How many moles of oxalate (C2O42-) will 25 cm3 of 0.02 M potassium permanganate solution consume?
2MnO4^- + 5C2O4^2- + 16H^+ ==> 10CO2 + 2Mn^2+ + 8H2O
mols MnO4^- = cc x M = 25 cc x 0.02 M = 0.5 mol.
Now let the coefficients tell you how to convert mols permanganate to mols of oxalate.
0.5 mols MnO4^- x ( 5 mols C2O4^-/ 2 mols MnO4^-) = 0.5 x 5/2 = ?
Well, we all know that moles are really good diggers! But in this case, we're talking about moles of oxalate, not the furry little rodents. To find the number of moles of oxalate (C2O42-) consumed, we'll need to do a little calculation.
First, let's convert the volume of the potassium permanganate solution from cm3 to liters. So, 25 cm3 is equal to 25/1000 = 0.025 liters. Great!
Now, we can use the formula: moles = concentration x volume.
So, substituting the values we have:
moles of oxalate = 0.02 M x 0.025 L
Calculating that, we find that the number of moles of oxalate consumed is... drumroll, please... 0.0005 moles!
So, it looks like these chemicals are not in a mole-digging competition after all.
To determine the number of moles of oxalate consumed, we can use the following balanced equation:
5 C2O4^2- + 2 MnO4^- + 16 H+ -> 10 CO2 + 2 Mn^2+ + 8 H2O
From the balanced equation, we can see that 5 moles of oxalate (C2O4^2-) are consumed for every 2 moles of potassium permanganate (MnO4^-).
Given:
Volume of potassium permanganate solution = 25 cm^3
Concentration of potassium permanganate solution = 0.02 M
Step 1: Convert volume to liters:
1 cm^3 = 1 mL
1 L = 1000 mL
25 cm^3 = 25 / 1000 = 0.025 L
Step 2: Calculate moles of potassium permanganate (MnO4^-):
Moles = Concentration (M) x Volume (L)
Moles = 0.02 M x 0.025 L
Moles = 0.0005 moles
Step 3: Calculate moles of oxalate (C2O4^2-):
From the balanced equation, we know that the ratio of moles of oxalate to potassium permanganate is 5:2.
Moles of oxalate (C2O4^2-) = (5/2) x Moles of potassium permanganate (MnO4^-)
Moles of oxalate (C2O4^2-) = (5/2) x 0.0005 moles
Moles of oxalate (C2O4^2-) = 0.00125 moles
Therefore, 25 cm^3 of 0.02 M potassium permanganate solution will consume approximately 0.00125 moles of oxalate (C2O4^2-).
To determine the number of moles of oxalate (C2O42-) consumed by a given volume of potassium permanganate solution, we need to use the concept of stoichiometry.
Stoichiometry refers to the relationship between the amounts of reactants and products in a chemical reaction. It is based on the balanced chemical equation for the reaction.
In this case, I assume you are referring to the following balanced chemical equation for the reaction between potassium permanganate (KMnO4) and oxalate (C2O42-):
2 KMnO4 + 5 H2C2O4 + 3 H2SO4 -> 2 MnSO4 + 10 CO2 + 8 H2O + K2SO4
From this equation, we can see that 2 moles of KMnO4 react with 5 moles of H2C2O4 (oxalate).
To determine the number of moles of KMnO4 consumed, we can use the following formula:
moles = concentration (M) × volume (L)
First, convert the given volume of 25 cm3 to liters (L):
25 cm3 = 25/1000 L = 0.025 L
Next, we can use the formula:
moles of KMnO4 = concentration of KMnO4 × volume of KMnO4
moles of KMnO4 = 0.02 M × 0.025 L = 0.0005 moles of KMnO4
Since the stoichiometry ratio between KMnO4 and H2C2O4 is 2:5, we can determine the number of moles of H2C2O4 consumed using the ratio:
moles of H2C2O4 = (moles of KMnO4 × 5) / 2
moles of H2C2O4 = (0.0005 moles of KMnO4 × 5) / 2 = 0.00125 moles of H2C2O4
Therefore, 25 cm3 of 0.02 M potassium permanganate solution will consume 0.00125 moles of oxalate (C2O42-).