Question

Given the following chemical equilibria,

N_{2} (g) + O_{2} (g) <---> 2NO (g)
K_{1}=0.641

4NH_{3} (g) + 5O_{2} (g) <---> 4NO (g) +
6H_{2}O (g) K_{2}=29.48

H_{2} (g) + 1/2O_{2} (g) <--->
H_{2}O (g) K_{3}=74.93

Determine the equilibrium constant for the reaction below:

N_{2} (g) + 3H_{2} (g) <--->
2NH_{3} (g) K_{c = ???}

Answer #1

1) N2(g) + 3H2(g) 2NH3(g)
2) 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)
3) 2NO(g) + O2(g) 2NO2(g)
What mass of hydrogen gas is needed to produce 147.0 kg of
nitrogen dioxide?

Use the information in the table below to determine
DGofor the reaction
2NH3(g) + 2O2(g) --> N2O(g)
+ 3H2O(l)
DGo (kJ)
N2(g) + 3H2(g) -->
2NH3(g)
-33.0
4NH3(g) + 5O2(g) --> 4NO(g) +
6H2O(l)
-1010.0
N2(g) + O2(g) --> 2NO(g)
174.9
N2(g) + 2O2(g) -->
2NO2(g)
102.6
2N2(g) + O2(g) -->
2N2O(g)
204.2

Q1Calculate the delta H for N2 (g) + O2 (g)------>2NO(g)
4NH3(g) +5O2(g)--->4NO(g)+6H2O(l). DeltaH= -1170kJ
4NH3(g) +
3O2(g)--->2N2(g)+6H2O(l) Delta H =-1530kJ
Q2Calculate standard heat of
formation delta H degree f. For NCl 3
NH3(g)+3HCl
(g)--->NCl3(g)+3H2(g). Delta H =564.8kJ

Consider these reactions and their corresponding K's.
1/2N2+ O2 yields NO2
K1
2NO2 yields 2NO + O2 K2
NOBr yields NO + 1/2Br2 K3
Express the K value for the reaction below in terms
of K1, K2 and K3
1/2N2+ 1/2O2 + 1/2Br2 yields
NOBr K=?

Using the information below determine the change in enthalpy for
the following reaction:
2NO(g) + 5 H2(g) → 2NH3(g) +
2H2O(l)
H2(g) + ½ O2(g) →
H2O(l)
∆H°= -285.8kJ
N2(g) + O2(g) →
2NO(g)
∆H°= +180.5 kJ
2NH3(g) → N2(g) +
3H2(g)
∆H°= + 92.22 kJ
please explain step by step! thanks!

Determine the value of the equilibrium constant, Kgoal, for the
reaction N2(g)+H2O(g)⇌NO(g)+12N2H4(g), Kgoal=? by making use of the
following information:
1. N2(g)+O2(g)⇌2NO(g), K1 = 4.10×10−31
2. N2(g)+2H2(g)⇌N2H4(g), K2 = 7.40×10−26
3. 2H2O(g)⇌2H2(g)+O2(g), K3 = 1.06×10−10

6a/ A sample of gas contains 0.1500 mol of
N2(g) and 0.3000 mol
of O2(g) and occupies a volume of
18.9 L. The following reaction takes place:
N2(g) +
2O2(g)
2NO2(g)
Calculate the volume of the sample after the reaction takes place,
assuming that the temperature and the pressure remain constant
(.......) L
6b/ A sample of gas contains 0.1200 mol of
NH3(g) and 0.1500 mol
of O2(g) and occupies a volume of
12.5 L. The following reaction takes place:...

Given the following data:
2NH3(g) --> N2(g) + 3 H2(g) deltaH* = 92KJ
2H2(g) + O2(g) --> 2H20(g) deltaH* = -484KJ
Calculate deltaH for the reaction:
2N2(g) + 6H2O(g) --> 3O2(g) + 4NH3(g)

At 2000 ?C the equilibrium constant for the reaction
2NO(g)???N2(g)+O2(g)
is Kc=2.4

Applying Hess’s Law, from the enthalpies of reactions,
N2(g) + 3H2(g) → 2 NH3(g) ΔH = − 91.8 kJ
O2(g) + 2H2(g) → 2H2O (g) ΔH = − 483.7 kJ
N2(g) + O2(g) → 2NO(g) ΔH = 180.6 kJ
Calculate the enthalpy change (ΔHrxn) for the reaction: 4NH3(g)
+ 5O2(g) → 4 NO (g) + 6H2O(g)

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