A sample of carbon dioxide gas collected at a pressure of 880 mm Hg and a temperature of 303 K has a mass of 26.9 g. The volume of the sample is L.

13.1dm³

Explanation:

Given parameters:

Pressure of gas  = 880mmHg

        760mmHg  = 1 atm

        880mmHg will give 1.16atm

Temperature  = 303k

Mass of gas = 26.9g

      Molar mass of CO₂   = 12 + 2(32)  = 44g/mol

       Number of moles  = mass/molar mass  = 26.9/44  = 0.61mole

Unknown:

Volume of the sample  = ?

Solution:

To solve this problem, we use the ideal gas equation:

           PV  = nRT

P is the pressure

V is the volume

n is the number of moles

R is the gas constant  = 0.082atmdm³mol⁻¹k⁻¹

T is the temperature

        V  =   =    = 13.1dm³

air

in a tire you fill a tire with air

then a couple days later you check the air pressure in the tire

hope this mark me brainliest