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Neetoo

Answer:

T₂ = 411.94 k

Explanation:

Given data:

Initial volume = 3.4 L

Initial temperature = 25 °C ( 25 + 273 = 298K )

Final volume = 4.7 L

Final temperature = ?

Solution:

According to Charles's Law,

The volume and temperature are directly related to each other at constant pressure and mount of gas.

V₁/T₁ = V₂/T₂

T₂ = V₂T₁/V₁

T₂ = 4.7 L×298 K / 3.4 L

T₂ = 1400.6 L.K / 3.4 L

T₂ = 411.94 k

nuhulawal20

The new temperature of the gas as the volume is increased to the given amount is 412.15K

Given the data in the question;

  • Initial volume; [tex]v_1 = 3.4L[/tex]
  • Final volume; [tex]v_2 = 4.7L[/tex]
  • Initial temperature; [tex]T_1 = 25^0C = 298.15K[/tex]
  • Final temperature; [tex]T_2 = ?[/tex]

Charles's law

Charles's law states that the volume occupied by a definite quantity of gas is directly proportional to its absolute temperature.

It is expressed as;\

[tex]\frac{V_1}{T_1} = \frac{V_2}{T_2}[/tex]

To determine the new temperature as the volume is decreased, we substitute our given values into the expression above.

[tex]\frac{V_1}{T_1} = \frac{V_2}{T_2} \\\\V_1T_2 = V_2T_1\\\\T_2 = \frac{V_2 * T_1}{V_1}\\ \\T_2 = \frac{4.7L * 298.15K}{3.4L}\\\\T_2 = \frac{1401.305LK}{3.4L} \\\\T_2 = 412.15K[/tex]

The new temperature of the gas as the volume is increased to the given amount is 412.15K

Learn more about Charles's law: brainly.com/question/12835309