Question

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)

Answer #1

Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g)
given the following reactions and enthalpies of formation:
12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ
12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ

From the enthalpies of reaction
2H2(g)+O2(g)→2H2O(g)ΔH=−483.6kJ3O2(g)→2O3(g)ΔH=+284.6kJ calculate
the heat of the reaction 3H2(g)+O3(g)→3H2O(g) Express your answer
using four significant figures. I have no idea how to approach this
problem.

Use the following information to find ΔH°f
of gaseous HCl:
N2(g) + 3H2(g) →
2NH3(g)
ΔH°rxn = - 91.8 kJ
N2(g) + 4H2(g) +
Cl2(g) →
2NH4Cl(s)
ΔH°rxn = - 628.8 kJ
NH3(g) + HCl(g) →
NH4Cl(s)
ΔH°rxn = - 176.2 kJ

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?

NO2(g) + 7⁄2H2(g) ---> 2H2O(ℓ) + NH3(g)
ΔH° = ??? kJ
Using the following two equations:
2NH3(g) ---> N2(g) + 3H2(g)
ΔH° = +92 kJ
1⁄2N2(g) + 2H2O(ℓ) ---> NO2(g) + 2H2(g)
ΔH° = +170 kJ

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

Part A:
The decomposition of NI3 to form N2 and I2 releases −290.0 kJ of
energy. The reaction can be represented as
2NI3(s)→N2(g)+3I2(g), ΔHrxn=−290.0 kJ
Find the change in enthaply when 15.0 g of NI3 decomposes.
Express your answer to three significant figures and include the
appropriate units.
Part B:
4NH3(g)+5O2(g)→4NO(g)+6H2O(g)
Calculate the standard heat of reaction, or ΔH∘rxn, for
this reaction using the given data. Also consider that the standard
enthalpy of the formation of elements in their pure...

I am having difficulty with understanding this particular types
of problems.
1) Calculate ΔHrxn for the following reaction:
C(s)+H2O(g)→CO(g)+H2(g)
Use the following reactions and given ΔH values:
C(s)+O2(g)→CO2(g), ΔH= -393.5 kJ
2CO(g)+O2(g)→2CO2(g), ΔH= -566.0 kJ
2H2(g)+O2(g)→2H2O(g), ΔH= -483.6 kJ
2) Calculate ΔHrxn for the following reaction:
5C(s)+6H2(g)→C5H12(l)
Use the following reactions and given ΔH values.
C5H12(l)+8O2(g)→5CO2(g)+6H2O(g),
ΔH=−3244.8 kJ
C(s)+O2(g)→CO2(g), ΔH=−393.5
kJ
2H2(g)+O2(g)→2H2O(g), ΔH=−483.5
kJ

Given the following chemical equilibria,
N2 (g) + O2 (g) <---> 2NO (g)
K1=0.641
4NH3 (g) + 5O2 (g) <---> 4NO (g) +
6H2O (g) K2=29.48
H2 (g) + 1/2O2 (g) <--->
H2O (g) K3=74.93
Determine the equilibrium constant for the reaction below:
N2 (g) + 3H2 (g) <--->
2NH3 (g) Kc = ???

Using the Information below determine the change in enthalpy for
the following reaction:
2NO (g) + 5H2
(g)!2NH3
(g) + 2H2O
(l)
H2 (g) + 1⁄2O2 (g)!H2O (l) ΔH° = -285.8 kJ
N2 (g) + O2 (g)!2NO (l) ΔH° = +180.5 kJ
2NH3 (g)!N2 (g) + 3H2 (g)ΔH° = +92.22 kJ
a)-197.52 kJ
b)-241.7 kJ
c)-483.3 kJ
d)-659.88 kJ
e)-844.3 kJ
please show me which equation is first second and thrid and
reason why? i may be taking the wrong...

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