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Blizzard [7]
3 years ago
9

A cylinder with a movable piston contains a sample of gas having a volume of 6.0 liters at 293 K and 1.0 atmosphere. What is the

volume of the sample after the gas is heated to 303 K, while the pressure is held at 1.0 atmosphere?
(1) 9.0 L (3) 5.8 L
(2) 6.2 L (4) 4.0 L
Chemistry
1 answer:
Lorico [155]3 years ago
8 0

The volume of sample when the gas is heated to 303 K is   \boxed{{\text{(2)6}}{\text{.2 L}}}

Further explanation:

Charles’s law:

Charles’s work showed that at constant pressure, the volume-temperature relationship for a fixed amount of gas is linear. In other words, Charles’s law can be stated that at constant pressure, the volume occupied by a fixed amount of a gas is directly proportional to its absolute temperature (Kelvin). This relationship is known as Charles’s law.

The mathematical representation of Charles’s law is,

{\mathbf{V}}\propto{\mathbf{T}}                                                                           [P and n are constant]

Where,

⦁ V is volume occupied by the fixed quantity of gas.

⦁ T is the temperature of a gas.

⦁ P is the pressure of a gas.

⦁ n denotes the number of moles of gas.

The relationship can also be expressed as,

\frac{{\text{V}}}{{\text{T}}} = {\text{constant}}                                                  [P and n are constant]

Or it can also be expressed as follows:

\frac{{{{\text{V}}_{\text{1}}}}}{{{{\text{T}}_{\text{1}}}}} = \frac{{{{\text{V}}_{\text{2}}}}}{{{{\text{T}}_{\text{2}}}}}                                                          …… (1)

Here,

{{\text{V}}_1}  is the initial volume of gas.

{{\text{V}}_2}  is the final volume of gas.

{{\text{T}}_1}  is the initial temperature of the gas.

{{\text{T}}_2}  is the final temperature of the gas.

Rearrange equation (1) to calculate {{\text{V}}_2} .

{{\text{V}}_{\text{2}}} = \frac{{{{\text{V}}_{\text{1}}}{{\text{T}}_{\text{2}}}}}{{{{\text{T}}_{\text{1}}}}}                                                                  …… (2)

The value of {{\text{V}}_1}  is 6 L.

The value of {{\text{T}}_1}  is 293 K.

The value of {{\text{T}}_2}  is 303 K.

Substitute these values in equation (2).

\begin{aligned}{{\text{V}}_{\text{2}}}&=\frac{{\left({{\text{6 L}}}\right)\left( {{\text{303 K}}}\right)}}{{\left( {{\text{293 K}}}\right)}}\\&={\text{6}}{\text{.20477 L}}\\&\approx{\mathbf{6}}{\mathbf{.2 L}}\\\end{aligned}

So option (2) is the correct answer.

Learn more:

1. Law of conservation of matter states: <u>brainly.com/question/2190120 </u>

2. Calculation of volume of gas: <u>brainly.com/question/3636135 </u>

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Ideal gas equation

Keywords: Charles’s law, volume, temperature, pressure, volume temperature relationship, absolute temperature, constant pressure, relationship, V directly proportional to T, ideal gas, ideal gas equation number of moles, moles, P, n, V, T, volume of gas, 6.2 L, 303 K, 293 K, 6 L.

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A sample of an ideal gas has a volume of 2.30 L at 281 K and 1.02 atm. 1.76 atm is the pressure when the volume is 1.41 L and the temperature is 298 K.

<h3>What is Combined Gas Law ?</h3>

This law combined the three gas laws that is (i) Charle's Law (ii) Gay-Lussac's Law and (iii) Boyle's law.

It is expressed as

\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}

where,

P₁ = first pressure

P₂ = second pressure

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V₂ = second volume

T₁ = first temperature

T₂ = second temperature

Now put the values in above expression we get

\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}

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