A 0.2 mol sample of N2 , CO2 with a pressure of 840 torr is exposed to solid CaO which react with theCO2 to form solidCaCO3 assume the reaction goes to completion complete pressure the gas had dropped to 320 how many moles of CO2 in origin mixtur? how

The total pressure in a gas is the product of the partial pressures of its constituents, which are proportionate to their respective molar fractions at constant volume and temperature.

Thus,

To find the number of moles of CO2 in the original mixture, we first need to calculate the number of moles of CO2 consumed in the reaction with CaO.

From the given reaction, 1 mole of CaO reacts with 1 mole of CO2 to form 1 mole of CaCO3.

Since the pressure dropped from 840 torr to 320 torr, the decrease in pressure is due to the consumption of CO2.

The decrease in pressure is (840 torr - 320 torr) = 520 torr.

Using the ideal gas law equation (PV = nRT), we can calculate the moles of CO2 consumed:

( n = \frac{{\Delta PV}}{{RT}} )

( n = \frac{{520 , \text{torr} \times 0.2 , \text{L}}}{{0.0821 , \text{L} \cdot \text{atm/mol} \cdot \text{K} \times 298 , \text{K}}} )

( n = 0.0127 , \text{moles} )

Since 1 mole of CaO reacts with 1 mole of CO2, the original mixture must have contained 0.0127 moles of CO2.