underline ( )H_(2)O_(2)arrow underline ( )H_(2)O+underline ( )O_(2) c. If you are given 25 g of H_(2)O_(2) how much Oxygen could theoretically be produced? d. If there were actually 9.41 g of Cl_(2) produced, what was the percent yield?

Question

Answer 1

c. The theoretical yield of

is approximately 22.15 g.d. The percent yield is approximately 42.35%.

Answer 2

## Step 1: The balanced chemical equation for the decomposition of hydrogen peroxide is given as:###

## Step 2:To find out how much oxygen could theoretically be produced from 25 g of

, we first need to calculate the molar mass of

. The molar mass of

is approximately 34.0147 g/mol.## Step 3:Next, we convert the given mass of

to moles using the formula:###

where

is the number of moles,

is the mass, and

is the molar mass.## Step 4:From the balanced chemical equation, we see that 2 moles of

produce 1 mole of

. Therefore, we can calculate the number of moles of

produced by multiplying the number of moles of

by 1/2.## Step 5:Finally, we convert the moles of

to grams using the molar mass of

, which is approximately 31.998 g/mol.## Step 6:To calculate the percent yield, we use the formula:###

where the actual yield is the given amount of

produced, and the theoretical yield is the amount of

that could theoretically be produced from the given amount of

.

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