A student generates carbon dioxide by reacting sodium carbonate with excess hydr

Question

A student generates carbon dioxide by reacting sodium carbonate with excess hydrochloric acid producing 0.00560 moles of CO_2. Calculate the volume (in L) this amount of carbon dioxide would occupy if this experiment were performed at STP. L of CO_2: Calculate the molar volume (V_m) of CO_2 at STP using the moles of CO_2 that were generated in the above mentioned experiment. V_m of CO_2 at STP: Based on your answer to question 7C, does CO_2 behave as an ideal gas at SIP? Explain in no more than two sentences.

Explanation / Answer

B) Using ideal gas equation,

PV = nRT

where P = Pressure,

V= volume

n = number ofmoles

R = gas constant

T = Temperature.

At STP T = 273 K & P = 1 atm

Putting values in above equation.

1atm x V = 0.00560 moles x 0.0821atm lit /mol x 273 k

V = ( 0.00560 moles x 0.0821 x 273 k ) / 1 atm

= 0.125 L

C ) Molar Volume = Volume / moles

= 0.125 L / 0.00560 moles

= 22.32 L/mole

D) From above, it is concluded that CO2 behaves as IDEAL gas, becouse at STP the molar volume of ideal gas is 22.4 L. and CO2 also possess same volume. Therfore CO2 behaves as ideal gas.

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