Chemistry: Asolution of na2co3 is added dropwise to a solution that contains 1.23×10? 2 m fe2 and 1.46×10? 2 m cd2 . what concentration of co32? is need to initiate precipitation? neglect any volume changes during the addition.

Answer : The partial pressure of the in the tank in psia is, 32.6 psia.Explanation :As we are given 75 % and 25 % in terms of volume.First we have to calculate the moles of and .Now we have to calculate the mole fraction of .Now we have to calculate the partial pressure of the gas.conversion used : (1 Kpa = 0.145 psia)Therefore, the partial pressure of the in the tank in psia is, 32.6 psia....

Asolution of na2co3 is added dropwise to a solution

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sarbjit879

27.04.2020

Chemistry

Answer : The partial pressure of the CO_2 in the tank in psia is, 32.6 psia.

Explanation :

As we are given 75 % CO_2 and 25 % N_2 in terms of volume.

First we have to calculate the moles of CO_2 and N_2 .

$\text{Moles of }CO_2=\frac{\text{Volume of }CO_2}{\text{Volume at STP}}=\frac{75}{22.4}=3.35mole$

$\text{Moles of }N_2=\frac{\text{Volume of }N_2}{\text{Volume at STP}}=\frac{25}{22.4}=1.12mole$

Now we have to calculate the mole fraction of CO_2 .

$\text{Mole fraction of }CO_2=\frac{\text{Moles of }CO_2}{\text{Moles of }CO_2+\text{Moles of }N_2}$

$\text{Mole fraction of }CO_2=\frac{3.35}{3.35+1.12}=0.75$

Now we have to calculate the partial pressure of the CO_2 gas.

$\text{Partial pressure of }CO_2=\text{Mole fraction of }CO_2\times \text{Total pressure of gas}$

$\text{Partial pressure of }CO_2=0.75mole\times 300Kpa=225Kpa=225Kpa\times \frac{0.145\text{ psia}}{1Kpa}=32.625\text{ psia}$

conversion used : (1 Kpa = 0.145 psia)

Therefore, the partial pressure of the CO_2 in the tank in psia is, 32.6 psia.

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Asolution of na2co3 is added dropwise to a solution that contains 1.23×10? 2 m fe2 and 1.46×10? 2 m cd2 . what concentration of co32? is need to initiate precipitation? neglect any volume changes during the addition.

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