Question:

The temperature of a gas is -50° C. To what temperature the gas should be heated so that the rms speed is increased by 3 times?

Updated On: Dec 22, 2024
  • 223 K
  • 669°C
  • 3295°C
  • 3097 K
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The Correct Option is C

Approach Solution - 1

We know that,
\(V_{rms}\propto \sqrt{T}\)

\(\frac{V_{1}}{V_{2}}=\sqrt{\frac{T_{1}}{T_{2}}}\)
\(⇒\) let the initial speed be \(v\).
As the speed increases by 3 times,
So, the final speed \(= 4v\)
\(⇒ \frac{v}{4v}\)

\(= \sqrt{\frac{223}{T}}\)
\(T=3568\text{ K}\)
So, the temperature in \(\degree{C} = 3568 - 273 = 3295\degree{C}\)

The correct answer is (C): \(3295°C\).

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Approach Solution -2

The new velocity (V’rms) has been increased by 3 times the old velocity (Vrms).
Therefore, \(V’_{rms} = V_{rms} + 3 V_{rms} = 4V_{rms}\)
And, we also know Vrms is directly proportional to \(\sqrt{T}\)
Given, the initial temperature (T) = -50°C
Converting the temperature (T) to Kelvin: -50°C + 273 = 223K
Therefore initial temperature (T) in kelvin = 223K
If the speed increases to 4 times, the temperature should also increase by 16 times.
\(\frac{V’_{rms}}{V_{rms}} = \sqrt{\frac{T'}{T}}\)

\(\frac{4V_{rms}}{V_{rms}} = \sqrt \frac{T'}{223}\)
Therefore, Final Temperature (T’) \(= 16 \times 223 = 3568 K\)
Hence, Final Temperature (T’) in \(\degree C = 3568-273 = 3295 \degree C\)

So, the correct option is (C): \(3295 \degree C\)

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Concepts Used:

Kinetic Theory of Gases & Formulae

Kinetic theory of ideal gases is based on the molecular picture of matter. An ideal gas is a gas that follows Boyle's law, Charles' law, Gay Lussac's law, and Avogadro’s law.

  • Gases have no shape or size and can be contained in vessels of any shape and size.
  • Since the molecule of the gases is apart from each other, they have a negligible force of molecular interaction.
  • Therefore, gases expand indefinitely and uniformly to fill the available space.
  • Many scientists like Boyle and Newton tried to explain the behavior of gases, but Maxwell and Boltzmann developed the real theory in the 19th century.
  • This theory is known as the Kinetic theory, which explains the behavior of gases.

The kinetic Theory of Gases is a classical model of the thermodynamic behavior of gases, with which many principal concepts of thermodynamics were established. The kinetic theory of gases describes a gas as a large number of identical submicroscopic particles, all of which are in constant, random, rapid motion.

Also Read: Kinetic Theory of Gases - Assumptions

Kinetic Theory of Gas Formulae:

Boltzmann’s Constant

kB = nR/N

kB is the Boltzmann’s constant

R is the gas constant

n is the number of moles

N is the number of particles in one mole (the Avogadro number)

Total Translational K.E of Gas

K.E = (3/2)nRT

n is the number of moles

R is the universal gas constant

T is the absolute temperature

Maxwell Distribution Law

Vrms > V> Vp

Vrms is the RMS speed.

V is the Average speed.

Vp is the most probable speed.

RMS Speed (Vrms)

Vrms\(\sqrt{8kt/m}\) =\(\sqrt{3RT/M}\)

R is the universal gas constant.

T is the absolute temperature.

M is the molar mass.

Average Speed

\(\overrightarrow{v} = \sqrt{8kt/πm} = \sqrt{8RT/πM}\)

Most Probable Speed (Vp)

\(V_ρ = \sqrt{2kt/m} = \sqrt{2RT/M}\)

The Pressure of Ideal Gas

\(P=\frac{1}{3}V^2rms\)

P is the density of molecules.

Equipartition of Energy

\(K=\frac{1}{2}K_BT\) for each degree of freedom.

K = (f/2) KвT for molecules having f degrees of freedom.

KB is the Boltzmann’s constant.

T is the temperature of the gas.

Internal Energy

U = (f/2) nRT

For n moles of an ideal gas.

Read About: Kinetic Theory of Gases Formulae