# Problem: The oxides of Group 2A metals (symbolized by M here) react with carbon dioxide according to the following reaction:MO(s) + CO2(g) → MCO3(s)A 2.85-g sample containing only MgO and CuO is placed in a 3.00-L container. The container is filled with CO2 to a pressure of 740. torr at 20.°C. After the reaction has gone to completion, the pressure inside the flask is 390. torr at 20.°C. What is the mass percent of MgO in the mixture? Assume that only the MgO reacts with CO2.

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###### FREE Expert Solution
• We can get the mass of MgO by calculating the moles of COreacted using the conditions provided which can be plugged in to the ideal gas equation
• The mass of MgO will be divided by 2.85 g sample to get the mass % MgO
• The reaction of Mg with COwill appear as

MgO(s) + CO2(g) → MgCO3(s)

• Calculating for the moles COreacted, it will appear as:

Moles COreacted = moles COinitially - moles CO2  excess

• Calculating for the moles of COinitally and excess using ideal gas equation (assuming COis the only gas in the vessel): ###### Problem Details

The oxides of Group 2A metals (symbolized by M here) react with carbon dioxide according to the following reaction:

MO(s) + CO2(g) → MCO3(s)

A 2.85-g sample containing only MgO and CuO is placed in a 3.00-L container. The container is filled with CO2 to a pressure of 740. torr at 20.°C. After the reaction has gone to completion, the pressure inside the flask is 390. torr at 20.°C. What is the mass percent of MgO in the mixture? Assume that only the MgO reacts with CO2.