Consider equal moles of carbon dioxide (CO2) and hydrogen (H2) gases that are ke

Question

Consider equal moles of carbon dioxide (CO2) and hydrogen (H2) gases that are kept in two separate containers with the same size at the same temperature T=300K. You may assume the two gases behave ideally.

Which container has more number of molecules? Explain.

Which container has a higher pressure? Explain.

Now assume it was equal mass of carbon dioxide and hydrogen kept in the same containers. What would be your predictions about the pressure in the two containters? Which one is higher? Explain.

Explanation / Answer

For example take 10 moles of CO2 and 10 moles of H2 in twoseparate containers.

No.of molecules in each container = ?

1 mole contains--------------- 6.023x10^23 molecules

10 moles contain------------- ?

= 10 x 6.023x10^23 molecules

= 6.023x10^24 molecules in both the containers.

Hence both the containers have same number of molecules.

Pressure is proportional to number of molecules of gas present in the container.

Hence both will be having same pressure.

Now if we consider equal masses of the gases in the containers:

For example take 44g of CO2 and 44g of H2 in the containers.

44g of CO2 means---------------- 1 mole (since no.of moles= given weight/molecular weight and molecular weight of CO2 is 44g/mol)

Similarly 44g of H2 means ----------- 44g/2g/mol

                                                         = 22 moles

Hence H2 number of moles is very high compared to CO2.

Hence the pressure in the container having H2 will have more pressure than CO2 container.

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.