Calculating the Amount of Product Formed

Chapter , Problem 2PE

(choose chapter or problem)

Calculating the Amount of Product Formed from a Limiting Reactant

The reaction

                                 \(2\ \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2\ \mathrm{H}_{2} \mathrm{O}(g)\)

is used to produce electricity in a hydrogen fuel cell. Suppose a fuel cell contains 150 g of \(\mathrm {H_2}(g)\) and 1500 g of \(\mathrm {O_2}(g)\) (each measured to two significant figures). How many grams of water can form?

When a 2.00-g strip of zinc metal is placed in an aqueous solution containing 2.50 g of silver nitrate, the reaction is

     \(\mathrm{Zn}(s)+2\ \mathrm{AgNO}_{3}(a q) \longrightarrow 2\ \mathrm{Ag}(s)+\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

(a) Which reactant is limiting? (b) How many grams of Ag form?
(c) How many grams of \(\mathrm {Zn(NO_3)_2}\) form? (d) How many grams of the excess reactant are left at the end of the reaction?

Equation Transcription:

Text Transcription:

2 H_{2}(g)+O_{2}(g){rightarrow}2 H_{2}O(g)

H_{2}(g)

O_{2}(g)

Zn(s)+2 AgNO_{3}(aq){rightarrow}2 Ag(s)+Zn(NO_{3})_{2}(aq)

Ag

Zn(NO_{3})_2