Q1:

If a person breathes at the rate of 15 respirations per minute, and each respiration involves 0.500 dm^3 of air, calculate the total mass of air breathed in one hour at 280K and 1 arm pressure. Average molar mass of air is 28.8g/mol.

 

 

 

Q2:

A 600cm^3 gas sample contains only methane, CH4, and ethane,H2C_CH2 . Half of the sample was burned in oxygen and found to produce 486.8cm^3 of dry carbon dioxide at 1atm, 300K. The water produced during combustion had been removed. The remainder of the sample was found to require 187.8cm^3 of hydrogen at 1 arm and 300K to convert the ethene to ethane C2H6.

 

A) determine the molar fraction of methane in the orginal sample?

B) what is the mass and density of the original gas sample?

This is simple. A little equation formulas, mathematics, and chemistry. Here. This will help. I won't soil the unfairness of solving it for you, but here.

Edited February 21, 201510 yr by Jordyn Rahizel

If a person breathes at the rate of 15 respirations per minute, and each respiration involves 0.500 dm^3 of air

 

Calculate the number of liters per minute 1 dm^3= 1 liter

 

calculate the total mass of air breathed in one hour at 280K and 1 arm pressure. Average molar mass of air is 28.8g/mol.

 

Avogadro's law I am assuming average molar mass of air is at stp or has been provided to you. Is arm pressure supposed to be atm never heard of arm pressure units it also must be converted to kPa for the formula

Edited February 21, 201510 yr by fiveworlds