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4 years ago

A gaseous mixture containing 1.5 mol ar and 3.5 mol co2 has a total pressure of 8.6 atm. What is the partial pressure of co2?

Chemistry

2 answers:

Sindrei [870]4 years ago

8 0

Answer:

The partial pressure of CO2 is 6,02 atm

Explanation:

This is the formula por partial pressure

$\frac{Gas pressure}{Total pressure} \\$ = $\frac{Gas moles}{Total moles} \\$

Total moles ---> 1,5 + 3,5 = 5 moles

Partial pressure CO2 / 8,6 atm = 3,5 moles CO2 / 5 moles (CO2 + Ar)

Partial pressure CO2 = (3,5 moles CO2 / 5 moles) . 8,6 atm = 6,02 atm

Brrunno [24]4 years ago

6 0

Answer:

The answer to your question is: pCO2 = 6.02 atm

Explanation:

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Answer : The volume of $CO_2$ will be, 514.11 ml

Explanation :

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$HCO_3^-+HCl\rightarrow Cl^-+H_2O+CO_2$

First we have to calculate the mass of $HCO_3^-$ in tablet.

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From the balanced chemical reaction, we conclude that

As, 1 mole of $HCO_3^-$ react to give 1 mole of $CO_2$

So, 0.0202 mole of $HCO_3^-$ react to give 0.0202 mole of $CO_2$

The moles of $CO_2$ = 0.0202 mole

Now we have to calculate the volume of $CO_2$ by using ideal gas equation.

$PV=nRT$

where,

P = pressure of gas = 1.00 atm

V = volume of gas = ?

T = temperature of gas = $37^oC=273+37=310K$

n = number of moles of gas = 0.0202 mole

R = gas constant = 0.0821 L.atm/mole.K

Now put all the given values in the ideal gas equation, we get :

$(1.00atm)\times V=0.0202 mole\times (0.0821L.atm/mole.K)\times (310K)$

$V=0.51411L=514.11ml$

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