On burning sulfur in oxygen, sulfur dioxide is produced
S + O2 → SO2
For producing 2240 L of SO2 at STP
(i) How many grams of sulfur and (ii) how many moles of O2 will be required? (0 = 16, S = 32) [3]
OR
On burning 480 g of a solid compound in 352 g of oxygen, 320 g of another solid compound and a gaseous compound are produced. If the vapour density of the gaseous compound is 32, how many moles of the gaseous compound are formed? [3]
Balanced Chemical Equation:
S + O2 → SO2
32 g 1 mol 22.4 L
(i) Amount of S required to produce 22.4 L of SO2 = 32 g
⇒ Amount of S required to produce 2240 L of SO2 = 32\over 22.4 × 2240 = 3200 g
(ii) The number of moles of oxygen required to produce 22.4 L of SO2 = 1
⇒ The number of moles of oxygen required to produce 2240 L of SO2 = 1\over 22.4 × 2240 = 100 mol
OR
Given Data
- Mass of solid compound burned = 480 g
- Mass of oxygen used = 352 g
- Mass of solid compound produced = 320 g
- Vapor density of gaseous compound = 32
Molar Mass = 2 × Vapor Density
= 2 × 32
= 64
Mass of gaseous compound=480 g + 352 g − 320 g
= 512 g
∴ Moles of gaseous compound = 512/64 = 8 mol
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