A 1.44-mole sample of an ideal gas is allowed to expand at a constant temperature of 258 K. The initial volume is 14.5 L and the final volume is 27.0 L. How much work does the gas perform on its container? Let the ideal-gas constant R = 8.314 J/(mol • K).

1920 J

2340 J

1550 J

1040 J

1920 J

Explanation:

19.6 L

Explanation:

In this process we have an isothermal process, a transformation in which the temperature of the gas remains constant.

In an isothermal process, the work done by the ideal gas on the surrounding is:

where:

n is the number of moles of the gas

R is the gas constant

T is the absolute temperature of the gas

is the initial volume of the gas

is the final volume

In this problem, we have:

n = 1.44 mol

T = 258 K is the gas temperature

is the initial volume of the gas

is the final volume

Solving the equation for W, we find the work done by the gas:

pythagoras' theorem

square root (-5^2+9^2)

square root (25+81)

square root (106)

angle is tan^-1(9/5)

neg x, pos y