Mole ConceptHard
Question
What is the total mass of the products formed, when 51 g of H2S is oxidized by oxygen to produce water and sulphur dioxide?
Options
A.72 g
B.27 g
C.123 g
D.96 g
Solution
$H_{2}S + \frac{3}{2}O_{2} \rightarrow H_{2}O + SO_{2}$
$34\text{ g} \frac{3}{2} \times 32\text{ g} $$$\therefore\text{51 g} \frac{48}{34} \times 51 = 72\text{ g}$$
∴ Total mass of product formed = 51 + 72 = 123 g
Create a free account to view solution
View Solution FreeMore Mole Concept Questions
Calculate the mass percent (w/w) of sulphuric acid in a solution prepared by dissolving 4 g of sulphur trioxide in a 100...The molec1ularity of a complex reaction given below is :- 2N2O5 (g) → 4NO2(g) + O2(g)...An amount of 0.3 mole of SrCl2 is mixed with 0.2 mole of K3PO4. The maximum moles of KCl which may form is...A 1.50 g sample of potassium bicarbonate having 80% purity is strongly heated. Assuming the impurity to be thermally sta...V1 ml of unknown gas (A) + V2 ml of O2 → (V1 + V2) ml of CO2. Gas ‘A’ may be...