Question

hat is the pressure of CO(g) in equilibrium with the CO2(g) and O2(g) in the atmosphere at 25 ????C? The partial pressure of O2(g) is 0.2 bar and the partial pressure of CO2(g) is 3 * 10-4 bar. CO is extremely poisonous because it forms a very strong complex with hemoglobin. Should you worry?

Answer 1

Answer:

The partial pressure of CO is 5.54x10⁻⁴⁹atm. You shouldn't worry because it is very low pressure

Explanation:

First, the balanced reaction is:

CO + 1/2O₂ → CO₂

The energies of formation are:

ΔG(CO)=-137.168kJ/mol

ΔG(O₂)=0

ΔG(CO₂)=-394.359kJ/mol

The energy of the reaction is:

$delta-G_{reaction} =delta-G_{CO_{2} } -(delta-G_{CO} +1/2delta-G_{O_{2} } )\\delta-G_{reaction}=-394.359-(-137.168+0)=-257.191kJ/mol$

The expression for calculate the partial pressure of CO is:

$p_{CO} =\frac{p_{CO2} }{p_{O_{2} }^{1/2}*exp^{-\frac{delta-G}{RT} } } \\p_{CO}=\frac{3x10^{-4} }{0.2^{1/2}*exp(-\frac{-257.191*1000}{8.314*298} ) } \\p_{CO}=5.54x10^{-49} atm$

Answer 2

We have that the partial pressure is mathematically given as

P_{CO}=5.54e-49

And you shouldn't worry because P_{CO}=5.54e-49 is very low pressure .

Partial pressure

Generally the equation for the balanced reaction  is mathematically given as

CO + 1/2O₂ → CO₂

Where

$dG(CO)=-137.168kJ/mol \\\\dG(O_2)=0 \\\\dG(CO_3)=-394.359kJ/mol$

The equation for the energy of the reaction is

$\delta-G_{reaction}=\delta-G_{CO2}-(\delta-G_{CO}+1/2\delta-G_O_2)\\\\\ \delta-G_{reaction}=-394.359-(-137.168)+1/2\delta-G_O_2)\\\\\ \delta-G_{reaction}=-257.191kJ/mol$

Hence Partial pressure is given as

$P_{CO}=\frac{P_{CO2}}{P_{O2}^{1/2}*e(-\frac{\delta-G}{RT})}\\\\P_{CO}=\frac{3*10^{-4}}{0.2^{0.5}*e(-\frac{-257.191*1000}{8.31*298})}$

P_{CO}=5.54e-49

Therefore,You shouldn't worry because P_{CO}=5.54e-49 is very low pressure .

For more information on Pressure visit

https://brainly.com/question/25688500