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∙ 14y agodude im not gonna do your homework for you.
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∙ 14y agoUsing the first law of thermodynamics, we have: ΔU = Q - W. Substituting the values, we get ΔU = 2893 J - 811 J = 2082 J. For a monatomic ideal gas, ΔU = (3/2)nRΔT, where n is the number of moles, R is the ideal gas constant, and ΔT is the change in temperature. Solving for ΔT, we find ΔT = ΔU / ((3/2)nR). Substituting the values gives ΔT = 2082 J / ((3/2) * 3 * 8.314 J/mol⋅K) = 34.5 K. Therefore, the final temperature is 335 K + 34.5 K = 369.5 K.
The temperature change when a gas is compressed without any heat exchange can be calculated using the ideal gas law. First, calculate the initial pressure of the gas using P1V1 = P2V2. Next, use the combined gas law to calculate the final temperature using the initial pressure, volume, final volume, and initial temperature. Subsequently, calculate the temperature decrease by subtracting the final temperature from the initial temperature.
The ideal gas law, also known as the equation of state for an ideal gas, relates the pressure, volume, and temperature of an ideal gas if the volume is kept constant. This law states that when the temperature of an ideal gas increases at constant volume, the pressure of the gas will also increase.
The ideal gas law is: PV = nRT, where P = pressure, V = volume, n= number of moles, R = ideal gas constant, T = Temperature in K.
To calculate the temperature rise of compressed air, you can use the formula: T2 = T1 + (P2 - P1) / (Cp * m), where T2 is the final temperature, T1 is the initial temperature, P2 and P1 are the final and initial pressures, Cp is the specific heat capacity of air at constant pressure, and m is the mass of the air. This formula assumes adiabatic compression and neglects heat transfer and work done in compression.
To find the final temperature, we can use the ideal gas law. First, calculate the initial specific volume of the mixture using the quality of the saturated steam. Then, use the equation of state to find the final specific volume at the new pressure. Finally, determine the final temperature using the final specific volume and the new pressure.
Argon is considered a nearly ideal gas under many conditions due to its low reactivity and monatomic structure, which leads to minimal intermolecular interactions. However, at extreme conditions of high pressure or low temperature, deviations from ideal gas behavior may occur.
the ideal temperature is 68degrees-86degrees F
A monatomic compound is a chemical compound composed of individual atoms of only one element. These compounds do not contain multiple elements bonded together, only a single element. Examples include noble gases like helium, neon, and argon.
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To determine the final temperature of the air in the rigid container, you would need to know the volume of the container and the gas constant for air. Using the ideal gas law (PV = nRT), you can calculate the initial and final temperatures. Without this information, it is not possible to determine the final temperature of the air in the container accurately.
What is the ideal set temperature for washing machines to conserve energy?
At standard temperature and pressure (STP), the most ideal gas would be one that is closest to an ideal gas behavior, such as helium or neon. These gases have low molecular weights and weak intermolecular forces, making them behave more like ideal gases.
Extremely limited chemical reactivity; low condensation temperatures compared with other gases of the same molecular weight; and very nearly ideal gas behavior at normal temperature and pressure.
The internal energy of an ideal gas increases as it is heated because the added heat increases the average kinetic energy of the gas molecules, leading to an increase in their internal energy. The internal energy is directly proportional to temperature for an ideal gas, so as the temperature increases from 0C to 4C, the internal energy also increases.
The temperature change when a gas is compressed without any heat exchange can be calculated using the ideal gas law. First, calculate the initial pressure of the gas using P1V1 = P2V2. Next, use the combined gas law to calculate the final temperature using the initial pressure, volume, final volume, and initial temperature. Subsequently, calculate the temperature decrease by subtracting the final temperature from the initial temperature.
For ideal gases, the partial pressure term in equilibrium constant expressions is independent of temperature. This means that the concentration term for ideal gases is independent of temperature, assuming the ideal gas law holds true.
Each enzyme has its ideal temperature