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Question

1 mole of $$H_{ 2 }$$, 2 moles of $$I_{ 2 }$$ and 3 moles of HI were taken in 1 litre flask. The equilibrium constant of the reaction:
     
        $$H_{ 2(g) }+I_{ 2(g) }\rightleftharpoons 2HI_{ (g) }$$ 

is 50 at $${ 330 }^{ o }C$$. The concentration of HI at equilibrium is: 


A
0.3
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B
1.6
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C
4.4
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D
2.7
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Solution

The correct option is C 4.4
$$ \begin{aligned} 2 t &=\dfrac{(3)^{2}}{(2)} \\ &=4.5 \end{aligned} $$

 $$ \mathrm{Keq}=\dfrac{(3+2 \mathrm{~x})^{2}}{(1-2x)(2-x)}=\dfrac{[H I]^{2}}{\left.\left[H_{2}\right] C I_{2}\right]} $$

 $$ \begin{array}{r} 50=\dfrac{(2 x+3)^{2}}{(1-x)(2-x)} \\ x=0.7 \end{array}$$

 $$ \begin{aligned} \text { at equilibrium concentration of } & H I=3+2 x \\ &=3+2 \times 0.7 \\ &=\underline{4.4} \end{aligned}$$

2004458_1018512_ans_815ecf7064814cdba87c4d6feadc0abc.jpeg

Chemistry

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