InterviewSolution
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InterviewSolution
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1 mole of `H_(2)` gas is contained in box of volume `V= 1.00 m^(3) at T = 300 K`. The gas is heated to a temperature of T = 3000 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)A. same as the pressure initially.B. 2 times the pressure initially.C. 10 times the pressure initiallyD. 20 times the pressure initially |
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Answer» Correct Answer - D Applying standard gas equation, `(P_(2)V_(2))/(T_2) = (P_(1)V_(1))/(T_1)` `(P_2)/(P_1) = (V_1)/(V_2)* (T_2)/(T_1)` As, `(T_2)/(T_1) = 3000/300 =10`, and every molecule of `H_(2)` splits into hydrogen atoms, dubling the number, therefore volume available to given number of entities becomes half i.e. `V_(2) = 1/2 V_(1)`, therefore, `(P_2)/(P_1) = 2 xx 10 = 20`. |
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