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 E1/7 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