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What happens to the internal energy of a gas when it expands?
When a gas expands, its internal energy typically increases. This is because the gas is doing work on its surroundings as it expands, which results in an increase in its internal energy.
When a gas expands to a region of low pressure what happen to its temperature?
The temperature drops. When a real (non ideal) gas expands ( in such a way that it does not take in heat from the environment- so called adiabatic) for example when hot air rises into a low pressure region the gas will cools. Real gases when they expand freely cool, this is the basis of the refrigerator (Joule Thomson effect). The explanation is that the separation of gas molecules involves "work" done against intermolecular forces which leads to a reductio in the kinetic of the molecules, hence the observed temperature.
How do vacuum flasks work?
think of it as a battery. it stores a large vacuum reserve while the engine is running. then its used whenever you use the device attached to it requiring the vacuum source. without it things like your heater and ac controls would not work properly because they require a large amount of vacuum to operate that your engine alone cannot supply fast enough.
How do liquid thermometers work to measure temperature accurately?
Liquid thermometers work by using a liquid that expands or contracts with changes in temperature. The liquid is contained in a sealed tube with a scale marked on it. As the temperature changes, the liquid expands or contracts, causing it to move up or down the tube, indicating the temperature on the scale. This allows for accurate measurement of temperature changes.
When an ideal gas does positive work on its surroundings which of the gas's quantities increases?
When an ideal gas does positive work on its surroundings, its volume increases. This is because the gas is expanding against an external pressure, leading to an increase in volume while maintaining pressure and temperature constant.
What is the formula for calculating the work done by an ideal gas in a thermodynamic process?
The formula for calculating the work done by an ideal gas in a thermodynamic process is: Work -PV where: Work is the work done by the gas, P is the pressure of the gas, and V is the change in volume of the gas.
Work done in a free expansion process is?
In a free expansion process, no work is done because there is no external pressure or constraint on the system. The gas expands into a vacuum freely without any opposing force to overcome, resulting in no work being performed.
A fulcrum is on the left side of a board as it is moved to the right will the force be the same?
Work: The work done by the force is the same as the work done on the load in an ideal simple machine.
What work is done when ideal gas at 15 ATM and 10 L expands against 2 ATM at constant temp?
The work done in this case is the area under the pressure-volume (P-V) curve. Since the gas is expanding against an external pressure of 2 ATM, the gas must do work to overcome this pressure. The work done is given by the formula: Work = P_ext(V_final - V_initial), where P_ext is the external pressure, and V_final and V_initial are the final and initial volumes of the gas respectively.
When the gas in a balloon is heated the balloon expands what are the correct signs of heat and work for this change?
When the gas in a balloon is heated and the balloon expands, the correct signs for heat and work are: the heat absorbed by the gas is positive (+Q) and the work done by the gas is also positive (+W). This is because the gas is gaining energy (heat) from its surroundings, and it is doing work on the balloon by pushing against the walls as it expands.
What is the relationship between the work done and the expansion of gas in a thermodynamic system?
The work done in a thermodynamic system is directly related to the expansion of gas. When gas expands in a system, it can perform work by pushing against a piston or moving a turbine. This work done is a result of the gas expanding and exerting a force on its surroundings.
What is the relationship between the work done by an expanding gas and the change in its internal energy?
The work done by an expanding gas is directly related to the change in its internal energy. When a gas expands, it does work on its surroundings, which can lead to a change in its internal energy. This change in internal energy is a result of the work done by the gas during the expansion process.
How will the work done on the input piston compare to the work done by the output piston in a hydraulic device?
In a hydraulic device, the work done by the input piston will be equal to the work done by the output piston if the system is ideal and there are no energy losses due to friction or other factors. This is based on the principle of conservation of energy in a closed system.
Why a gas cools when it expands at high pressure?
When a gas expands at high pressure, it does work on its surroundings to overcome the external pressure. This work done by the gas results in a decrease in its internal energy, leading to a decrease in temperature as per the first law of thermodynamics. So, the gas cools down as it expands at high pressure.
Why is work done with a machine is the same as work done without a machine?
In an ideal scenario, the work done with a machine is the same as work done without a machine because the total work output must be equal to the total work input. While machines can make work easier by multiplying force or changing the direction of force, they cannot create energy. Therefore, the work done by the machine should ideally be equal to the work done without a machine.
How does work play a role in an adiabatic expansion process?
In an adiabatic expansion process, work is done by the gas as it expands without gaining or losing heat from its surroundings. This work is done against the external pressure, causing the gas to decrease in temperature and increase in volume. The work done in this process is equal to the change in internal energy of the gas.
A monatomic ideal gas at a pressure of 2x105pa expands at a constant temperature from an initial volume of 3.00m3 until its volume doubles. How much work is done on the environment?
The work done by the gas on the environment as it expands is given by the equation: (W = -P \Delta V), where (P) is the pressure and (\Delta V) is the change in volume. Since the gas expands at constant temperature, its final pressure is equal to its initial pressure. Therefore, the work done on the environment is (W = -(2x10^5 \text{ Pa}) \times (3.00 \text{ m}^3) = -6.00 \times 10^5 \text{ J}).
