Question

A mixture of propane and oxygen in a 1L closed vessel has an internal pressure of 4atm. at 373K. When the mixture is ignited, the reaction produces CO2(g) and H2O(g) until all the oxygen is consumed. After the reaction, the pressure of the vessel is 4.2atm at the same temperature. Calculate the weight of the oxygen present before the reaction. (gas constant R= 0.082 atm mol-1 L K-1)

Answer 1

nobody to help me on this ques???

Answer 2

what's the balanced reaction that takes place?

Answer 3

\[C _{3}H _{8} + 5O _{2}= 3CO _{2} + 4H _{2}O

Answer 4

\[C _{3}H _{8} + 5O _{_{2}} = 3CO _{2} + 4H _{2}O \]

Answer 5

Basically you want to set up a table for "initial moles" and then "at equilibrium". From there you denote some x value to be the number of moles (of any of the reactants) that was consumed in the process. OBEY Stoichiometry. From there you can set up an expression like P1=(n moles reactants initial)RT/V which equals P2=(n moles reactants final)RT/V.... You can then manipulate these equations (Divide) to find your answer.

Answer 6

Anyway if you want to go through the problem completely i can do that for you. MAke an attempt and see where we get.... :)