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1.) For the reaction 2NOCl(g) = 2NO(g) + Cl2 (g)
the value of Kp at 50 degrees Celsius is 4.2 x 10^-4 atm. What isthe value of Kc at this temperature.

for this I have the Kc= [NOCl]^2 / [NO]^2 x [Cl2]

2.) When heated, carbon monoxide reacts with water according to theequation
CO(g) + H2O(g) = CO2(g) + H2(g)
The value of the equilibrium constant for this reaction is 2.2 at700 celsius. What will be the concentrations of all gases atequilibrium, when 2.00 mol of CO and 2. mol of H20 are mixed in a 2liter reactor and heated to 700.

* I know you make an ICE chart..but I don't know where to go fromthere.

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Jean Keeling
Jean KeelingLv2
28 Sep 2019

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Related questions

Cosider the reaction

2NOCl(g) <--> 2NO(g) + Cl2(g)

Which takes place at 295 K. Equilibrium constant Kc=1.6x10^-5

A) You place 4 g of NOCl in a 2 liter flask. What are the equilibrium concentrations of each species?

B)What is the pressure of the flask at equilibrium? **I used Kp=(1.6x10^-5)(.0821x295) for part b yet still got the wrong answer. I know it should be raised to the power of delta n but how exactly do you find delta n for this particular question?

Please show work for each questions so I can better understand. thank you!!!!

please help and explain... I am beyond lost on this assignment

1. A certain process has ∆H◦>0 and ∆S◦<0. Which of the following is a correct conclusion about this process

Non spontaneous at all T.

Spontaneous at high T / Spontaneous at low T / Spontaneous at all T / None of the above­­­­­­­­­­­­­­­­­­­

2. the formation constant for the reaction Ag+(aq)+2NH3(aq) ß-à Ag(NH3)2+(aq) is K=1.7x10^7 at 25 deg C. what is ∆G◦ (kJ/mol) at this temp

-23 / -18 / -3.5 / -1.5 / -41

3. Nitric oxide reacts with chlorine to form NOCL. What is the free energy (kJ) of the reaction at 277 dec C.

2NO(g) + Cl2(g) Ã 2NOCl(g)

+144 / -41.0 / -10.3 / -22.2 / +41.0

4. How much free energy is released or absorbed(kJ) when 95.0 g of ozone is produced.

3 O2(g)à 2 O3(g) ∆G◦ = +326 kJ

+645 / -323 / +95 / +323 / -645

5. Estimate the boiling point (deg C) of phosphoric acid? H3PO4(s)ßà H3PO4(l)

42 / 181 / 315 / -92 / 305

6. Calculate the ∆S◦ (J/K) for the reaction, SiCl4(g)+2Mg(s)à 2MgCl2(s)+Si(s)

+198 / -198 / +255 / -255 / +472

7. Calculate the equilibrium constant, K, for the following reaction at 25 deg C: CH4(g)+2H2O(g)ßà CO2(g) ∆G◦ =-113.6kJ

Which of the following results in a decrease in the entropy of the system

O2(g),300KÃ O2(g), 400K / H2O(s)Ã H3O(l) / N2(g)Ã N2(aq) / NH3(l)Ã NH3(g) / 2H2O2(g)Ã 2H2O(g)+O2(g)

8. Identify the incorrect statemtent?

When ∆G◦ >0, energy can be added to force a non-spontaneous to proceed.

When K>1, ∆G◦ <0.

Enthalpy is a good predictor of free energy.

Entropy of the universe increases in a spontaneous reaction

All of the above

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