22. The First Law of Thermodynamics

Which law of thermodynamics is primarily concerned with the conservation of energy in a system?

According to the First Law of Thermodynamics, if a system is isolated, the total energy of the system $E$ ________.

According to the $FirstLawofThermodynamics$, in which direction does $Q$ naturally flow between two objects at different $T$?

According to the First Law of Thermodynamics, what does it mean that energy cannot be created or destroyed?

Which of the following is a statement of the first law of thermodynamics?

According to the law of conservation of energy, what will most likely happen in a closed system?

A scuba diver releases a 3.60-cm-diameter (spherical) bubble of air from a depth of 14.0 m. Assume the temperature is constant at 298 K, and that the air behaves as an ideal gas. Sketch a PV diagram for the process. Take the density of water to be 1000 kg/m³.

Which of the following devices violates the first law of thermodynamics ($\mathrm{\Delta U}=Q-W$)?

Which fundamental physical law forms the basis of the first law of thermodynamics?

Which of the following statements best describes the first law of thermodynamics?

A gas in a cylinder held at a constant pressure 1.80×10⁵ Pa expands from a volume of 1.2 m³ to 1.6 m³. The internal energy of the gas decreases from 4.40×10⁵ J to 3×10⁵ J. How much heat was transferred to the gas?

The internal energy of a system decreases by 500 J, and 230 J of work is done on the system. What is the heat transfer into or out of this system?

When water is boiled at a pressure of $2.00$ atm, the heat of vaporization is $2.20\times10^6$ J/kg and the boiling point is $120$°C. At this pressure, $1.00$ kg of water has a volume of $1.00\times10^{-3}$ m³, and $1.00$ kg of steam has a volume of $0.824$ m³. Compute the increase in internal energy of the water.

A gas in a cylinder is held at a constant pressure of $1.80\times {10}^5$ Pa and is cooled and compressed from $1.70$ m³ to $1.20$ m³. The internal energy of the gas decreases by $1.40\times {10}^5$ J. Does it matter whether the gas is ideal? Why or why not?

Five moles of an ideal monatomic gas with an initial temperature of $127$°C expand and, in the process, absorb $1500$ J of heat and do $2100$ J of work. What is the final temperature of the gas?