A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 72 J of heat while 35 J of work is done on it. Step 2: The system absorbs 35 J of heat while performing 72 J of work. Calculate ΔE for the overall process.

A piston performs work of $210 . \mathrm{L} \cdot \text {atm}$ on the surroundings, while the cylinder in which it is placed expands from 10. L to 25 L. At the same time, 45 J of heat is transferred from the surroundings to the system. Against what pressure was the piston working?

A sample of an ideal gas at 15.0 atm and 10.0 L is allowed to expand against a constant external pressure of 2.00 atm at a constant temperature. Calculate the work in units of kJ for the gas expansion.

Explain why the following argument is incorrect.

$$\lim _ { x \rightarrow 0 } \left( \frac { 1 } { x } - \frac { 2 } { x ^ { 2 } + 2 x } \right) = \lim _ { x \rightarrow 0 } \frac { 1 } { x } \left( 1 - \frac { 2 } { x + 2 } \right)= \infty \cdot 0 = 0$$

When a gas expands, what is the sign of "w" ? Why? When a gas contracts, what is the sign of "w" ? Why? How does one calculate the work associated with the expansion or compression of a gas? What is a L.atm unit?

An ideal gas at a given state expands to a fixed final volume first at constant pressure and then at constant temperature. For which case is the work done greater?

A system releases 125 kJ of heat while 104 kJ of work is done on it. Calculate $\Delta E$.

A triangular field has sides of lengths 22, 36, and 44 yd. Find the largest angle.

Find the value of k so that the lines through the given points are parallel. Line 1: (-4, -2) and (0, 0) Line 2: (2, 7) and (k, 5)

What is the change in internal energy (in J) of a system that absorbs 0.615 kJ of heat from its surroundings and has 0.247 kcal of work done on it.

Which has the greater kinetic energy, an object with a mass of 2.0 kg and a velocity of 1.0 m/s or an object with a mass of 1.0 kg and a velocity of 2.0 m/s?

A system releases $125 \mathrm{~kJ}$ of heat while $104 \mathrm{~kJ}$ of work is done on it. Calculate $\Delta E$.

How is average bond strength related to relative potential energies of the reactants and the products?

Consider a process in which an ideal gas changes from state 1 to state 2 in such a way that its temperature changes from 300 K to 200 K. Does the change in the internal energy,

$$\Delta E$$

depend on the particular pathway taken to carry out this change of state?