At 700 K the equilibrium constant for the reaction
CCl4(g)←−→C(s)+2Cl2(g)
is Kp=0.76. A flask is charged with 2.00 atm of CCl4, which then reaches equilibrium at 700 K.
1) What fraction of the CCl4 is converted into C and Cl2?
2) What is the partial pressure of CCl4 at equilibrium?
3) What is the partial pressure of Cl2 at equilibrium?
The answer to the question is available in the PDF file https://www.assignmentexpert.com/https://www.assignmentexpert.com/homework-answers/chemistry-answer-63428.pdf
Numbers and figures are an essential part of our world, necessary for almost everything we do every day. As important…
APPROVED BY CLIENTS
Finding a professional expert in "partial differential equations" in the advanced level is difficult.
You can find this expert in "Assignmentexpert.com" with confidence.
Exceptional experts! I appreciate your help. God bless you!
Comments
Leave a comment