[Tutorial: Limiting reactant determination] This question will walk you through the steps of determining which reactant is limiting based on a balanced chemical equation. a) Step 1: Evaluate the question. Which of the following correctly describes a limiting reactant? b) Calculate the theoretical yield in moles CO₂ from the complete combustion of 29.3 grams CH. according to the following balanced chemical equation: 1 CH.(g) + 2 Oz(g) — 1 COz(g) + 2 HO(I) c) Calculate the theoretical yield in moles CO₂ from the complete reaction of 81.7 grams O₂ according to the following balanced chemical equation: CH.(g) + 2 Oz(g) — COz(g) + 2 H2O(I) d) Which of the following is the limiting reactant? e) What is the mass in grams of the excess CH. remaining after the partial combustion in 81.7 grams O₂?
[Tutorial: Limiting reactant determination] This question will walk you through the steps of determining which reactant is limiting based on a balanced chemical equation. a) Step 1: Evaluate the question. Which of the following correctly describes a limiting reactant? b) Calculate the theoretical yield in moles CO₂ from the complete combustion of 29.3 grams CH. according to the following balanced chemical equation: 1 CH.(g) + 2 Oz(g) — 1 COz(g) + 2 HO(I) c) Calculate the theoretical yield in moles CO₂ from the complete reaction of 81.7 grams O₂ according to the following balanced chemical equation: CH.(g) + 2 Oz(g) — COz(g) + 2 H2O(I) d) Which of the following is the limiting reactant? e) What is the mass in grams of the excess CH. remaining after the partial combustion in 81.7 grams O₂?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter3: Chemical Reactions
Section3.2: Balancing Chemical Equations
Problem 3.1CYU: (a) Butane gas, C4H10, can burn completely in air [use O2(g) as the other reactant] to give carbon...
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The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
please answer only part e
![[Tutorial: Limiting reactant determination]
This question will walk you through the steps of determining which
reactant is limiting based on a balanced chemical equation.
a) Step 1: Evaluate the question. Which of the following correctly describes a
limiting reactant?
b) Calculate the theoretical yield in moles CO₂ from the complete combustion of
29.3 grams CH4 according to the following balanced chemical equation: 1
CH4(g) + 2 O₂(g) → 1 CO₂(g) + 2 H₂O(1)
c) Calculate the theoretical yield in moles CO₂ from the complete reaction of
81.7 grams O₂ according to the following balanced chemical equation:
CH4(g) + 2 O2(g) → CO₂(g) + 2 H₂O(1)
d) Which of the following is the limiting reactant?
e) What is the mass in grams of the excess CH. remaining after the partial
combustion in 81.7 grams O₂?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2c653cb9-ab7a-49e3-bea3-1c34e4b2ce5f%2F90511e78-afd0-46bc-ab63-ce1eb0f6f65b%2Fewztiis_processed.png&w=3840&q=75)
Transcribed Image Text:[Tutorial: Limiting reactant determination]
This question will walk you through the steps of determining which
reactant is limiting based on a balanced chemical equation.
a) Step 1: Evaluate the question. Which of the following correctly describes a
limiting reactant?
b) Calculate the theoretical yield in moles CO₂ from the complete combustion of
29.3 grams CH4 according to the following balanced chemical equation: 1
CH4(g) + 2 O₂(g) → 1 CO₂(g) + 2 H₂O(1)
c) Calculate the theoretical yield in moles CO₂ from the complete reaction of
81.7 grams O₂ according to the following balanced chemical equation:
CH4(g) + 2 O2(g) → CO₂(g) + 2 H₂O(1)
d) Which of the following is the limiting reactant?
e) What is the mass in grams of the excess CH. remaining after the partial
combustion in 81.7 grams O₂?
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