***CHEMICAL KINETICS PROBLEM***PLEASE HELP*** ***Many people have done this prob

Question

***CHEMICAL KINETICS PROBLEM***PLEASE HELP***

***Many people have done this problem but have gotten the wrong solution. Please be carfeul***

1. Suppose you inject 30.0 mL of air (initially at a temperature of 23.5 deg. Celcius and a pressure of 0.983 atm) into a bottle at the same temperature and pressure. After the injection, the pressure is observed to be 1.014 atm with no change in temperature .

A. How many moles of gas were in the syringe to cause this pressure change?

B. Calculate the mole-to-pressure change ratio (a conversion factor)

Explanation / Answer

V1 = 30 ml

T1 = 23.5C = 296.5K

P1 = 0.983 atm or 99.6 kPa

T2 = T1

P2 = 1.014 atm

Important NOTES

* Assume all 30 ml are injected

* Assume there is no reaction between substance (initially),.. If this is no the case, then it is impossible to solve.

* Assume ideal gas las

PV = nRT

n = PV/(RT) = 0.983*(30/1000) / (0.0082*296.5) =0.01213 gmol of substance (air)

B)

Mole to ¨PRessure change ratio

dMol/dP

dP = 1.014 - 0.983 = 0.027 atm

dMol = 0.01213 gmol

Ratio = 0.01213/0.027 = 0.449 mol/atm

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