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abruzzese [7]
2 years ago
10

Determine the number of grams of C4H10 that are required to completely react to produce 8.70 mol of CO2 according to the followi

ng combustion reaction: 2C4H10 13O2 --> 8CO2 10H2O
Chemistry
1 answer:
Nitella [24]2 years ago
5 0

Answer:

126.4 g of C_{4}H_{10} are required

Explanation:

Balanced reaction: 2C_{4}H_{10}+13O_{2}\rightarrow 8CO_{2}+10H_{2}O

According to balanced reaction-

8 moles of CO_{2} are produced from 2 moles of C_{4}H_{10}

So, 8.70 moles of CO_{2} are produced from (\frac{2}{8}\times 8.70) moles of C_{4}H_{10} or 2.175 moles of C_{4}H_{10}

Molar mass of C_{4}H_{10} = 58.12 g/mol

So, mass of C_{4}H_{10} required = (2.175\times 58.12)g = 126.4 g

Hence 126.4 g of C_{4}H_{10} are required

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In order to convert moles <em>of any given substance</em> into a number of molecules, we need to use <em>Avogadro's number</em>, which states the number of molecules -or atoms, in the case of elements- present in one mol:

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