The equilibrium constant, Kc, for the following reaction is 1.80Ã—10-2 at 698 K. 2HI(g) -->H2(g) + I2(g) Calculate the equilibrium concentrations...

80.2K

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Chemistry

The equilibrium constant, K_c, for the followingreaction is 1.80Ã—10^-2 at698 K.

2HI(g)-->H₂(g) +I₂(g)

Calculate the equilibrium concentrations of reactant and productswhen 0.257 moles of HI areintroduced into a 1.00 L vessel at 698K.
[HI] = M
[H₂] = M
[I₂] = M
The equilibrium constant, K_c, for the followingreaction is 83.3 at 500 K.

PCl₃(g) +Cl₂(g)-->PCl₅(g)

Calculate the equilibrium concentrations of reactant and productswhen 0.420 moles ofPCl₃ and 0.420 molesof Cl₂ are introduced into a 1.00 Lvessel at 500 K.
[PCl₃] = M
[Cl₂] = M
[PCl₅] = M

Answer & Explanation Solved by verified expert

4.4 Ratings (992 Votes)

Consider reaction2 HI g H2 g I2 gEquilibrium constant for above reaction is K c H2 I 2 HI 2 00180Lets use ICE tableM2 HI g H2 g I 2 gI0257C 2XXXE0257 2 XXXK c X X 0257 2 X 2 00180X 2 0257 2 X 2 00180Taking square root on See Answer

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[PCl₃]	=	M
[Cl₂]	=	M
[PCl₅]	=	M