Calculating the Amount of Product Formed
Chapter , Problem 1PE(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?
Molten gallium reacts with arsenic to form the semiconductor, gallium arsenide, GaAs, used in light-emitting diodes and solar cells:
\(\mathrm{Ga}(l)+\mathrm{As}(s) \longrightarrow \mathrm{GaAs}(s)\)
If of gallium is reacted with of arsenic, how many grams of the excess reactant are left at the end of the reaction?
(a) 4.94 g As, (b) 0.56 g As, (c) 8.94 g Ga, or (d) 1.50 g As.
Equation Transcription:
Text Transcription:
2 H_{2}(g)+O_{2}(g){rightarrow}2 H_{2}O(g)
H_{2}(g)
O_{2}(g)
GaAs
Ga(l)+As(s)GaAs(s)
As
As
Ga
As
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