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question_answer1) 110 J of heat are added to a gaseous system by which internal energy increases by 40 J, find the amount of work done (in J)
question_answer2) During an adiabatic change for monatomic gas the relation between pressure of a gas and temperature T is \[P\propto {{T}^{x}}\]where x is ?
question_answer3) A polyatomic gas with six degree of freedom does 25J work when it is expended at constant pressure. The heat given to the gas is (in J)
question_answer4) A diatomic gas follows equation\[P{{V}^{m}}=\] constant, during a process. What should be the value of m such that its molar heat capacity during process\[=R\]
question_answer5) An ideal gas is enclosed in an insulated vessel is heated through a coil of resistance \[100\Omega \] carrying current 1A for 5 minutes. Then change in internal energy will be(in kJ)
question_answer6) Two spherical vessels of equal volume are connected by a narrow tube. The apparatus contains an ideal gas at one atmosphere and 300K. Now if one vessel is immersed in a bath of constant temperature 600K and the other in a bath of constant temperature 300K, then the common pressure will be?
question_answer7) One mole of a perfect gas, initially at a pressure and temperature of \[{{10}^{5}}N/{{m}^{2}}\]and 300K respectively expends isothermally until its volume is doubled and then adiabatically until its volume is again doubled. Find the total work done (in J) during the isothermal and adiabatic processes. (Given\[\gamma =1.4,\,\ell n2=0.693,\,{{2}^{0.4}}=1.319\])
question_answer8) A closed container of volume 0.02\[{{m}^{3}}\]contains a mixture of neon and argon gases, at a temperature of \[27{}^\circ C\]and pressure of\[1\times {{10}^{5}}N{{m}^{-2}}\]. The total mass of the mixture is 28g. If the molar masses of neon and argon are 20 and 40g per mole, respectively, then the mass(in gram) of the neon in the container, assuming them to be ideal is ?
question_answer9) Calculate the work done (in J) on the gas when one mole of a perfect gas is compressed adiabatically. The initial pressure and volume of the gas are \[{{10}^{5}}N/.{{m}^{2}}\]and 6 litres respectively. The final volume of the gas is 2 litres. Molar specific heat of the gas at constant volume is 3R/2?
question_answer10) One mole of an ideal gas requires 204 J heat to raise the temperature by 10 K when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same 10 K, then the heat required(in J) is-
question_answer11) 70 calories of heat required to raise the temperature of 2 moles of an ideal diatomic gas at constant pressure form \[30{}^\circ C\]and\[35{}^\circ C\]. The amount of heat required (in calories) to raise the temperature of the same gas through the same range (\[30{}^\circ C\]to \[35{}^\circ C\]) at constant volume is-
question_answer12) The internal energy of a monoatomic ideal gas is 1.5 nRT. One mole of helium is kept in a cylinder of cross-section\[A=8.5c{{m}^{2}}\]. The cylinder is closed by a light frictionless piston. The gas is slowly heated in a process during which a total of 42 J heat is given to the gas. If the temperature rises through\[2{}^\circ C\], find the displacement (dx) (in cm) of the piston. Atmospheric pressure \[=100\text{ }kPa.\]
question_answer13) Three moles of an ideal gas at 300 K are isothermally expended to five times its volume and heated at this constant volume so that the pressure is raised to its initial value before expansion. In the whole process 83.14 kJ heat is required. Calculate the ratio \[{{C}_{P}}/{{C}_{V}}\]of gas \[\left( {{\log }_{e}}5=1.61 \right)\]
question_answer14) What amount of heat (in J) is to be transferred to nitrogen in the isobaric heating process for that gas to perform the work\[\Delta W=2.0J\]?
question_answer15) Figure shows the variation in the internal energy U with the volume V of 2.0 mole of an ideal gas in a cyclic process abcda. The temperatures of the gas at b and c are 500 K and 300 K respectively. Calculate the heat absorbed by the gas during the process.
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