Calculate how much heat in J has to be added to a sample of an ideal monoatomic gas at a pressure of 2.0x105 N/m2 and a temperature of 310 K so it undergoes a quasi-static isobaric expansion from 2.2x103 cm3 to 3.9x103 cm3 . I was told to start with the first law, and consider both how much E (internal energy) changes during the expansion, and W (work done by the system).

A car tire contains 0.0440 m3 of air at a pressure of 2.75 x 10° N/m2 (about 40 psi). How much more internal energy (in J) does this gas have than the same volume has at zero gauge pressure (which is equivalent to normal atmospheric pressure)? (Assume the tire pressure of 2.75 x 105 N/m2 is absolute pressure, not gauge pressure. Assume for this question that air is monatomic.) Additional Materials O Reading Submit Answer

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 %3D

A 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 cylinder containing n mol of an ideal gas undergoes an adibatic process. Starting with dW = pdV and using the condition pVY = constant, show that the work done by the gas: 1 W × (p;V; - PfV¢) %3D Starting from the first law of thermodynamics in differential form, prove that the work done by the gas is n×Cy(T; - Tf).

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) J

One mole of an ideal gas, for which CV,m = 3/2R, initially at 298 K and 1.00 × 10^5 Pa undergoes a reversible adiabatic compression. At the end of the process, the pressure is 1.00 × 10^6 Pa. Calculate the final temperature of the gas. Calculate q, w, ΔU, and ΔH for this process.