Heat is supplied to a diatomic gas. .

Heat is supplied to a diatomic gas. Solution: For a diatomic gas, C V = 25R;C P = 27R ΔQ = nC P ΔT = n(27R)ΔT ΔU = nC V ΔT = n(25R)ΔT According to first law of thermodynamics, ΔW = ΔQ −ΔU = nRΔT ∴ ΔQ: ΔU: ΔW = 27: 25: 1 or 7: 5: 2. To solve the problem of finding the ratio of ΔQ: ΔU:ΔW for a diatomic gas at constant pressure, we can follow these steps: Step 1: Understand the relationship between heat, internal energy, and work Oct 21, 2019 · The molar specific heat capacity of a gas at constant volume (C v) is the amount of heat required to raise the temperature of 1 mol of the gas by 1 °C at the constant volume. Its value for monatomic ideal gas is 3R/2 and the value for diatomic ideal gas is 5R/2. The heat required to produce the same change in temperature, at a constant pressure is:. Understanding the Problem: Apr 10, 2019 · When heat Q is supplied to a diatomic gas of rigid molecules, at constant volume its temperature increases by ΔT. May 18, 2025 · To solve the problem, we need to determine the portion of heat supplied to a diatomic gas at constant pressure that increases its internal energy. 7:2:5. 1. Jul 8, 2024 · The ratio of ΔQ:ΔU:ΔW when heat is supplied to a diatomic gas at constant pressure is D. To understand this, we start with the first law of thermodynamics: ΔQ = ΔU + ΔW, where ΔQ is the heat added to the system, ΔU is the change in internal energy, and ΔW is the work done by the gas. Note: We know that the first law of thermodynamics states that when a certain amount of heat is supplied to a thermodynamic system then a part of this heat energy is used to change the internal energy of the gas while rest of the energy is used in doing work. olsmmhz cxxw kxxo ral ukiopz dlkd wraujj fgrpcm ktocz qnregm