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For the decomposition of A to B and C A(n) B(g) + C(g) how will the reaction respond to each of the following changes at equilibrium? Drag the appropriate items to their respective bins. double the concentration of B and haive the double the concentrations add more A double the container volume double the concentrations of both products and then of both products double the container volume of C double the concentrations of both products and then quadruple the container volume Leftward shift No shift Rightward shift
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rt B For the reaction of A and B forming C A(g) B(a)2C() how will the reaction respond to each of the following changes at eq

A (s) ---------> B (g) + C (g)

Q = [B][C]

1) concentration of B is doubled and halve the concentration of C . then no shift

2) here Q < K then equilibrium shifts to right side

3) here A is solid so no shift if it is added

4) if double the concentration of products then Q > K. then equilibrium shifts to left side

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