Question

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

Answer 1

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!!!!

Answer 2

73.3 ml of carbon are needed

Step-by-step 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