In an isothermal reversible expansion at 23°C, an ideal gas does 55 J of work. What is the entropy change of the gas (in J/K)?
In an isothermal reversible expansion at 23°C, an ideal gas does 55 J of work. What...
An ideal gas undergoes a reversible isothermal expansion at 57.0 degree C, increasing it's volume from 1.50 L to4.50 L. The entropy change of the gas is 36.0 J/K. How many moles of gas are present?
Three moles of an ideal gas undergo a reversible isothermal compression at 22.0 ∘C. During this compression, 1700 J of work is done on the gas. Q: What is the change in entropy of the gas? (J/K)
Three moles of an ideal gas undergo a reversible isothermal compression at temperature 17.0 degree C. During this compression, an amount of work totalling 1600 J is done on the gas. What is the change of entropy of the gas? What is the change of entropy of the gass?
5. Isothermal (87°C) reversible expansion of 3.00 moles of an ideal gas from 7.00 to 13.00 liters. (Cv.m=(3/2)R a. Calculate AS for the reversible expansion. b. Calculate w (work). c. What are AU and AH, the change in internal energy and change in enthalpy, respectively?
One mole of an ideal gas undergoes a reversible isothermal expansion from a volume of 1 L to a volume of 2 L. The change in entropy of the gas in terms of the universal gas constant R is? Final Answer is R ln(2), but I need to know how to calculate this
During a reversible isothermal expansion, the entropy of an ideal gas: a) decreases b) stays constant c) increases When dry ice sublimes into gas at 194.65 K and 1 atm, the entropy a) increases b) stays constant c) decreases Which one of the following is true? a) The entropy of an isolated system can only stay constant or increase during a process b) We can construct a heat engine that extracts heat from a hot reservoir and delivers an equal...
A gas sample undergoes a reversible isothermal expansion. The figure gives the change AS in entropy of the gas versus the final volume Vf of the gas. The scale of the vertical axis is set by ΔSs = 73.7 J/K. How many moles are in the sample? 0.8 1.6 2.4 3.2 4.0 Vy (m3)
22 g of Co, gas is in a container under 1.50 bar. After isothermal reversible expansion, volume of the gas changes from 2 dm to 5 dm'. Calculate the change in the system's entropy? (C: 12 g/mol; O: 16 g/mol) (R-8.314 1/mol.) A-) 6.69 J/K B-) 335.2 J/K C-) 3.81 J/K D-) 0.458 J/K E-) 167.6 J/K
Two moles of an ideal gas undergo a reversible isothermal expansion from 2.41×10−2 m3 to 4.42×10−2 m3 at a temperature of 26.7 ∘C. What is the change in entropy ΔS of the gas? Express your answer numerically in joules per kelvin.
b) How much energy must be transferred as heat for the reversible isothermal expansion of an ideal gas at 159.0 C, if the entropy of the gas increases by 52.0)/K?