Thermodynamics II

Explanation
In a thermodynamic process where the pressure is held constant, the heat transferred to the system can be calculated using the equation ΔU + W. ΔU represents the change in internal energy of the system, which is the energy stored within the system. W represents the work done on or by the system. By adding these two values together, we can determine the total heat transferred to the system.

Explanation
In a thermodynamic process where the heat content of the system or a certain quantity of matter remains constant, it means that there is no change in the internal energy of the system. This implies that the heat transferred to or from the system is equal to zero. Therefore, the correct answer is "= zero".

Explanation
A reversible process is one that can be reversed by making insignificant changes to the system, such as by reversing the direction of heat flow or by restoring the system to its initial state. A cyclic process is one that starts and ends at the same state, meaning that the system goes through a series of changes and returns to its original state. Therefore, the statement "The process is cyclic" is true about a reversible process.

Explanation
This statement is false. According to Boyle's Law, at constant temperature, the volume of a gas is inversely proportional to its pressure. This means that as pressure increases, the volume decreases, and vice versa.

Explanation
Amonton's law, also known as the pressure-temperature law, states that when the volume of a fixed amount of gas is kept constant, the pressure of the gas is directly proportional to its temperature. This means that as the temperature of the gas increases, the pressure also increases, and vice versa. This relationship can be mathematically expressed as P ∝ T, where P is the pressure and T is the temperature. Therefore, the statement "if the volume of a fixed gas is held constant, its pressure is directly proportional to its temperature" is true.

Explanation
Boyle-Mariotte's Law states that the pressure of a fixed amount of gas at constant temperature is inversely proportional to its volume. This means that as the volume of the gas decreases, the pressure increases, and vice versa, as long as the temperature remains constant. This law is derived from the observation that when the volume of a gas decreases, the gas molecules collide more frequently with the walls of the container, resulting in an increase in pressure.

Explanation
When oxygen gas (O2) is converted into ozone (O3), the molar ratio is 1:1. This means that for every mole of oxygen gas, one mole of ozone is produced. Since the initial sample contains 0.25 moles of oxygen gas, it will produce 0.25 moles of ozone. The volume of the ozone will remain the same as the volume of the initial sample, which is 12 liters. Therefore, the correct answer is 12.0 liters.

Explanation
At standard pressure, the volume of a gas is directly proportional to its initial volume. Since the initial volume is 2.00 liters and the volume at standard pressure is 1.95 liters, it can be concluded that the gas has decreased in volume.

Explanation
According to the question, the gas is collected at 25.0°C. Standard temperature is defined as 0°C or 273.15K. As temperature decreases, the volume of a gas decreases, assuming pressure remains constant. Therefore, the volume of the gas will be less at standard temperature compared to 25.0°C. Among the given options, 2.61 liters is the closest value to represent the decrease in volume due to the decrease in temperature.

Explanation
Internal energy refers to the total energy of the motions of atoms and molecules within an object or system. It includes the kinetic energy of individual particles as well as the potential energy associated with their interactions. Internal energy is a measure of the overall thermal energy of a system and is influenced by factors such as temperature, pressure, and the number of particles present. It is a fundamental concept in thermodynamics and plays a crucial role in understanding the behavior and changes in energy within a system.