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Snowcat [4.5K]
3 years ago
9

N2(g) + 3h2(g) ⇌ 2nh3(g) the equilibrium constant kc at 375°c is 1.2. starting with [h2]0 = 0.76 m, [n2]0 = 0.60 m and [nh3]0 =

0.48 m, which concentration(s), if any, will have increased when the mixture comes to equilibrium?
Chemistry
1 answer:
nekit [7.7K]3 years ago
8 0
N2(g)   +  3  H2(g) =  2NH3(g)

Qc =  (NH3^2)   / { (N2)(H)^3)}

Qc=  0.48^2  /{ ( 0.60) (0.760^3) }=  0.875

Qc < Kc  therefore  the  equilibrium  will   shift     to  the  right.  This  implies  that  Nh3  concentration  will    increase    
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When a chemist collects hydrogen gas over water, she ends up with a mixture of hydrogen and water vapor in her collecting bottle
elixir [45]

<u>Answer:</u> The partial pressure of hydrogen is 93.9 kPa.

<u>Explanation:</u>

To calculate the partial pressure of hydrogen, we will follow Dalton's Law.

This law states that the total pressure of a mixture of gases is equal to the sum of the individual pressures exerted by the constituent gases.

Mathematically,

p_{total}=p_A+p_B

According to the question,

p_{total}=p_{H_2O}+p_{H_2}

We are given:

p_{total}=97.1 kPa

p_{H_2O}=3.2kPa

p_{H_2}= ?kPa

Putting values in above equation, we get:

97.1kPa=3.2kPa+p_{H_2}

p_{H_2}= 93.9kPa

Hence, the partial pressure of hydrogen is 93.9 kPa.

5 0
3 years ago
Read 2 more answers
1. How many molecules are in 2.40 moles of H2O?
anzhelika [568]

Answer:

There arr 1.5*1024 molecules in 2.40 moles of H2O.

4 0
3 years ago
Frequency of 6.98 x 1013
MAVERICK [17]

Answer:7,070.74

Explanation:because frequency has a lot of energy

6 0
3 years ago
Calculate the energy required to ionize a ground state hydrogen atom. report your answer in kilojoules.
hjlf

First we find for the wavelength of the photon released due to change in energy level. We use the Rydberg equation:

1/ʎ = R [1/n1^2 – 1/n2^2]

where,

ʎ is the wavelength

R is the rydbergs constant = 1.097×10^7 m^-1

n1 is the 1st energy level = 1

n2 is the higher energy level = infinity, so 1/n2 = 0

 

Calculating for ʎ:

1/ʎ = 1.097×10^7 m^-1 * [1/1^2 – 0]

ʎ = 9.1158 x 10^-8 m

 

Then calculate the energy using Plancks equation:

E = hc/ʎ

where,

h is plancks constant = 6.626×10^−34 J s

c is speed of light = 3x10^8 m/s

 

E = (6.626×10^−34 J s * 3x10^8 m/s) / 9.1158 x 10^-8 m

E = 2.18 x 10^-18 J = 2.18 x 10^-21 kJ

 

This is still per atom, so multiply by Avogadros number = 6.022 x 10^23 atoms / mol:

E = (2.18 x 10^-21 kJ / atom) * (6.022 x 10^23 atoms / mol)

E = 1312 kJ/mol

3 0
3 years ago
Please help. I need someone smart
Sveta_85 [38]
5678+910=13000
257-466=198
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3 years ago
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