Question

When sulfuric acid reacts with sodium bicarbonate, carbon dioxide gas is released. If 2.0 L of CO2 gas is collected at standard temperature and pressure, how many grams of sodium bicarbonate we consumed? (use ideal gas law - R = 0.0821 l*atm/mol*k) H2So4 (aq) + 2NaHCO3 (aq) -> Na2SO4 (aq) + 2H2O (I) + 2CO3 (g)

a) 7.5 g

b) 8.7 g

c) 3.9 g

d) 4.7 g

Answer 1

H2SO4(aq) + 2NaHCO3(aq) Na2SO4(aq) + 2H2O(1) + 2C029)

From the reaction, it is clear that for every 2 moles of sodium bicarbonate consumption, 2 moles of carbon dioxide gas is formed.

Hence the stoichiometric ratio of $NaHCO_3:CO_2=1:1$

1mol or 22.4 L $CO_2$ $\equiv$ 1 mol of

NaHCO3

2 L $CO_2$ $\equiv$$\frac{2*1}{22.4}=0.089\: mol\:NaHCO_3$

Now,

$number\:of\:moles=\frac{given\:mass}{molar\;mass}$

$0.089mol=\frac{given\:mass}{84g/mol}$

$0.089mol*84g/mol=given\:mass$

$given\:mass=7.47g\approx 7.5g$

option a) 7.5g of sodium bicarbonate is consumed