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#gas-laws
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#thermodynamics
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#physics
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If a balloon containing 12.2l of gas at 298k is heatwd so the balloon expands to 17.4l, what is the final temperature if the pressure remaina constant?

Jan 12

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Jan 12

To solve this problem, we can use the ideal gas law equation:

PV = nRT

Where:

P = pressure (constant)

V = volume

n = number of moles of gas (constant)

R = ideal gas constant

T = temperature

Since the pressure remains constant, we can rewrite the equation as:

V1/T1 = V2/T2

Where:

V1 = initial volume

T1 = initial temperature

V2 = final volume

T2 = final temperature

Given:

V1 = 12.2 L

T1 = 298 K

V2 = 17.4 L

We can rearrange the equation to solve for T2:

T2 = (V2 * T1) / V1

Substituting the given values:

T2 = (17.4 L * 298 K) / 12.2 L

T2 ≈ 424.59 K

Therefore, the final temperature is approximately 424.59 K.

PV = nRT

Where:

P = pressure (constant)

V = volume

n = number of moles of gas (constant)

R = ideal gas constant

T = temperature

Since the pressure remains constant, we can rewrite the equation as:

V1/T1 = V2/T2

Where:

V1 = initial volume

T1 = initial temperature

V2 = final volume

T2 = final temperature

Given:

V1 = 12.2 L

T1 = 298 K

V2 = 17.4 L

We can rearrange the equation to solve for T2:

T2 = (V2 * T1) / V1

Substituting the given values:

T2 = (17.4 L * 298 K) / 12.2 L

T2 ≈ 424.59 K

Therefore, the final temperature is approximately 424.59 K.