure of $O_2$ is given by:

For the chemical reaction $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$,$\Delta H^o$ of reaction can be determined from which one of the following plots?

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