Write the relationship between the rate of disapperance of H2C2O4 (aq) and the rate of apperance on Mn ^2+ (aq) for the reaction represented by the following equation.
2MnO4^-(aq)+ 5H2C2O4 (aq)+6H3)^+(aq)
-->10CO2(g)+2Mn^2+ (aq)+14H2) (l)
To determine the relationship between the rate of disappearance of H2C2O4 (aq) and the rate of appearance of Mn^2+ (aq) for the given reaction, we need to analyze the stoichiometry of the reactants and products.
The balanced chemical equation for the reaction is:
2MnO4^-(aq) + 5H2C2O4 (aq) + 6H3O^+(aq) --> 10CO2(g) + 2Mn^2+(aq) + 14H2O(l)
From the equation, we can see that for every 5 moles of H2C2O4 reacting, 2 moles of Mn^2+ are formed. Therefore, the ratio of the rate of change for H2C2O4 to Mn^2+ can be expressed as:
-(1/5) * (d[H2C2O4]/dt) : (1/2) * (d[Mn^2+]/dt)
This means that as the concentration of H2C2O4 decreases, the concentration of Mn^2+ increases. The rate at which H2C2O4 is consumed is negative because it is disappearing, while the rate at which Mn^2+ is formed is positive because it is being produced.
It is important to note that the relationship between the rate of disappearance of H2C2O4 and the rate of appearance of Mn^2+ is based on the stoichiometry of the reaction.