What mass of C₄H₁₀ needs to be burned to produce 12 g of H₂O?

Question

Quizplus · Accepted Answer

First, we need to balance the chemical equation: C₄H₁₀ + 3O2 → CO2 + 4SO2 + 2H2O Next, we need to determine the limiting reactant. Let x be the mass of C₄H₁₀. Using stoichiometry, we can determine the amount of H₂O produced: x g C₄H₁₀ x (1 mol C₄H₁₀ / 192.665 g C₄H₁₀) x (1 mol H₂O / 1 mol C₄H₁₀) x (90.06 g H₂O / 1 mol H₂O) = 0.468x g H₂O We want this to equal 12 g H₂O, so: 0.468x = 12 x = 25.64 g C₄H₁₀ Therefore, the mass of C₄H₁₀ that needs to be burned is 25.64 g. To determine the answer choice closest to 25.64 g, we can divide each answer choice by 25.64 and choose the one closest to 1: A) 3.9 g / 25.64 g = 0.152 B) 15 g / 25.64 g = 0.586 C) 7.7 g / 25.64 g = 0.301 (closest to 1) D) 9.2 g / 25.64 g = 0.359 Therefore, the best choice is C.

What Mass of C4H10 Needs to Be Burned to Produce

What Mass of C₄H₁₀ Needs to Be Burned to Produce