Calculating the Amount of Product Formed

Chapter , Problem 1PE

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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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