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Zigmanuir [339]
3 years ago
9

How many moles of potassium hydroxide are needed to completely react with 2.94 moles of aluminum sulfate

Chemistry
1 answer:
ArbitrLikvidat [17]3 years ago
6 0

Answer:- Third choice is correct, 17.6 moles


Solution:- The given balanced equation is:


Al_2(SO_4)_3+6KOH\rightarrow 2Al(OH)_3+3K_2SO_4


We are asked to calculate the moles of potassium hydroxide needed to completely react with 2.94 moles of aluminium sulfate.


From the balanced equation, there is 1:6 mol ratio between aluminium sulfate and potassium hydroxide.


It is a simple mole to mole conversion problem. We solve it using dimensional set up as:


2.94molAl_2(SO_4)_3(\frac{6molKOH}{1molAl_2(SO_4)_3})


= 17.6 mol KOH


So, Third choice is correct, 17.6 moles of potassium hydroxide are required to react with 2.94 moles of aluminium sulfate.



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Step 1: List the known quantities and plan the problem.

Known

given: 75.0 g Sn
molar mass of Sn = 118.69 g/mol
1 mol Sn = 2 mol HF (mole ratio)
Unknown

mol HF
Use the molar mass of Sn to convert the grams of Sn to moles. Then use the mole ratio to convert from mol Sn to mol HF. This will be done in a single two-step calculation.

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Step 2: Solve.

75.0 g Sn×1 mol Sn118.69 g Sn×2 mol HF1 mol Sn=1.26 mol HF
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1
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118.69
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1
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Step 3: Think about your result.

The mass of tin is less than one mole, but the 1:2 ratio means that more than one mole of HF is required for the reaction. The answer has three significant figures because the given mass has three significant figures.
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