A 4.00 g sample of a mixture of BaO and CaO is placed in a 1.00 L vessel containing CO2 at a pressure of 730 torr and a temperature of 298 K. The CO2 reactions with both oxide reagents to form BaCO3 and CaCO3. When the reaction is complete, the pressure of the remaining CO2 is 150 torr. a. Calculate the total number of moles of CO2 that has reacted. b. Calculate the mass percentage of CaO in the initial mixture.

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Asked Nov 13, 2019
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A 4.00 g sample of a mixture of BaO and CaO is placed in a 1.00 L vessel containing CO2 at a pressure of 730 torr and a temperature of 298 K. The CO2 reactions with both oxide reagents to form BaCO3 and CaCO3. When the reaction is complete, the pressure of the remaining CO2 is 150 torr. a. Calculate the total number of moles of CO2 that has reacted. b. Calculate the mass percentage of CaO in the initial mixture.

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Expert Answer

Step 1

First we have to calculate the reacted pressure of CO2 gas in the given reaction:-

The initial pressure of CO2 in the reaction is given as 730 torr.

The remaining pressure of CO2 gas after the reaction is given as 150 torr.

So, the reacted pressure of CO2 gas in the given reaction is 580 torr.

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the reacted pressure of CO2 gas in the given reaction is 730 torr-150 torr 580 torr

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Step 2

Now, we will find the no. of moles of reacted CO2 gas reacted in the given reaction: -

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The pressure of reacted CO,is calculated as - 1 atm 580 torr = 0.7631 atm 580 torr 760 torr

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Step 3

The volume of container is 1.00 L.

The temperature of the reaction is 298 K.

H...

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P x V No. of moles R T 0.7631 atm 1.00L atm mol x 298K 0.0821L 0.7631 24.4658 mol = 0.0311 mol

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