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A gas undergoes isothermal expansion. If the volume changes from 175 cm^3 to 343 cm^3, and the total work done by the gas during this process is 9.67 J, what is the initial pressure?

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Answer:

HERE IS YOUR ANSWER

Step-by-step explanation:

To find the initial pressure of the gas during the isothermal expansion, we can use the formula for work done in an isothermal process:

Work = nRT ln(V2/V1)

Where:

Work is the total work done by the gas (9.67 J)

n is the number of moles of the gas

R is the ideal gas constant (8.314 J/(mol·K))

T is the temperature in Kelvin (since it's an isothermal process, the temperature remains constant)

V1 is the initial volume (175 cm^3)

V2 is the final volume (343 cm^3)

First, we need to convert the volumes from cm^3 to m^3:

V1 = 175 cm^3 = 175 × 10^(-6) m^3

V2 = 343 cm^3 = 343 × 10^(-6) m^3

Next, we rearrange the formula to solve for the initial pressure (P1):

P1 = (Work) / (nRT ln(V2/V1))

Since we don't have information about the number of moles, we cannot calculate the exact initial pressure without that information.

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