Suppose 6.36 moles of a monatomic ideal gas expand adiabatically, and its temperature decreases from 387 to 263 K. Determine (a) the work done (including the algebraic sign) by the gas, and (b) the change in its internal energy.

Assume 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 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