can someone explain to me how to do this question step by step and what equation
ID: 1002250 • Letter: C
Question
can someone explain to me how to do this question step by step and what equations are needed ? thank you very much A 3.07 g sample of trans-4-methylcyclohexanol (formula C7H14O), is mixed with 11.61 atm of O2 in a 1.02 L combustion chamber at 109.27 °C. The combustion reaction to CO2 and H2O is initiated and the vessel is cooled back to 109.27 °C. Report all answers to two decimal places in standard notation (i.e. 1.23 atm). 1. What is PCO2 (in atm) in the combustion chamber assuming the reaction goes to completion? Assume all water is water vapour and that the volume of the systemdoes not change. 2. What is PO2 (in atm) in the combustion chamberafter the reaction goes to completion?Explanation / Answer
The conbustion reaction is C7H14O + 10O2---> 7CO2 + 7H2O
molecular weight of C7H14O= 7*12+14+16= 114, moles of C7H14O=3.07/114=0.02693
moles of oxygen supplied can be calculated from PV/RT = 11.61*1.02/(0.0821*(109.27+273.15)=0.37 moles
Oxygen required is 10 times the moles of C7H14O= 10*0.02693= 0.2693, Oxygen is excess and exces moles of oxygen =0.37-0.2693=0.1007 moles
Product gases contains CO2, H2O and unreacted oxygen
moles of CO2 forned= 7*0.02693 =0.1885, moles of water formed = 0.1885 , moles of oxygen =0.1007
total moles = 0.4777 Partial pressure of CO2= mole fraction of CO2* total pressure = (0.1885/0.4777)*1.23 atm=0.4854 atm, partial pressure of oxygen= (0.1007/0.4777)*1.23=0.2593 atm
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