Question

5SO2 + 2MnO4- + 2H205SO42- + 2Mn2+ + 4H+ Calculate the number of grams of SO2 in a sample of air if 7.37 mL of 0.008 M KMnO4 solution are required for the titration.

Answer 1

0.09536 g of SO2 in the sample of air

Step-by-step explanation:

The first step is to convert the volume of KMnO4 solution to moles. This can be done using the formula:

moles = Molarity x volume (in liters)

So,

moles = 0.008 M x (7.37 mL) x (1 L/1000 mL)

= 0.0000596 moles

Next, we need to find the ratio of moles of SO2 to moles of KMnO4 in the balanced equation:

5SO2 + 2MnO4- + 2H205SO42- + 2Mn2+ + 4H+

From the equation, it can be seen that 2 moles of KMnO4- react with 5 moles of SO2. So,

moles of SO2 = (moles of KMnO4) x (5 moles of SO2 / 2 moles of KMnO4)

= 0.0000596 x (5/2)

= 0.0001495 moles

Finally, to convert moles of SO2 to grams, we can use the formula:

grams = moles x molar mass

Since the molar mass of SO2 is 64 g/mol,

grams = 0.0001495 x 64

= 0.09536 g

So, there are 0.09536 g of SO2 in the sample of air.