A gas at a pressure of 100 atmospheres and temperature of 300 K is suddenly (i.e. adiabatically) compressed from having a volume of 1 liter to a volume of 0.5 liters. What is the new pressure? What if, instead, the compression is done very slowly?
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A gas at a pressure of 100 atmospheres and temperature of 300 K is suddenly (i.e. adiabatically) compressed from having a volume of 1 liter to a volume of 0.5 liters. What is the new pressure? What if, instead, the compression is done very slowly?
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- A sample of gas is compressed to one-third of its initial volume at a constant pressure of 1.25 × 105 Pa. During the compression 100J of work is done on the gas. What is the final volume of the gas?An ideal gas initially at 340 K undergoes an isobaric expansion at 2.50 kPa. The volume increases from 1.00 m3 to 3.00 m3 and 12.6 kJ is transferred to the gas by heat. (a) What is the change in internal energy of the gas? kJ (b) What is the final temperature of the gas? KAn ideal gas, initially at a pressure of 10.3 atm and a temperature of 312 K, is allowed to expand adiabatically until its volume doubles. What is the gas’s final temperature, in kelvin, if the gas is monatomic? What is the gas’s final pressure, in atmospheres, if the gas is diatomic?
- A cylinder of volume 0.320 m3 contains 10.5 mol of neon gas at 17.4°C. Assume neon behaves as an ideal gas. (a) What is the pressure of the gas? Pa(b) Find the internal energy of the gas. J(c) Suppose the gas expands at constant pressure to a volume of 1.000 m3. How much work is done on the gas? J(d) What is the temperature of the gas at the new volume? K(e) Find the internal energy of the gas when its volume is 1.000 m3. J(f) Compute the change in the internal energy during the expansion. J(g) Compute ΔU − W. J(h) Must thermal energy be transferred to the gas during the constant pressure expansion or be taken away? This answer has not been graded yet. (i) Compute Q, the thermal energy transfer. J(j) What symbolic relationship between Q, ΔU, and W is suggested by the values obtained?A sample of n = 2.00 moles of monoatomic ideal gas expands adiabatically, the work done on the gas is W = -5.00 x 103 J. The initial temperature and pressure of the gas are Ti = 600 K and Pi = 4.05 x 105 Pa. Calculate: a) the final temperature of the gas; b) the final pressure of the gas. R = 8.314 J/mol KA sealed cylinder has a piston and contains 8.90×103 cm3 of an ideal gas at a pressure of 7.50 atm. Heat is slowly introduced, and the gas isothermally expands to 1.70×104 cm3. How much work ? does the gas do on the piston?
- One mole of an ideal gas does 3900 J of work as it expands isothermally to a final pressure of 1.00 atm and volume of 0.022 m3. What was the initial volume of the gas, in cubic meters? What is the temperature of the gas, in kelvin?tab Consider the following figure. (The x axis is marked in increments of 2.5 m³.) P (Pa). esc caps lock 6 x 106 4 X 106 2 x 106 V (m³) 1 (a) Determine the work done on a gas that expands from i to f as indicated in the figure. MJ (b) How much work is performed on the gas if it is compressed from f to / along the same path? MJ ! 1 F1 A NO 2 N FF 200 F2 W S # 3 80 F3 X E * D $ 4 F4 R C % 5 F MacBook Air T V の‥ 6 F6 G & 7 F7 H B 2 EAn ideal gas is taken through a quasi-static process described by P = aV2, with a = 2.60 atm/m6, as shown in the figure. The gas is expanded to twice its original volume of 1.00 m³. How much work is done on the expanding gas in this process? MJ P=av² 1.00 m³ 2.00 m³