Consider the following reactions at equilibrium and determine which of the indic
ID: 880913 • Letter: C
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.