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pychu [463]
3 years ago
11

For the reaction of oxygen and nitrogen to form nitric oxide, consider the following thermodynamic data (Due to variations in th

ermodynamic values for different sources, be sure to use the given values in calculating your answer.):
ΔH∘rxn 180.5kJ/mol
ΔS∘rxn 24.80J/(mol⋅K)
a. Calculate the temperature in kelvins above which this reaction is spontaneous

b. The thermodynamic values from part A will be useful as you work through part B:

ΔH∘rxn 180.5kJ/mol
ΔS∘rxn 24.80J/(mol⋅K)
Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C :

N2(g)+O2(g)→2NO(g)
Chemistry
1 answer:
CaHeK987 [17]3 years ago
7 0

Answer:

a. 7278 K

b. 4.542 × 10⁻³¹

Explanation:

a.

Let´s consider the following reaction.

N₂(g) + O₂(g) ⇄ 2 NO(g)

The reaction is spontaneous when:

ΔG° < 0  [1]

Let's consider a second relation:

ΔG° = ΔH° - T × ΔS° [2]

Combining [1] and [2],

ΔH° - T × ΔS° < 0

ΔH° < T × ΔS°

T > ΔH°/ΔS°

T > (180.5 × 10³ J/mol)/(24.80 J/mol.K)

T >  7278 K

b.

First, we will calculate ΔG° at 25°C + 273.15 = 298 K

ΔG° = ΔH° - T × ΔS°

ΔG° = 180.5 kJ/mol - 298 K × 24.80 × 10⁻³ kJ/mol.K

ΔG° = 173.1 kJ/mol

We can calculate the equilibrium constant using the following expression.

ΔG° = - R × T × lnK

lnK = - ΔG° / R × T

lnK = - 173.1 × 10³ J/mol / (8.314 J/mol.K) × 298 K

K = 4.542 × 10⁻³¹

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Calculate the volume of water which was liberated during the decomposition of hydrogen peroxide.
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4 0
1 year ago
A vessel of volume 100ml contains 10% of oxygen and 90% of an unknown gas. The gases diffuses in 86 second through a small hole
swat32

The molecular weight of unknown gas : 23.46 g/mol

<h3>Further explanation</h3>

Given

A vessel contains 10% of oxygen and 90% of an unknown gas.

diffuses rate of mixed gas = 86 s

diffuses rate of O₂ = 75 s

Required

the molecular weight of unknown gas (M)

Solution

The molecular weight of mixed gas :(M O₂=32 g/mol)

\tt 0.1\times 32+0.9\times M=3.2+0.9M

Graham's Law :

\tt \dfrac{r_{O_2}}{r_{mixed~gas}}=\sqrt{\dfrac{M_{mixed}}{M_{O_2}} }\\\\\dfrac{75}{86}=\sqrt{\dfrac{3.2+0.9M}{32} }\\\\0.76=\dfrac{3.2+0.9M}{32}\\\\24.32=3.2+0.9M\\\\21.12=0.9M\rightarrow M=23.46~g/mol

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How will you recognize that a single replacement reaction has occured when you combine an active metal with 6m hcl?
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A single replacement or displacement reaction occurs when one ingredient in a compound replaces another. Only another metal can replace a less active one; a metal can only displace another metal, and a non-metal can only displace another non-metal.

<h3>Displacement reaction:</h3>

The tendency of the element to lose electrons is what makes it metallic. Due to their bigger sizes and propensity to lose electrons as size, the number of shells, and nuclear force of attraction rise, the most active metals are found on the left side of the periodic table.

The reaction in which the more reactive element displaces the less reactive element is known as the displacement reaction.

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Three ways to recognize if a single displacement reaction has taken place:

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