Question

Permanganate and oxalate ions react in an acidified solution according to the balanced equation above. How many moles of co2(g) are produced when 20. Ml of acidified 0. 20 m kmno4 solution is added to 50. Ml of 0. 10 m na2c2o4 solution?.

Answer 1

Answer:

There will be produced 0.01 moles of CO2

Explanation:

Step 1: Data given

volume of 0.20 M KMnO4 solution = 20 mL = 0.02 L

Volume of 0.10 M Na2C2O4 solution = 50 mL = 0.05 L

Step 2: The balanced equation

2 MnO4-(aq) + 5C2O4^2- (aq) + 16 H+ (aq) → 2 Mn^2+ (aq) + 10CO2 (g) + 8H2O (l)

Step 3: Calculate moles of KMnO4

moles KMnO4 = Molarity * volume

moles KMnO4 = 0.20 M * 0.02 L

moles KmnO4 = 0.004 moles

Step 4: Calculate moles of Na2C2O4

Moles Na2C2O4 = 0.10 M * 0.05 L

Moles Na2C2O4 = 0.005 moles

Step 5: Calculate limiting reactant

For 2 moles KMnO4 we need 5 moles Na2C2O4

Na2C2O4 is the limiting reactant

There will react 0.005 moles

KMnO4 is in excess. There will react 0.005 / 2.5 = 0.002 moles

Step 6: Calculate moles of CO2

For 2 moles KMnO4 we need 5 moles Na2C2O4, there will be produced 10 moles of CO2

For 0.005 moles of Na2C2O4 there will be produced 0.01 moles of CO2