For the process: H 2 O(s) ? H 2 O(l) ; ? H = 6.0 x 10 3 J. Calculate the ?S surr
ID: 789734 • Letter: F
Question
For the process: H2O(s) ? H2O(l) ; ? H = 6.0 x 103 J. Calculate the ?Ssurr at 0oC.
The system: 2NO2(g) ? N2O4(g) ?H = -14 kcal ; increasing the temperature will _____ the equilibriun constant value
For the system: 2CO(g) + O2(g) ? 2CO2(g) ; decreasing the volume of the container will shift the equilibrium:
The system: A(g) ? 2B(g) Kc = 1.0 x 10-4 initially [A] = 0.22M . The equilibrium concentration of B is
For the reaction: I2(g) + Cl2g) ? 2ICl(g) the Kp value is 3.4 x 10-2
The Kp value for: 2ICl(g) ?I2(g) + Cl2g) is 29
For the system: H2(g) + Cl2(g) ? 2HCl(g) ; ?Go = -190.6 kJ at 25oC. Calculate the equilibrium constant. (be careful of the negative sign)
Calculate Keq for the reaction: A(g) + B(g) ? C(g) + D(g) given Kp = 3.1 x 10-4 @ 35
A. -6 J/K B. -22 J/K C. 0 J/KExplanation / Answer
1) C
2) A
3) A
4) B
5) True
6) C
7) C