Question

11. Consider a sample of hydrogen (H) and another sample of oxygen (O2). Both gases are at the same temperature and pressure. The volume of each gas is equal. (5) a) which gas has the greatest number of moles, or are they the same? b) which gas has the greatest number of molecules, or are they the same? c) which gas has the greatest mass, or are they the same? d) Which gas has the highest kinetic energy, or are they the same? e) Which gas has the greater velocity? 12. Consider the following molecules: (5) NH3 CH4 HCI Type of IMFs: Rank the molecules by their vapor pressure: higest VP lowest VP 13. Assume you have two 1L tanks (both at 325K). One tank contains 1.00g of hydrogen and then other contains 1.00g helium. Which tank has the greater pressure?

Answer 1

11)

A) as both gases has same Pressure , Temperature and Volume , then they have same number of moles

B) both have same number of molecules

C) O2 has greatest mass(because it has higher molar mass)

D) they have same kinetic energy

E) H2 has greater velocity (as it has lower molar mass)

12) NH3 = Hydrogen bonding

CH4 = London dispersion force

HCl = dipole-dipole

Vapour pressure order (strong the IMF ,lower the vapour pressure)

NH3 > HCl > CH4

13) as both are at same temperature and volume. So hydrogen has higher moles so it has greater pressure.

Tank containing hydrogen has greater pressure