In a constant-volume process, 216 J of energy is transferred by heat to 0.98 mol of an ideal monatomic gas initially at 309 K. (a) Find the work done on the gas. (b) Find the increase in internal energy of the gas. (C) Find its final temperature.
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Q: Find the work done on the gas.
A: Given: A constant-volume process of an ideal monatomic gas. Initial temperature is Ti=309 K Heat…
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- 1.013 x 10° Pa) and We consider a 5.15-L sample of monatomic ideal gas at atmospheric pressure (1 atm 302 K. This initial state would be called point A, if we were to draw the process on a pV diagram (you should!). The gas is then heated at constant volume to 3.00 atm (point B). It then undergoes an isothermal expansion (point C) and is then compressed isobarically to its original state (point A). a. What is the number of moles of the sample? mol b. What are the temperatures at point B? K c. What are the temperatures at point C? K d. What is the volume at point C? L e. During the isothermal expansiom (B to C), calculate the following quantities The change in internal energy AE = %3D The work done by the gas is W = kJ The heat added to the gas is Q = kJ %3DIn a constant-volume process, 208 J of energy is transferred by heat to 1.07 mol of an ideal monatomic gas initially at 303 K. (a) Find the work done on the gas. (b) Find the increase in internal energy of the gas. (c) Find its final temperature. KA 2.00 mol sample of an ideal diatomic gas at a pressure of 1.10 atm and temperature of 420 K undergoes a process in which its pressure increases linearly with temperature. The final temperature and pressure are 720 K and 1.70 atm . Fid the change in internal energy, work done by the gas, and heat added.
- A balloon holding 4.50 moles of oxygen (0,) gas absorbs 935 J of thermal energy while doing 112 J of work expanding to a larger volume. HINT (a) Apply the first law of thermodynamics. (b) Recall that the molar specific heat at constant volume, C, takes different values depending on whether the gas is monatomic or diatomic. Click the hint button again to remove this hint. (a) Find the change in the balloon's internal energy (in J). (b) Calculate the change in temperature of the gas (in K). K2.0 moles of an ideal gas is initially at P = 1.0 atm and T = 300 K. It is then taken through a three-step reversible process: (i) isobaric expansion to twice its original volume; (ii) isothermal compression, returning to its original volume; (iii) isochoric reduction in pressure to the original state. Find the work done on the gas in each step of the process and the net work done on the gas for the process.A 1.70-mol sample of hydrogen gas is heated at constant pressure from 302 K to 426 K. (a) Calculate the energy transferred to the gas by heat. kJ (b) Calculate the increase in its internal energy. k] (c) Calculate the work done on the gas. kJ