Home
Class 11
CHEMISTRY
Determine the volume of air containing 2...

Determine the volume of air containing 20% oxygen by volume, that would have to be inhaled at `20^(@)`C and 1.0 atm to consume 1.00 kg of fat `C_(57) H_(110) O_(6)` assuming that only 70% (by volume) of the oxygen present in the air is used up in combustion.

A

15715 L

B

23123 L

C

18832 L

D

16312 L

Text Solution

Verified by Experts

The correct Answer is:
A
The combustion reactions is `C_(57) H_(110) O_(6) + (163)/(2) O_(2) to 57 CO_(2) + 55 H_(2) O implies n = (1000)/(890) = (100)/(89)`
Moles of `O_(2)` required = `(100)/(89) xx (163)/(2)` (theoretical)
Actual moles of `O_(2)` required = `(100)/(89) xx (163)/(2) xx (100)/(70) = 130.82`
`V_(O_2)` required = `130.82 xx 0.082 xx 293 = 3143` L , Volume of the air required `= 3143 xx (100)/(20) = 15715`
Promotional Banner

Topper's Solved these Questions

  • STATES OF MATTER

    BRILLIANT PUBLICATION|Exercise LEVEL III (Multiple Correct Answer type )|14 Videos

  • STATES OF MATTER

    BRILLIANT PUBLICATION|Exercise LEVEL III (Numerical Type)|7 Videos

  • STATES OF MATTER

    BRILLIANT PUBLICATION|Exercise LEVEL II |55 Videos

  • SOME BASIC CONCEPTS OF CHEMISTRY

    BRILLIANT PUBLICATION|Exercise LEVEL-I|55 Videos

  • STRUCTURE OF ATOMS

    BRILLIANT PUBLICATION|Exercise LEVEL - III (Linked Comprehension Type)|8 Videos

Similar Questions

Explore conceptually related problems

Air contains nearly 20% oxygen by volume. The volume of air needed for complete combustion of 100 ml of acetylene will be

If the components of air are N_(2), 78%, O_(2), 21%, Ar, 0-9% and CO_(2), 0-1% by volume, what would be the molecular weight of air?

An air bubble of volume 0.21 cm^3 at the bottom of a water tank, at 5^(@)C and 3 atm pressure, rises to the surface where the temperature is 25^(@)C and pressure is 1 atm. What will be the volume of the bubble when it reaches the surface?