solve under rate of reaction:
1)Mno4^- + Fe2^+=Mn2^+ + Fe3^+
rate of reactions
Fe^2+ + Cr2O7^2- » Cr^3+ +Fe^3+
You need to provide more information than that and make your question clearer. I don't know what you're asking.
To solve the rate of reaction for the given reaction:
MnO4^- + Fe2+ -> Mn2+ + Fe3+
You need to know two things:
1) The balanced chemical equation for the reaction.
2) The rate law for the reaction.
1) Balanced Chemical Equation:
First, let's balance the chemical equation.
MnO4^- + Fe2+ -> Mn2+ + Fe3+
To balance the equation, count the number of each type of atom on both sides of the equation. Adjust the coefficients so that the number of each type of atom is equal on both sides.
MnO4^- + 5Fe2+ -> Mn2+ + 5Fe3+
Now the equation is balanced.
2) Rate Law:
Next, let's determine the rate law for the reaction.
The rate law shows how the rate of the reaction depends on the concentrations of the reactants. It can be determined experimentally.
Assuming the reaction proceeds through a single elementary step, the rate law can be expressed as:
rate = k[Fe2+]^a[MnO4^-]^b
Here, k is the rate constant, [Fe2+] is the concentration of Fe2+, and [MnO4^-] is the concentration of MnO4^-.
The exponents 'a' and 'b' need to be determined through experimentation.
Overall, to fully solve the rate of reaction, you would need the experimental values for the rate constant (k), as well as the values of 'a' and 'b' in the rate law equation.