Question

17. The reaction hydrochloric acid with sodium hydrogen carbonate produces carbon dioxide gas as one product.

a) Write the equation for the reaction of these chemicals as aqueous solutions. 500. mL of equimolar concentration of each solution are combined in this reaction.

b) If 2.461 daL of carbon dioxide gas are produced at 32.81 ̊C and 762.7 torr, constituting an 89.62% yield, what molarity of sodium hydrogen carbonate solution was originally reacted, presuming additive volumes?

Answer 1

Q17.

the equation (ablanced)

HCl + NaHCO3 = NaCl + CO2 + H2O

a)

add phases

HCl(aq) + NaHCO3(aq) = NaCl(aq) + CO2(g) + H2O(l)

b)

note: assume daL stands for "liters"

then

V = 2.461 L of CO2

T = 32.81°C = 32.81+273 K = 305.8 K

P = 762.7 torr = 762.7/760 = 1.003 atm

Apply Ideal Gas Law,

PV = nRT

where

P = absolute pressure

V = total volume of gas

n = moles of gas

T = absolute Tmperature

R = ideal gas constant

n = PV/(RT) = (1.003)(2.461)/(0.082*305.8 ) = 0.09843 moles

then.

% yield = Reacted / theoretical * 100%

data is given as:

89.62% = 0.09843 mol / theoretical * 100%

Theoretical = 0.09843 / (89.62/100) = 0.10983 mol should be added

mol of NaHCO3 = 0.10983 mol

M = mol/V

V = 500 mL = 0.5 L

M = 0.10983/(.5) = 0.21966 mol of NaHCO3 / L