If you have 1.33g of oxygen (Mr = 32) in a container of volume 1000cm^3 at atmospheric pressure (101.3*10^3 Pa), what is the temperature of the gas in Celsius? R=8.314
T=20.2 degrees Celsius. Start by finding number of moles using n=mass/Mr so n=1.33/32=0.0416. Find the volume in m^3 using 1cm^3=110^-6 m^3 giving V=110^-3 m^3 then rearrange PV=nRT to get T=PV/nR so T=(101.310^3 * 110^-3) / (0.0416 * 8.314)=293.2K then convert to Celsius using K-273 so 293.2-273=20.2 degrees Celsius.
ET
Related Physics A Level answers
All answers ▸An ideal gas within a closed system undergoes an isothermal expansion from an initial volume of 1m^3 to 2m^3. Given that the initial pressure of the gas is 10^5 Pa, find the final pressure of the gas following the expansion.
Describe the principles of fission and fusion. With reference to the nuclear binding energy curve, explain how energy is released.
Describe and explain the photoelectric effect in terms of photons interacting with the surface of a metal.
Why are values for gravitational potential always negative?