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notka56 [123]
2 years ago
13

Consider the reaction 3CH4(g)→C3H8(g)+2H2(g).

Chemistry
1 answer:
padilas [110]2 years ago
6 0

From the calculations performed, the free energy change for the reaction is 72 kJ/mol.

<h3>What is the equilibrium constant?</h3>

The equilibrium constant is a value that shows the extent to which reactants have been converted to products.

Given that the equation of the reaction is;

3CH4(g)→C3H8(g)+2H2(g)

Then;

PC3H8 = 0.013 atm

PH2 =  2.3×10−2 atm

PCH4 = 41 atm

Now;

ΔG = ΔG° + RTlnQ

ΔG°reaction = ΔG°products - ΔG°reactants

ΔG°reaction = [( -23.4) +2(0)] - 3(-50.8)

ΔG°reaction = 129 kJ/mol

Q = PC3H8 * PH2^2/PCH4^3

Q = 0.013 * (2.3×10−2)^2/( 41)^3

Q = 6.877 * 10^-6/68921

Q= 9.9* 10^-11

Hence;

ΔG = 129 * 10^3  + [8.314 * 298 * (ln  9.9* 10^-11 )]

ΔG = 129 * 10^3 - 57073

ΔG = 72 kJ/mol

Learn more about free energy change: brainly.com/question/14143095

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Hikers were climbing Mount McKinley and pitched camp part way up. While boiling eggs in water for breakfast, they noticed that t
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We know that the boiling temperature of the water depends on the atmospheric pressure.

Here we will find that the atmospheric pressure is 760.62 torr.

To get the atmospheric pressure we need to analyze the given information.

Boiling temperature = 79.0°C

∆Hvap = 40.7 kJ/mol

The equation we need to use is:

ln(p_1/p_2) = \frac{\Delta H}{n*R} (\frac{1}{T_1}  - \frac{1}{T_2} )

Where:

p₁ = 1 atm

p₂ = what we want to know.

n*R = 8.314 J/K*mol

T₁ = (100° + 273.15°) = 374.15°

T₂ = (79.0  + 273.15°) = 352.15°K

We can replace all that in the equation to get:

ln(1 atm/p_2) = \frac{40.7 kJ/mol}{8.314 J/K*mol} (\frac{1}{374.15\°K}  - \frac{1}{352.15\°K} ) = -0.000817\\\\p_2 = (1atm)/exp(-0.000817) = 1.000817 atm

And we want this in torr:

1 atm = 760 torr.

Then 1.000817 atm = 760.62 torr.

This is the pressure at the mountain.

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brainly.com/question/23358029

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