Linolenic acid (C18H30O2 - M. W. = 278.42 g/mol) reacts with hydrogen gas according to the equation: C18H30O2 + 3H2 (g) → C18H36O2 What volume of hydrogen gas, as measured at P = 1.00 atm and T = 273.15 K, is required to react with 10.5 g of linolenic acid in this reaction?

2.53 L is the volume of H₂ needed

Explanation:

The reaction is: C₁₈H₃₀O₂ + 3H₂ → C₁₈H₃₆O₂

By the way we can say, that 1 mol of linolenic acid reacts with 3 moles of oxygen in order to produce, 1 mol of stearic acid.

By stoichiometry, ratio is 1:3

Let's convert the mass of the linolenic acid to moles:

10.5 g. 1 mol / 278.42 g = 0.0377 moles

We apply a rule of three:

1 mol of linolenic acid needs 3 moles of H₂ to react

Then, 0.0377 moles will react with (0.0377. 3) / 1 = 0.113 moles of hydrogen

We apply the Ideal Gases Law to find out the volume (condition of measure are STP) → P. V = n. R. T → V = (n. R. T) / P

V = (0.113 mol. 0.082 L. atm/mol. K. 273.15K) 1 atm = 2.53 L