One mole of a monatomic ideal gas is initially at 273 K and 1 atm. (a) What is its initial internal energy? (b) Find its final internal energy and the work done by the gas when 500 J of heat are added at constant pressure. (c) Find the same quantities when 500 J of heat are added at constant volume.
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- In a constant-volume process, 206 J of energy is transferred by heat to 0.97 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.In 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. KSuppose 3.32 moles of a monatomic ideal gas expand adiabatically, and its temperature decreases from 371 to 254 K. Determine (a) the work done (including the algebraic sign) by the gas, and (b) the change in its internal energy.
- 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). KAssume that 9.63 moles of a monatomic ideal gas expand adiabatically, lowering the temperature from 388 to 262 K. Calculate (a) the work done by the gas (including the algebraic sign) and (b) the change in the gas's internal energy.A monatomic ideal gas expands adiabatically from 1.8 m³ to 4 m³. If the initial pressure is 102 kPa, calculate the energy in kJ transferred to or from the system by heat.
- An ideal monatomic gas expands adiabatically from 0.530 m³ to 1.72 m³. If the initial pressure and temperature are 1.30 × 105 Pa and 355 K, respectively, find the number of moles in the gas, the final gas pressure, the final gas temperature, and the work done on the gas. HINT (a) the number of moles in the gas (Enter your answer to at least three significant figures.) mol (b) the final gas pressure (Enter your answer in Pa, to at least three significant figures.) Pa (c) the final gas temperature (in K) K (d) the work done on the gas (in J) JPlease help meAn ideal gas expands at constant pressure. (a) Show that PΔV = nRΔT. (b) If the gas is monatomic, start from the definition of internal energy and show that ΔU = 3/2 Wenv, where Wenv is the work done by the gas on its environment. (c) For the same monatomic ideal gas, show with the first law that Q = 5/2 Wenv. (d) Is it possible for an ideal gas to expand at constant pressure while exhausting thermal energy? Explain.