A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a...

A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a 2.00 L vessel at 700 K . These substances react as follows:

H2(g)+Br2(g)⇌2HBr(g)

At equilibrium the vessel is found to contain 0.566 g of H2.

1A)

Calculate the equilibrium concentration of Br2

1B)

Calculate Kc.

1C)

Calculate the equilibrium constant Kp for this reaction, given the following information (at 299 K ):
2NO(g)+Br2(g)⇌2NOBr(g) Kc=1.8
2NO(g)⇌N2(g)+O2(g) Kc=2.3×10^30

Thank you in advance!

Expert Solution

queen_honey_blossom answered 2 years ago

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