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Question

If the equilibrium constant for the reaction:
N2(g)+3H2(g)2NH3(g)
at 750K is 49, then the equilibrium constant for the reaction,
NH3(g)12N2(g)+32H2(g)
at the same temperature is:

A
1/49
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B
49
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C
7
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D
492
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E
1/7
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Solution

The correct option is E 1/7
If the equilibrium constant for the reaction:
N2(g)+3H2(g)2NH3(g).....(1)
at 750K is 49, then the equilibrium constant for the reaction,
NH3(g)12N2(g)+32H2(g).....(2)
at the same temperature is 1/7.
When reaction (1) is reversed and divided by 2, the reaction (2) is obtained.
K2=1K1
K2=149
K2=17

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