Heat & Thermodynamics
In an adiabatic process 90 J of work is done on the gas. The change in internal energy of the gas is
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A flask of 1L having NH3(g) at 2.0atm and 200K is connected with the another flask of volume 800mL having HCI(g) at 8atm and 200K through a narrow tube of negligible volume. The two gases react to form NH4(CI(s) with evolution of 43kJmol−1 heat. if heat capacity of HCI(g) at constant volume is 20JK−1mol−1 and neglecting heat capacity of flask, and volume of solid NH4CI formed, calculate the final temperature, and final pressure in the flasks. (Assume R=0.08LatmK−1mol−1)
A system undergoes a process in which ΔU=+300J while absorbing 400j of heat energy and undergoing an expansion 0.5 bar. What is the change in the volume(in L)?
Calculate heat required to raise the temperature of 1 g of water by 1oC?
When an idea gas in a cylinder was compressed isothermally by a piston, the work done on the gas found to be 1.5×104 joules. During this process about
Figur shows P−T diagram for a given mass of an ideal gas for the process A→B. during this process, density of the gas is
One mole of an ideal monoatomic gas is heated a constant pressure of one atmosphere from 0oC to 100oC. Then the work done by gas is
Heat energy absorbed by a system in going through a cyclic process shown in Fig. 2.123 is
Refer to figure. Let ΔU1 and ΔU2 be the changes in internal energy of the system in the processes A andB. Then