Questions LLC
Login
or
Sign Up
Ask a New Question
Chemistry
Reaction Equilibrium
Calculating Kc
The value of kp at 20°c for the reaction 2NO(g) + Cl2(g) 2NOCl(g) is 1.9x10^3 atm-1 calculate the value of KC at the same temperature
1 answer
Kp = Kc*(RT)^delta n
1900 = Kc*(0.08205*293)^-1
Solve for Kc.
You can
ask a new question
or
answer this question
.
Related Questions
Consider the reaction:
I2(g) + Cl2(g) 2 ICl(g) Kp = 81.9 at 25°C Calculate ΔGrxn for the reaction at 25°C under each of the
What is occurring in the following reaction?
H2 + Cl2 → 2HCl A. H2 is being reduced. B. Cl2 is being oxidized. C. H2 is gaining
The equilibrium constant Kp for the reaction below at 700°C is 0.76 atm.
CCl4(g) --> C(s) + 2 Cl2(g) Determine the initial
Nitrogen monoxide reacts with chlorine gas according to the reaction:
2NO (g) + Cl2 (g) ⇔ 2NOCl (g) Kp = 0.27 at 700 K A
Consider the following reaction:
I2(g) + Cl2(g) 2ICl(g) o Kp = 81.9 at 25 C. Calculate ∆Grxn for the reaction at 25 C under
The reaction 2NO (g) + 2H2 -> N2 (g) + 2H2O (g) was found to follow the rate law, rate = k[NO]^2[H2]. By what factor will the
Determine the values of Kc that correspond to the following values of Kp
(a) SO2Cl2(g)--->SO2(g) + Cl2(g) Kp= 2.9 x 10^-2 at 303
Consider the following reaction:
2NOCl(g) 2NO(g) + Cl2(g) Initially pure NOCl(g) is placed in a vessel at 3.00 atm. At
2.5 mol NOCl(g) was placed in a 2.50 L reaction vessel at 400 degrees C. After equilibrium was established, it was found that
A mixture of 0.47 mole of H2 and 3.59 moles of HCl is heated to 2800C. Calculate the equilibrium partial pressures of H2 Cl2 and