Consider the following gas-phase reaction:
C2H2(g) + 4 Cl2(g) 2CCl4(g) + H2(g)
Using data from Appendix C of your textbook calculate thetemperature, To, at which this reaction will be atequilibrium under standard conditions (Go = 0) andchoose whether >Go will increase, decrease, or notchange with increasing temperature from the pulldown menu.
To = K, and Go will
---Select---
increase
decrease
not change with increasing temperature.
For each of the temperatures listed below calculateGo for the reaction above, and select from the pulldownmenu whether the reaction under standard conditions will bespontaneous, nonspontaneous, or near equilibrium (\"nearequilibrium\" means that T is within 5 K of To).
(a) At T = 1282 K Go = kJ/mol, and the reactionis
---Select---
spontaneous
nonspontaneous
near equilibrium under standard conditions.
(b) At T = 1923 K Go = kJ/mol, and the reactionis
---Select---
spontaneous
nonspontaneous
near equilibrium under standard conditions.
(c) At T = 641 K Go = kJ/mol, and the reaction is
---Select---
spontaneous
nonspontaneous
near equilibrium under standard conditions.
