Given the equation for the decomposition of hydrogen peroxide, 2H_(2)O_(2)... O_(2)+2 H_(2)O, a student sets up a problem to convert from 63.4 grams of hydrogen peroxide to the mass of oxygen produced. Most of the setup is shown below. What is the final conversion factor? 63.4gH_(2)O_(2)times 1molH_(2)O_(2)times 1molO_(2)times 34.02gH_(2)O_(2) 2molH_(2)O_(2) 1molH_(2)O_(2) 1molO_(2) 32.00gO_(2) 1molO_(2) There isn't one - the problem is completely set up. 16.00gO_(2) 1molO_(2)

## Step 1: Analyze the given setup### The problem involves converting 63.4 g of to the mass of . The equation for the decomposition is balanced as . The student has already set up most of the conversion factors, but we need to verify if the final conversion factor is correct.---## Step 2: Identify the correct molar masses and stoichiometric ratios### From the balanced equation:- Molar mass of .- Stoichiometric ratio: .- Molar mass of .The correct sequence of conversions should be: ---## Step 3: Verify the final conversion factor### The final step in the calculation converts moles of to grams of . This requires the molar mass of , which is . Therefore, the correct final conversion factor is: ---