posted by .

1) Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is

2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227oC

Using delta Ho = 81.2 kJ and delta So = 128 J/K, calculate the value of the equilibrium constant for this reaction.

I do not know how to start this problem or what formula I should use.

dGo = dHo - TdSo
Then dGo = -RTlnK

So for delta G= delta H - T delta S it would be delta G= 81200 J/K - 500K(128J/k)

This would equal 17200. Did I do this correctly so far before I move on?

## Similar Questions

1. ### Ap Chemistry

Hi, I was wondering if you could possibly help me with this chem question. For the relatively slow decomposition of NOCL into NO and Cl2 according to the reaction below, it is known that the reaction is second order w/ respect to NOCl …
2. ### chemistry 101

Calculate (delta) H rxn for 2NOCl(g)---- N2(g) + O2(g) + Cl(g) given the following set of reactions: 1/2N2(g) + 1/2O2(g)-----NO(g) delta H =90.3kJ NO(g) + 1/2Cl2(g)----NOCl(g) delta H = -38.6 kJ
3. ### Chemistry

0.500 moles of NOCl is placed in a 1.00L vessel at 700K,and after the system comes to equilibrium,the concentration of the NOCl is .440M. Calculate the value of Kc for the reaction @NOCl(g)->2NO(g)+Cl2(g)?
4. ### chemistry

Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is 2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227C Using delta H = 81.2 kJ and delta S = 128 J/K, calculate the value of the equilibrium constant for this reaction. …
5. ### chemistry

Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is 2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227C Using delta H = 81.2 kJ and delta S = 128 J/K, calculate the value of the equilibrium constant for this reaction. …

1) Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is 2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227oC Using delta Ho = 81.2 kJ and delta So = 128 J/K, calculate the value of the equilibrium constant for this reaction. …
7. ### Chemistry

Nitric oxide reacts with chlorine to form nitrosyl chloride, NOCl. Use the following data to determine the rate equation for the reaction. NO + (1/2)Cl2 -> NOCl Expt.[NO] [Cl2] Initial rate 1 0.22 0.065 0.96 M/min 2 0.66 0.065 8.6 …
8. ### Chemistry

NOCL(g) decomposes to from nitrogen monoxide gas and chlorine gas. The equation is 2NOCL ----> 2NO +Cl2 At a certain temperature the equilibrium constant is 1.60 x 10^-6. Calculate the equilibrium concentrations of all gases if …
9. ### chem 12

consider the following equilibrium 2NOCl(g)--- 2 NO(g) + Cl2(g) Initally 1.00 mol of NO and 1.00 mol of Cl2 are placed in a 5.00L container. Calculate the initial concentrations of NOCl, NO and Cl2 NO= 0.20 mol/L Cl2= 0.20 mol/l NOCl=0 …
10. ### Chemistry Honors

Nitrosyl chloride (NOCl)decomposes to nitrogen oxide and chlorine gases. The concentration of NOCl drops from 0.580 M to 0.238 M in 8.00 min. Calculate the average rate of reaction over this time interval.

More Similar Questions