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2Consider a container with a frictionless piston that contains a given amount of an ideal gas. If the external pressure is kept constant, the piston will move up or down in response to a change in the internal pressure. The piston will move up if $P_{int} > P_{ext}$ and vice versa. The piston will stop moving when $P_{int} = P_{ext}$ (the system is equilibrated). What is the final volume of the gas? $V = 4.55$ L The following problem will slowly guide you through a work calculation. Some questions may appear trivial, so trust your instincts and don't assume there are hidden tricks. The goal of such a guided exercise is to help you picture the situation so you understand how all relevant variables change or stay the same. This is the first in a sequence of related problems. Remember to use three significant figures for all numerical answers. The margin of error for each non-trivial numerical answer is 2%. To avoid rounding errors use the unrounded intermediate values in your final calculations. Let's assume the initial volume of the gas is 4.20 L, the initial temperature of the gas is 28.0 $^\circ$C and the system is in equilibrium with an external pressure of 1.2 bar (given by the sum of a 1 bar atmospheric pressure and a 0.2 bar pressure due to a brick that rests on top of the piston). What happens with the piston after you finish heating the gas? Assume you do not need to a constant temperature that equals 53.2 $^\circ$C So far this was all at the level of your general chemistry class. Let's now calculate the wor look at the last slide from 8/29/18), and always think from the point of view of the system What is the sign of $w$? What is the value of $w$? Be careful with units. How do you convert bar$\cdot$L to J?

2Consider a container with a frictionless piston that contains a given amount of an ideal gas. If the
external pressure is kept constant, the piston will move up or down in response to a change in the
internal pressure. The piston will move up if $P_{int} > P_{ext}$ and vice versa. The piston will stop moving
when $P_{int} = P_{ext}$ (the system is equilibrated).
What is the final volume of the gas?
$V = 4.55$ L
The following problem will slowly guide you through a work calculation. Some questions may
appear trivial, so trust your instincts and don't assume there are hidden tricks. The goal of such a
guided exercise is to help you picture the situation so you understand how all relevant variables
change or stay the same. This is the first in a sequence of related problems.
Remember to use three significant figures for all numerical answers. The margin of error for each
non-trivial numerical answer is 2%. To avoid rounding errors use the unrounded intermediate values
in your final calculations.
Let's assume the initial volume of the gas is 4.20 L, the initial temperature of the gas is 28.0 $^\circ$C
and the system is in equilibrium with an external pressure of 1.2 bar (given by the sum of a 1 bar
atmospheric pressure and a 0.2 bar pressure due to a brick that rests on top of the piston).
What happens with the piston after you finish heating the gas? Assume you do not need to
a constant temperature that equals 53.2 $^\circ$C
So far this was all at the level of your general chemistry class. Let's now calculate the wor
look at the last slide from 8/29/18), and always think from the point of view of the system
What is the sign of $w$?
What is the value of $w$? Be careful with units. How do you convert bar$\cdot$L to J?

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