A mixture of 1.374g of H2 and 70.31g of Br2 is heated in a 2.00L vessel at 700K

Question

A mixture of 1.374g of H2 and 70.31g of Br2 is heated in a 2.00L vessel at 700K . These substances react as follows:
H2(g)+Br2(g)?2HBr(g)
At equilibrium the vessel is found to contain 0.566 g of H2.
Part A
Calculate the equilibrium concentration of H2.
Express your answer using three significant figures.
Part B
Calculate the equilibrium concentration of Br2.
Express your answer using three significant figures.
Part C
Calculate the equilibrium concentration of HBr.
Express your answer using three significant figures.
Part D
Calculate Kc.
Express your answer using two significant figures.

Explanation / Answer

H2 +Br2 ------>2 HBr

[H2] =1.374/2x2 =0 .3435 M

[Br2] = 70.31/2x160 = 0.2197M part A- At equlibirium concentration of H2 = 0.566/4 =0.1415M

x=.3435-0.1415=0.202

H2 + Br2 ----->2 HBr

0.3435 0.2197    0    initial concentration

-x        -x            2x     change

0.1415 0.0177     0.404   equlibirium concentration

equlibirium concentration

[H2]=0.1415M

[Br2] = 0.0177M [HBr] =0.404M

Kc=[HBr]^2 /[H][Br]= [0.404]^2 / [0.1415][0.0177]=0.163216 / 2.50455x10^-3=65.16779

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