(B) The overall reaction is the sum of the two given equilibrium steps:Step $1$: $Ag^{+} + NH_3 \rightleftharpoons [Ag(NH_3)]^{+}$,$K_1 = 1.6 \times 1

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(B) The overall reaction is the sum of the two given equilibrium steps:Step $1$: $Ag^{+} + NH_3 \rightleftharpoons [Ag(NH_3)]^{+}$,$K_1 = 1.6 \times 10^3$Step $2$: $[Ag(NH_3)]^{+} + NH_3 \rightleftharpoons [Ag(NH_3)_2]^{+}$,$K_2 = 6.8 \times 10^3$Adding these two equations gives the net reaction:$Ag^{+} + 2 NH_3 \rightleftharpoons [Ag(NH_3)_2]^{+}$The equilibrium constant $(K_{net})$ for the net reaction is the product of the equilibrium constants of the individual steps:$K_{net} = K_1 \times K_2$$K_{net} = (1.6 \times 10^3) \times (6.8 \times 10^3)$$K_{net} = 10.88 \times 10^6 = 1.088 \times 10^7$

Class 11 Chemistry 1 Equilibrium: Chemical Equilibrium Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

Easy

Observe the following equations:
$Ag^{+} + NH_3 \rightleftharpoons [Ag(NH_3)]^{+}$,$K_1 = 1.6 \times 10^3$
$[Ag(NH_3)]^{+} + NH_3 \rightleftharpoons [Ag(NH_3)_2]^{+}$,$K_2 = 6.8 \times 10^3$
The equilibrium constant for the following reaction,$Ag^{+} + 2 NH_3 \rightleftharpoons [Ag(NH_3)_2]^{+}$ is

AP EAMCET 2019 All AP EAMCET

A
$6.008 \times 10^3$
B
$1.088 \times 10^7$
C
$1.088 \times 10^6$
D
$1.028 \times 10^3$

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1 Equilibrium: Chemical Equilibrium

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

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Match the items in List-$X$ with List-$Y$ and select the correct option.

List-$X$ List-$Y$

$(A)$ Active mass $(i)$ $\Delta n = 0$

$(B)$ Equilibrium constant $(ii)$ Molar concentration

$(C)$ $A + \text{Heat} \rightleftharpoons B$ $(iii)$ Van't Hoff equation

$(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)}$ $(iv)$ Favoured by increase in temperature

$(v)$ Chemical equilibrium

Medium

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For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,what is the relationship between $\Delta H$ and $\Delta E$?

MediumAIPMT 2002

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In a closed vessel at $448^{\circ} C$,$0.5 \ mol$ of $H_2$ and $0.5 \ mol$ of $I_2$ react to form hydrogen iodide.
Reaction: $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,$K_c = 50$.
$(i)$ Calculate the moles of $I_2$ that remain unreacted at equilibrium.
$(ii)$ Calculate $K_p$.

Difficult

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$2$ moles each of $A$ and $B$ were taken in a container and the following reaction takes place: $2 \ A_{(g)} + B_{(g)} \rightleftharpoons 2 \ C_{(g)} + D_{(g)}$. When the system attains equilibrium,which of the following is true?

Medium

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For the reaction $XCO_{3(s)} \rightleftharpoons XO_{(s)} + CO_{2(g)},$ $K_p = 1.642 \text{ atm}$ at $727^{\circ}C.$ If $4 \text{ moles}$ of $XCO_{3(s)}$ were placed into a $50 \text{ L}$ container and heated to $727^{\circ}C,$ what mole percent of the $XCO_3$ remains unreacted at equilibrium?

Difficult

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List-$X$	List-$Y$
$(A)$ Active mass	$(i)$ $\Delta n = 0$
$(B)$ Equilibrium constant	$(ii)$ Molar concentration
$(C)$ $A + \text{Heat} \rightleftharpoons B$	$(iii)$ Van't Hoff equation
$(D)$ $2A_{(g)} + B_{(g)} \rightleftharpoons 3C_{(g)}$	$(iv)$ Favoured by increase in temperature
	$(v)$ Chemical equilibrium

Observe the following equations:$Ag^{+} + NH_3 \rightleftharpoons [Ag(NH_3)]^{+}$,$K_1 = 1.6 \times 10^3$$[Ag(NH_3)]^{+} + NH_3 \rightleftharpoons [Ag(NH_3)_2]^{+}$,$K_2 = 6.8 \times 10^3$The equilibrium constant for the following reaction,$Ag^{+} + 2 NH_3 \rightleftharpoons [Ag(NH_3)_2]^{+}$ is

Similar Questions

For the reaction $N_2 + 3H_2 \rightleftharpoons 2NH_3$,what is the relationship between $\Delta H$ and $\Delta E$?

In a closed vessel at $448^{\circ} C$,$0.5 \ mol$ of $H_2$ and $0.5 \ mol$ of $I_2$ react to form hydrogen iodide.Reaction: $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,$K_c = 50$.$(i)$ Calculate the moles of $I_2$ that remain unreacted at equilibrium.$(ii)$ Calculate $K_p$.

$2$ moles each of $A$ and $B$ were taken in a container and the following reaction takes place: $2 \ A_{(g)} + B_{(g)} \rightleftharpoons 2 \ C_{(g)} + D_{(g)}$. When the system attains equilibrium,which of the following is true?

For the reaction $XCO_{3(s)} \rightleftharpoons XO_{(s)} + CO_{2(g)},$ $K_p = 1.642 \text{ atm}$ at $727^{\circ}C.$ If $4 \text{ moles}$ of $XCO_{3(s)}$ were placed into a $50 \text{ L}$ container and heated to $727^{\circ}C,$ what mole percent of the $XCO_3$ remains unreacted at equilibrium?

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Observe the following equations:
$Ag^{+} + NH_3 \rightleftharpoons [Ag(NH_3)]^{+}$,$K_1 = 1.6 \times 10^3$
$[Ag(NH_3)]^{+} + NH_3 \rightleftharpoons [Ag(NH_3)_2]^{+}$,$K_2 = 6.8 \times 10^3$
The equilibrium constant for the following reaction,$Ag^{+} + 2 NH_3 \rightleftharpoons [Ag(NH_3)_2]^{+}$ is

In a closed vessel at $448^{\circ} C$,$0.5 \ mol$ of $H_2$ and $0.5 \ mol$ of $I_2$ react to form hydrogen iodide.
Reaction: $H_{2(g)} + I_{2(g)} \rightleftharpoons 2HI_{(g)}$,$K_c = 50$.
$(i)$ Calculate the moles of $I_2$ that remain unreacted at equilibrium.
$(ii)$ Calculate $K_p$.