The reaction below is at dynamic equilibrium. mc004-1.jpg Which statement is true for the equilibrium system? The concentration
2 answers:
Answer: The correct statement is :
'The rate of the forward reaction equals the rate of the reverse reaction'.
Explanation:
Dynamic Equilibrium : A chemical reaction is said to be in equilibrium if the concentration of reactant and products become constant. The rate of the reaction going forward is equal to the rate of reaction going backward. Hence, reversible reaction.
Only rates of the backward and forward reaction are equal not the the concentrations.
According to the given reaction:
Rate of the decomposition of ammonia is equal to the rate of formation of ammonia from hydrogen gas and nitrogen gas.
From the given statements the correct statement is:'
The rate of the forward reaction equals the rate of the reverse reaction'.
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The solubility equilibrium of :
[tex] CaCrO_{4}(aq)<===>Ca^{2+}(aq) + CrO_{4}^{2-}(aq)\\
Q_{sp}=[Ca^{2+}][CrO_{4}^{2-}]\\
= (0.0200 M)(0.0300 M) \\
= 0.0006
Ksp (0.00071) > Qsp (0.0006). So, <u>no precipitate would form</u>.
