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# Finding equilibrium constant using pressure changes?

## At 273$K$ 1 mole of ammonia was present. When temperature gone up to 819$K$, pressure increased 5.61 times with equilibrium of $2 N {H}_{3} r i g h t \le f t h a r p \infty n s {N}_{2} + 3 {H}_{2}$ $\circ$ Calculate the equilibrium constant $\circ$ How many moles of ${H}_{2}$ is present in equilibrium $\circ$ When volume decreases 4 times, find rates of forward and backward reactions?

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