280 g of a mixture containing Ch4 and c2h6 in 5:2 molar ratio is burnt in presence of excess of oxygen. calculate total moles of co2 produced
Answers
From the given ratio we can get the masses of the two compounds.
From the ratio the mass of CH₄ will be :
5/7 × 280 = 200 g
The mass of C₂H₆ will be :
2/7 × 280 = 80 g
Equation for combustion of both is :
CH₄ + 2O₂ —> CO₂ + 2 H₂O
The moles of CH₄ are :
200 / 16 = 12.5 moles.
The mole ratio of CH₄ to CO₂ is 1 : 1 and hence moles of CO₂ are 12.5 moles.
C₂H₆ + 3.5O₂ —> 2CO₂ (g) + 3H₂O
Moles of C₂H₆ are :
80/30 = 2.667 moles.
The mole ratio is 1 : 2
Moles of CO₂ will be :
2 × 2.667 = 5.334 moles.
Total moles :
5.334 + 12.5 = 17.834 moles
Answer:
Explanation:
From the given ratio we can get the masses of the two compounds.
From the ratio the mass of CH₄ will be :
5/7 × 280 = 200 g
The mass of C₂H₆ will be :
2/7 × 280 = 80 g
Equation for combustion of both is :
CH₄ + 2O₂ —> CO₂ + 2 H₂O
The moles of CH₄ are :
200 / 16 = 12.5 moles.
The mole ratio of CH₄ to CO₂ is 1 : 1 and hence moles of CO₂ are 12.5 moles.
C₂H₆ + 3.5O₂ —> 2CO₂ (g) + 3H₂O
Moles of C₂H₆ are :
80/30 = 2.667 moles.
The mole ratio is 1 : 2
Moles of CO₂ will be :
2 × 2.667 = 5.334 moles.
Total moles :
5.334 + 12.5 = 17.834 moles
Hope it helps!