Question

# How many liters of carbon dioxide gas, measured at 20 degrees Celsius and 715 torr, are...

How many liters of carbon dioxide gas, measured at 20 degrees Celsius and 715 torr, are formed when 49 grams of chalk (CACO3, 100.9 g/mol) are reacted with 60 ml of 3.20 M sulfuric acid (H2SO4) according to the following molecular equation (R= .0821 Latm/molK).

CACO3 (s) + H2SO4 (aq) -> CO2 + H2O (l) + CASO4 (s)

Number of moles of CaCO3 , n = mass/molar mass

= 49 g / 100.9(g/mol)

= 0.486 moles

Number of moles of H2SO4 , n' = Molarity x volume in L

= 3.20 M x 60 mL x 10 -3 L/mL

= 0.192 moles

CaCO3 (s) + H2SO4 (aq) ----> CO2 + H2O (l) + CaSO4 (s)

1 mole of H2SO4 reacts with 1 mole of CaCO3

0.192 moles of H2SO4 reacts with 0.192 moles of CaCO3

So 0.486 - 0.192 moles of CaCO3 left unreacted so CaCO3 is excess reactant.

All of H2SO4 completly reacted it is limiting reactant.

Again 1 mole of H2SO4 produces 1 mole of CO2

0.192 mole of H2SO4 produces 0.192 mole of CO2

Calculation of volume of CO2 :

We know that ideal gas equation is PV = nRT

Where

T = Temperature = 20 oC = 20+273 = 293 K

P = pressure = 715 torr x ( 1 atm / 760 torr) = 0.941 atm

n = No . of moles = 0.192 moles

R = gas constant = 0.0821 L atm / mol - K

V= Volume of the gas = ?

Plug the values we get V = ( nRT) / P = 4.91 L

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