Given that the molar volume of Ne gas is 22.414 L/mol at STP (1.00 atm of pressu

Question

Given that the molar volume of Ne gas is 22.414 L/mol at STP (1.00 atm of pressure and at a temperature of 273.15 K), predict the number of moles of H2 gas when its volume is 11.2 L under the same conditions of temperature and pressure.

2.00 mol

4.00 mol

0.500 mol

0.100 mol

10.0 mol

2.

Which of the following gases has the lowest average molecular velocity at the same temperature?

Ne

Xe

N2

F2

All of these have the same average molecular velocity.

2.00 mol

4.00 mol

0.500 mol

0.100 mol

10.0 mol

2.

Which of the following gases has the lowest average molecular velocity at the same temperature?

Ne

Xe

N2

F2

All of these have the same average molecular velocity.

Explanation / Answer

1. According to Ideal Gas Equation, PV=nRT

Here P= pressure, v=volume, n=no. of moles, R= gas constant, T= temperature

As per question, values of pressure and temp are taken to be same as that of Ne.

So, moles of H2, n=PV/RT= 1*11.2/ 0.082*273.15 = 0.50 moles

2. Average kinetic energy of particle is 3kT/2

According to Newton theory, KE= 1/2mv2

Equating both energies, 3kT/2= 1/2mv2

or, v2 = 3KT/m

v2 is inversely proprtional to mass of the particles.

In all of the given options, Ne has lowest molar mass, so it has more velocity

So Answer is Ne(Neon)

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