Question

how many grams of H2S will react with 6.32g of KMnO4 to produce K2SO4 and MnO2?

Answer 1

0.51 grams is ur answer dear

Answer 2

Answer:

0.51 g of H₂S.

Explanation:

It is given that, 6.32 grams of KMnO₄ is reacting with H₂S in a chemical reaction, to form K₂SO₄ and MnO₂....

And we have been asked to find the weight of H₂S that will be required to react with the given amount of KMnO₄....

Now we know that reactants in a chemical reaction react in equal number of equivalents.....

Here, n factor of:-

• KMnO₄ = 3....... As oxidation number of Mn changes from +7 to +4.
• H₂S = 8........ As oxidation number of S changes from -2 to +6.

∴No. of Eq. of KMnO₄ = No. of Eq. of H₂S

∴Eq. wt. of KMnO₄ in this reaction = $\frac{molar mass}{n factor}$ = $\frac{158}{3}$ = 52.67 g

∴ No. of Eq. of KMnO₄ =  $\frac{6.32}{52.67}$ = 0.12 eq

∴ No. of Eq. of H₂S = 0.12 eq

We know, that given wt = No. of eq. * eq. wt

∴ Wt of H₂S = 0.12 * $\frac{34}{8}$

                  = 0.51 g

Hence, the answer is 0.51 g i.e., 0.51 g of H₂S is required to react with 6.32 g KMnO₄ to produce K₂SO₄ and MnO₂.