The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....

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The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....

The equilibrium constant for the reaction: H₂(g) + I₂(g) <--> 2HI(g) is 54 at 700 K.

A mixture of H₂, I₂ and HI, each at 0.020 M, was introduced into a container at 700 K. Which of the following is true?

At equilibrium, [H₂] = [I₂] = [HI].
	No net change occurs because the system is at equilibrium.
	The reaction proceeds to the left producing more H₂(g) and I₂(g).
	The reaction proceeds to the right producing more HI(g).
	At equilibrium, [HI] = 0.010 M.

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Answer 1

Answer #1

2HI Initial 0.02 0.02 0.02 Atequilibium- 0.02-x 0.02- O.02 27x K 54 o.01 (0.02) (o.02) Q K hence to eael eauilibviuM produet

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The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....

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The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....