InterviewSolution
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InterviewSolution
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1500 mL flask contains `400 mg O_(2) " and " 60 mg H_(2) " at " 100^(@)C`. (a) What is the total pressure in the flask ? (b) If the mixture is permitted to react to form water vapour at `100^(@)C`, what will be left and what will be their partial pressure ? |
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Answer» (a) No. of moles of `O_(2) = (400)/(1000 xx 32) = 0.0125` No. of moles of `H_(2) = (60)/(1000 xx 2) = 0.03` Partial pressure of `O_(2) = (0.0125 xx 0.0821 xx 373)/(1.5) = 0.255 atm` Partial pressure of `H_(2) = (0.03 xx 0.0821 xx 373)/(1.5) = 0.612 atm` Total pressure `= 0.255 + 0.612 = 0.867 atm` (b) `{:(,2H_(2),+O_(2),= 2H_(2) O),("Initital",0.03,0.0125," "0),("After reaction",0.005,0," "0.025):}` Partial pressure of `H_(2) = (0.005 xx 0.0821 xx 373)/(1.5) = 0.102 atm` Partial pressure of `H_(2) O = (0.025 xx 0.0821 xx 373)/(1.5) = 0.51 atm` |
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