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question_answer1) Sulphur dioxide and oxygen were allowed to diffuse through a porous partition. \[20\text{ }d{{m}^{3}}\] of \[S{{O}_{2}}\] diffuses through the porous partition in 60 seconds. Calculate the volume of \[{{O}_{2}}\] in \[d{{m}^{3}}\] which diffuses under the similar condition in 30 seconds (atomic mass of sulphur = 32 u).
question_answer2) 4.5 g of \[PC{{l}_{5}}\] on vapourisation occupied a volume of 1700 mL at 1 atmosphere pressure and \[227{}^\circ C\] temperature. Calculate its degree of dissociation.
question_answer3) A spherical balloon of 21 cm diameter is to be filled up with hydrogen at N.T.P. from a cylinder containing the gas at 20 atmospheres at \[27{}^\circ C.\] If the cylinder can hold 2.82 litres of water, calculate the number of balloons that can be filled up.
question_answer4) At \[27{}^\circ C\] hydrogen is leaked through a tiny hole into a vessel for 20 minutes. Another unknown gas at the same temperature and pressure as that of \[{{H}_{2}}\] is leaked through the same hole for 20 minutes. After the effusion of the gases the mixture exerts a pressure of 6 atmosphere. The hydrogen content of the mixture is 0.7 mole. If the volume of the container is 3 litres, what is the molecular weight of the unknown gas?
question_answer5) A bubble of gas released at the bottom of a lake increases to four times its original volume when it reaches the surface. Assuming that atmospheric pressure is equivalent to the pressure exerted by a column of water 10m high, what is the depth of the lake (in m)?
question_answer6) A mixture of \[N{{H}_{3}}\,(g)\] and \[{{N}_{2}}{{H}_{4}}(g)\] is placed in a sealed container at 300 K. The total pressure is 0.5 atm. The container is heated to 1200 K at which both substances decompose completely according to the equations \[2N{{H}_{3}}(g)\to {{N}_{2}}(g)+3{{H}_{2}}(g)\] and \[{{N}_{2}}{{H}_{4}}(g)\to {{N}_{2}}(g)+2{{H}_{2}}(g)\] After decomposition is complete, the total pressure at 1200 K is found to be 4.5 atm. Find the mole % of \[{{N}_{2}}{{H}_{4}}\] in the original mixture.
question_answer7) If 250 mL of \[{{N}_{2}}\] over water at \[30{}^\circ C\] and a total pressure of 740 torr is mixed with 300 mL of Ne over water at \[25{}^\circ C\] and a total pressure of 780 torr, what will be the total pressure if the mixture is in a 500 mL vessel over water at \[35{}^\circ C\]? Given: vapour pressure (Aqueous tension) of \[{{H}_{2}}O\] at \[25{}^\circ C\], \[30{}^\circ C\] and \[35{}^\circ C\] are 23.8, 31.8 and 42.2 torr respectively Assume volume of \[{{H}_{2}}O(l)\] is negligible in final vessel)
question_answer8) At 300 K, the density of a certain gaseous molecule at 2 bar is double to that of dinitrogen \[({{N}_{2}})\] at 4 bar. Find the molar mass of gaseous molecule.
question_answer9) Calculate the total pressure (in atm) in a 10.0 L cylinder which contains 0.4 g helium, 1.6 g oxygen and 1.4 g nitrogen at \[27{}^\circ C\].
question_answer10) At STP, a container has 1 mole of He, 2 mole Ne, 3 mole and 4 mole \[{{N}_{2}}\] without changing total pressure if 2 mole of \[{{O}_{2}}\] is removed. Calculate the percentage decrease in the partial pressure of \[{{O}_{2}}\].
question_answer11) A gaseous mixture contains three gases A, B and C with a total number of moles of 10 and total pressure of 10 atm. The partial pressure of A and B are 3 atm and 1 atm respectively. If C has molecular weight of 2 g/mol then, then find the weight of C in grams present in the mixture.
question_answer12) Two flasks A and B of equal volumes maintained at temperatures 300K and 600K contain equal mass of \[{{H}_{2}}\] and \[C{{H}_{4}}\]respectively. Calculate the ratio of total translational kinetic energy of gas in flask A to that in flask B.
question_answer13) If one mole of mono-atomic gas \[(\gamma =5/3)\] is mixed with one mole of a diatomic gas \[(\gamma =7/5).\] What is the value of \[\gamma \] for the mixture.
question_answer14) A mixture of Ne and Ar kept in a closed vessel at 250 K has a total K.E. of 3 kJ. The total mass of Ne and Ar is 30 g. Find mass % of Ne in gaseous mixture at 250 K.
question_answer15) What is the compressibility factor (Z) for 0.02 mole of a van der Waals' gas at pressure of 0.1 atm. Assume the size of gas molecules is negligible. Given: \[RT=20\text{ }L\text{ }atm\text{ }mo{{l}^{-\,1}}\] and \[a=1000\] \[atm\,{{L}^{2}}\,mo{{l}^{-2}}\]
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