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Consider the reaction: A(g) hArr B(g)+...

Consider the reaction:
`A(g) hArr B(g)+C(g)`
When the system is at equilibrium at `200^(@)C`, the concentrations are found to be:
`[A]=0.20 M, [B]=0.30 M, [C]=0.30 M`
a. If the volume of the container is suddenly doubled at `200^(@)C`, find the equilibrium concentrations.
b. If the volume of the container is suddenly halved (instead of being doubled in part (i) at `200^(@)C`, find the equilibrium concentrations.

Text Solution

Verified by Experts

`{:(,A,hArr,B,+,C),("At equilibrium",0.2,,0.3,,0.3):}`
`K_(c )=((0.3)(0.3))/(0.2)=9/20`
a. When volume is doubled `(i.e. rarr 2V)`
`rArr [A]=0.1, [B]=0.15=[C]`
`Q_(c )=((0.15)(0.15))/(0.1)=9/40rArr Q_(c ) lt K_(c )`
Reaction goes forward.
`K_(c )=9/20=((0.15+x)(0.15+x))/((0.1-x))`
solve for `x, x~~0.03`
`[A]=0.1-0.03=0.07 M`
`[B]=[C]=0.15+0.03=0.18 M`
b. When volume is halved `(i.e. Vrarr V//2)`
`rArr [A]=0.4, [B]=[C]=0.6`
`Q_(c )=(0.6xx0.6)/(0.4)=9/10rArr Q_(c ) gt K_(c )`
Reaction goes backward.
`K_(c )=9/20=((0.6-x)^(2))/((0.4+x))`
Solve for `x, x~~0.12`
`[A]=0.4+0.12=0.16 M`
`[B]=[C]=0.6-0.12=0.48 M`
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