How many moles of hypochlorous acid are needed to react with 0.257 mol of 9-fluorenol?
Molecular weight of hypochlorous acid = 52.46 g/mol
MW of 9-fluorenol = 182.22 g/mol
Write and balance the equation, then follow the steps in this worked example of a stoichiometry problem.
http://www.jiskha.com/science/chemistry/stoichiometry.html
The answer is much less difficult to find. The answer for your problem is 0.257 mol because there is a 1:1 ratio of hypochlorous acid to 9-fluorenol.
To determine the number of moles of hypochlorous acid needed to react with 0.257 mol of 9-fluorenol, we need to use the stoichiometry of the reaction.
First, we need to know the balanced chemical equation for the reaction between hypochlorous acid (HOCl) and 9-fluorenol. Without that information, we cannot determine the stoichiometric ratio.
Once we have the balanced chemical equation, we can determine the stoichiometric ratio between hypochlorous acid and 9-fluorenol. By comparing the coefficients in the balanced equation, we can determine how many moles of hypochlorous acid react with one mole of 9-fluorenol.
Let's assume the balanced equation for the reaction is:
x HOCl + y 9-fluorenol → z products.
Now we can set up a ratio:
(x mol HOCl) / (y mol 9-fluorenol) = (0.257 mol 9-fluorenol) / (1 mol HOCl)
Simplifying the equation, we have:
x mol HOCl = (y mol 9-fluorenol) * (0.257 mol 9-fluorenol) / (1 mol HOCl)
Now we need to know the stoichiometric coefficients (x and y) from the balanced chemical equation to complete the calculation. Let's assume the balanced equation is:
2 HOCl + 1 9-fluorenol → 2 products.
From this equation, we can see the stoichiometric ratio is 2:1 between HOCl and 9-fluorenol. Therefore, x = 2 and y = 1.
Plugging these values into the equation, we have:
x mol HOCl = (1 mol 9-fluorenol) * (0.257 mol 9-fluorenol) / (1 mol HOCl)
x mol HOCl = 0.257 mol 9-fluorenol
Therefore, you would need 0.257 moles of hypochlorous acid to react with 0.257 moles of 9-fluorenol.