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raketka [301]
3 years ago
11

If 1.332 mol of C4H10 are reacted with 6.504 mol of O2, how many mol of the excess reagent will remain unreacted? 2 C4H10 + 13 O

2 ——> 8 CO2 + 10 H2O MM: 58.1 32.0 44.0 18.0
Chemistry
1 answer:
Luden [163]3 years ago
5 0

Answer: The number of moles of excess reagent remain unreacted will be, 6.004 moles.

Explanation : Given,

Moles of C_4H_{10} = 1.332 mol

Mass of O_2 = 6.504 mol

First we have to calculate the limiting and excess reagent.

The balanced chemical equation is:  

C_4H_{10}+13O_2\rightarrow 10H_2O+8CO_2

From the balanced reaction we conclude that

As, 13 mole of O_2 react with 1 mole of C_4H_{10}

So, 6.504  moles of O_2 react with \frac{6.504}{13}=0.5003 moles of C_4H_{10}

From this we conclude that, C_4H_{10} is an excess reagent because the given moles are greater than the required moles and O_2 is a limiting reagent and it limits the formation of product.

Number of moles remain unreacted = 6.504 mol - 0.5003 mol = 6.004 mol

Therefore, the number of moles of excess reagent remain unreacted will be, 6.004 moles.

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