y eview fassigimentProblemID- 105177264&offs Chem 1B TTh CCC Fall 2018 KChapter
ID: 716247 • Letter: Y
Question
y eview fassigimentProblemID- 105177264&offs Chem 1B TTh CCC Fall 2018 KChapter 15 Exercise 15.60 - Enhanced- with Feedback Part A Consider the following reaction Calculate the equilibrium partial pressure of CO2 Express the pressure in torr to three significant figures. CO(g) + H20(g)CO2(g) H2(8) Kp 0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1340 torr and a H2O partial pressure of 1710 torr at 2000 K You may want to reference (Pages 693 -702) Section 15.8 while completing this problem. torr Submit Request Answer Part B Complete previous part(s) Provide FeedbackExplanation / Answer
CO(g ) + H20(g) --> CO2(g) + H2(g)
t=0sec 1340 torr 1710 torr
t=eq. 1340-p 1710-p p p
Kp=(PCO2*PH2)/(PCO*PH20)
0.0611=(p*p)/(1340-p)*(1710-p)
16.37 p2=(1340-p)*(1710-p)
16.37p2=2291400 - 3050 p + p2
15.37 p2+3050 p -2291400=0
Solving the quadratic equation,we get two roots out of which one will be neglected since pressure can't be negative.So,-
p(equilibrium partial pressure of CO2)=299 torr{upto 3 significant figures}
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.