Consider the following reactions at equilibrium and determine which of the indic

Question

Consider the following reactions at equilibrium and determine which of the indicated changes will cause the reaction to proceed to the right

1) 2 H2O(g) <---> 2 H2(g) + O2(g) (remove water)

2) H2(g) + I2(g) <----> 2 HI(g) (add iodine)

3) CaCO3(s) <----> CaO(s) + CO2(g) (add CaCO3)

4) N2(g) + O2(g) <-----> 2NO (g) (remove oxygen)

5) BaO(s) + SO3(g) <-----> BaSO4 (s) (add SO3)

The answer is 2 and 5.

Will someone explain to me how this is figured out? How could I look at this and understand that the answer is 2 and 5.

Explanation / Answer

yes your answer is correct 2 nnd 5

in any equilibrium reactions if we increase the reactants reaction proceeds to decrease the concentration of reactants.so reaction will proceed to right.

in above 2 and 5 in both the cases we are increasing the concentration of reactants so reaction proceeds right.

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