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hichkok12 [17]
3 years ago
10

If 13.8 moles of carbon (c), with a density of 2.26 g/ml, are needed for a chemical reaction, how many milliliters of carbon are

needed? 73.3 ml c 16.5 ml c 6.11 ml c 2.60 ml c
Chemistry
2 answers:
charle [14.2K]3 years ago
8 0

13.8 moles of carbon = 12 g/mol*13.8 or 165.6 grams

165.6 grams/ 2.26 g/mL = 73.27434 or 73.3 mL


I hope this helps!!!!


Aleks [24]3 years ago
5 0

Answer:

73.3 ml of carbon are needed

Explanation:

To determine the volume of carbon needed, the formula for density can be used. The formula for density is

Density = mass ÷ volume

Although the density (2.26 g/ml) was provided in the question, but the mass was not provided.

The mass can be derived from the formula for number of moles shown below.

number of moles = mass ÷ molar mass

number of moles of carbon (provided in the question) is 13.8 moles and the molar mass of carbon is 12 g/mol hence

13.8 = mass ÷ 12

mass = 13.8 × 12

mass = 165.6g

If the mass of the carbon needed for the reaction is 165.6g and the density is 2.26 g/ml, the volume needed will be

Density = mass ÷ volume

2.26 = 165.6 ÷ volume

volume = 165.6 ÷ 2.26

volume = 73.3 ml

73.3 ml of carbon are needed

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