What is the percent yield of O2 if 10.2 g of O2 is produced from the decomposition of 17.0 g of H2O?

Chemistry

2 answers:

yawa3891 [41]2 years ago

5 0

The balanced chemical reaction will be:

2H2O = 2H2 + O2

We are given the amount of water used in the decomposition reaction. This will be our starting point.

17.0 g H2O (1 mol H2O/ 18.02 g H2O) (1 mol O2/2 mol H2O) ( 32.00 g O2/1mol O2) = 15.09 g O2

Percent yield = actual yield / theoretical yield x 100

Percent yield =10.2 g / 15.09 g x 100

Percent yield = 67.58%

sineoko [7]2 years ago

3 0

Answer: D

Explanation: 67.6

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4 0

2 years ago

Consider this mechanism:

DerKrebs [107]

Answer:

$ClO^- + I^-\rightarrow IO^- + Cl^-$

Explanation:

Given a reaction mechanism, we will typically have catalysts and intermediates which will not be observed in the final balanced overall reaction. In order to obtain a net reaction, we need to add all the separate steps of the given reaction.

First of all, the reactants are combined followed by a combination of products. The repeating species on both sides of the final equation are then canceled out. Let's sum everything we have in our steps:

$ClO^- + H_2O + I^- + HClO + OH^- + HIO\rightarrow HClO + OH^- + HIO + Cl^- + H_2O + IO^-$