Chemistry homework

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 These are a portion of the questions that are needed to be answered. If you decided to complete this assignment I will screenshot and send the remaining 9 questions.

1. The equilibrium constant KP for the reaction is 203 at a certain temperature. Calculate 

PO2

if 

PNO = 0.411 atm and PNO2 = 0.385 atm.

2NO2(g)⇆ 2NO(g) + O2(g) PO2 = atm 

2.  Enter your answer in the provided box. For the reaction N2(g) + 3H2(g)⇆ 2NH3(g) KP is 0.000817 at 683°C. 

What is Kc for the reaction? Kc = 

3.  A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temperature. The equilibrium concentrations are [N2] = 0.41 M, [H2] = 1.26 M, and [NH3] = 0.40 M. 

Calculate the equilibrium constant, Kc, if the reaction is represented as (1/2)N2(g) + (3/2)H2(g) ⇌ NH3(g)

4. Ammonium carbamate, NH4CO2NH2,decomposes as follows: NH4CO2NH2(s) ⇆ 2NH3(g) + CO2(g) Starting with only the solid, it is found that at 40°C the total gas pressure 

(NH3 and CO2) is 0.263 atm.

Calculate the equilibrium constant KP 

5.  Enter your answer in the provided box.
A 2.180 mole quantity of NOCl was initially placed in a 

1.150 L reaction chamber at 400°C. After equilibrium was established,

it was found that 28.60 percent of the NOCl has dissociated:
2NOCl(g) ⇆ 2NO(g) + Cl2(g)
Calculate the equilibrium constant Kc for the reaction. 

6.  At 1000 K, a sample of pure NO2 gas decomposes:

2NO2(g) ⇌ 2NO(g) + O2(g)

The equilibrium constant, KP, is 158. Analysis shows that the partial pressure of O2 is 0.43 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture. 

    • Posted: 21 days ago
    • Due: 
    • Budget: $15
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