The following unbalanced equation represents a reaction that occurs in basic solution: MnO42 - + C2O42 - → MnO2 + CO32 - How many moles of MnO42 - are required to produce 1 mole of CO32-?

Question

Jimmy Wall

Chemistry

10 January, 01:36

The following unbalanced equation represents a reaction that occurs in basic solution: MnO42 - + C2O42 - → MnO2 + CO32 - How many moles of MnO42 - are required to produce 1 mole of CO32-?

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Answers (1)

Know the Answer?

Scooby · Answer 1

0.5

Explanation:

To be able to get the answer, we need to balance the ionic equation.

MnO42 - + C2O42 - - -> MnO2 + 2CO32-

Firstly we balance mole-wise and then charge-wise.

Let's check If the equation is balanced.

We can see that the equation is balanced both mole-wise and charge wise

From the balanced equation we can see that 1 mole of MnO42 - produced 2 moles of CO32-.

This means x moles of MnO42 - will produce 1 mole of CO32-.

To get x, we simply make a cross multiplication.

2x = 1 and x = 0.5

Hence 0.5 mole of MnO42 - will produce 1 mole of CO32-