A 211 g sample of barium carbonate reacts with a solution of nitric acid to give barium nitrate, carbon dioxide, and water. If the acid is present in excess, what mass and volume of carbon dioxide gas at STP will form?

May 18, 2017

We assess the stoichiometric equation...............

Explanation:

$B a C {O}_{3} \left(s\right) + 2 H N {O}_{3} \left(a q\right) \rightarrow B a {\left(N {O}_{3}\right)}_{2} \left(a q\right) + {H}_{2} O \left(l\right) + C {O}_{2} \left(g\right) \uparrow$

Given the stoichiometry, ONE MOLE of carbon dioxide is evolved for each mole of barium carbonate.

$\text{Moles of barium carbonate} = \frac{211 \cdot g}{197.34 \cdot g \cdot m o {l}^{-} 1} = 1.07 \cdot m o l .$

Given the stoichiometry, $1.07 \cdot m o l$ of carbon dioxide gas will be evolved.

With respect to $C {O}_{2}$, this represents a mass of 1.07*molxx44.01*g*mol^-1=??*g.

And a volume of $1.07 \cdot m o l \times 24.5 \cdot L \cdot m o {l}^{-} 1$ given room temperature and pressure...