Question

1.
Given the
equations:
N_{2}*(g)* + O_{2}*(g)* ®
2NO*(g)*
∆H = +180.7 kJ

2NO*(g)* + O_{2}*(g)* ®
2NO_{2}*(g)*
∆H = -113.1 kJ

2N_{2}O*(g)* ® 2N_{2}*(g)* +
O_{2}*(g)*
∆H = -163.2 kJ

Calculate the change in enthalpy for
the reaction:
N_{2}O*(g)* + NO_{2}*(g)* ®
3NO*(g)*

_______________

2. An electron in a
*carbon atom* makes a transition from n=2 to n=3.

a) Does this transition require energy or emit energy?

_________________

b) Can you calculate the amount of
energy involved using E = -R_{H}/n^{2} ?

Calculate ∆E or explain why this is invalid.

_________________

3. Determine the wavelength of light (nm) emitted when an electron makes a transition from n= 5 to n=2 in a hydrogen atom. Show your work.

_________________

Answer #1

1)

Lets number the reaction as 1, 2, 3, 4 from top to bottom

required reaction should be written in terms of other reaction

This is Hess Law

required reaction can be written as:

reaction 4 = +1 * (reaction 1) -0.5 * (reaction 2) +0.5 * (reaction 3)

So, deltaHo rxn for required reaction will be:

deltaHo rxn = +1 * deltaHo rxn(reaction 1) -0.5 * deltaHo rxn(reaction 2) +0.5 * deltaHo rxn(reaction 3)

= +1 * (180.7) -0.5 * (-113.1) +0.5 * (-163.2)

= 155.65 KJ/mol

Answer: 155.65 KJ/mol

Only 1 question at a time please

Find ΔG∘rxn for the reaction: N2O(g)+NO2(g)→3NO(g) Use the
following reactions with known ΔG values:
2NO(g)+O2(g)→2NO2(g)ΔG∘rxn=−71.2kJ
N2(g)+O2(g)→2NO(g)ΔG∘rxn=+175.2kJ
2N2O(g)→2N2(g)+O2(g)ΔG∘rxn=−207.4kJ

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

Consider the reaction:
4CO(g)+2NO2(g)?4CO2(g)+N2(g).
Using the following information, determine ?H? for the reaction
at 25?C.
NO(g) ?H?f = +91.3 kJ/mol
CO2(g) ?H?f = -393.5 kJ/mol
2NO(g)+O2(g)?2NO2(g) ?H? = -116.2 kJ/mol
2CO(g)+O2(g)?2CO2(g) ?H? = -566.0 kJ/mol
Express your answer using one decimal place.

Consider the reaction: 4CO(g)+2NO2(g)?4CO2(g)+N2(g) Using the
following information, determine ?H? for the reaction at 25?C.
NO(g) ?H?f = +91.3 kJ/mol CO2(g) ?H?f = -393.5 kJ/mol
2NO(g)+O2(g)?2NO2(g) ?H? = -116.2 kJ/mol 2CO(g)+O2(g)?2CO2(g) ?H? =
-566.0 kJ/mol Express your answer using one decimal place.

Calculate the enthalpy change for the following reaction, in kJ
mol-1
N2O4(g) + Cl2(g)
→ 2NOCl(g) + O2(g)
given the following
data: ∆H
(kJ mol-1)
2NOCl(g) → 2NO(g) +
Cl2(g) +75.56
2NO(g) + O2(g) →
2NO2(g) -113.05
2NO2(g) →
N2O4(g
) -58.03

1)calculate the equilibrium constants at 25∘C for each
reaction.
Part A
2NO(g)+O2(g)⇌2NO2(g)
Express your answer using two significant figures.
Part B
N2(g)+O2(g)⇌2NO(g)
Express your answer using two significant figures.
2) Calculate the change in Gibbs free energy for each of the
following sets of ΔHrxn, ΔSrxn, and
T.
Part A
ΔH∘rxn=+ 85 kJ , ΔSrxn=+ 155 J/K , T=
298 K
Express your answer as an integer.
Part B
ΔH∘rxn=+ 85 kJ , ΔSrxn=+ 155 J/K , T=
753 K...

1) Express your answer as a molecular
formula.
a) Use the data below to calculate the heat of hydration of
lithium chloride.
b) Calculate the heat of hydration of sodium chloride.
Compound
Lattice Energy
(kJ/mol)
ΔHsoln(kJ/mol)
LiCl
-834
-37.0
NaCl
-769
+3.88
2)A certain reaction with an activation energy of 115 kJ/mol was
run at 485 K and again at 505 K . What is the ratio of f
at the higher temperature to f at the lower temperature?
Express...

C2N2O2Hg(s) + O2 (g)
-> Hg(g) + 2CO2(g) + N2(g)
Determine the theoretical enthalpy (in kJ/mol) of the mercury
fulminate reaction by using the enthalpy of formation for mercury
fulminate (+ 386 kJ/mol) Remember, ΔH° rxn = Σn x
H°f(products) - Σn x ΔH°f(reactants). Explain
your work. We are assuming a constant pressure situation.
This is can also be termed the heat of
explosion, but when it is termed heat of explosion,
the units are traditionally kJ/kg of substance. Convert...

Given the following reactions and their enthalpies:
ΔH(kJ/mol)−−−−−−−−−−−
H2(g)⟶2H(g) +436
O2(g)⟶2O(g) +495
H2+1/2O2(g)⟶H2O(g) −242
A. Devise a way to calculate ΔH for the reaction
H2O(g)⟶2H(g)+O(g)
B. estimate the H-O bond energy

1)At 25°C, some second-order reaction 3 X
(g)→ 2 Y (g) + Z
(g) has a half-life of 5.82 hours when the
initial concentration of X is 4.46 M.
(a) What is rate constant for this reaction?
(b) How much X will be left after
17.5 hours?
Example of answer: (a)
k = [type
your answer] M–1 h–1;
(b) [X]t =
[type your answer] M.
2)
For some second-order reaction: 3 X
(g)→ Y (g) + Z
(g).
The following...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 5 minutes ago

asked 34 minutes ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 3 hours ago

asked 3 hours ago

asked 4 hours ago