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A mixture of methane (CH₄) and butane (C₄H₁₀) at one atmosphere pressure and 25°C has a density of 1.375 g/L. Assuming ideal behavior, what is the mass in grams of carbon that are in 1 liter of the mixture?

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mickymike92

The mass of carbon in 1 liter of mixture = 1.108 g

What is the mass of carbon in 1 liter of the mixture?

The mass of carbon in 1 liter of the mixture is determined as follows:

First the moles of gas is determined using the ideal gas formula:

  • n = PV/RT

n = (1 * 1)/(0.08205L * 298)

n = 0.0409 mole of total gas

mass of gas is then determined using the formula:

  • mass = density * volume

mass = 1 * 1.375

mass = 1.375 g

Let x = mass of CH₄ and y = mass of C₄H₁₀

x + y = 1.375 g

nCH₄ + nC₄H₁₀ = ntotat

moles = mass/molar mass

x + y = 1.695 => y = 1.695 - x

(x/molar mass of CH₄) + [(1.375 - x)/ molar mass C₄H₁₀ = 0.0409

x/16 + (1.375 - x)/58 = 0.0409

x = 0.380 g CH₄

y = 1.375 - 0.380

y = 0.995 g of C₄H₁₀

mass of C in CH₄ = 12/16 * 0.380 = 0.285

mass of C in C₄H₁₀ = 48/58 * 0.995 = 0.823

Mass of carbon in 1 liter of mixture = 0.285 + 0.823

Mass of carbon in 1 liter of mixture = 1.108 g

In conclusion, the carbon is the major component in the mixture.

Learn more about ideal gas at: https://brainly.com/question/20348074

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