"లిం[Tutorial: Limiting reactant determination]This question will walk you through the steps of determining whichreactant is limiting based on a balanced chemical equation.a) Step 1: Evaluate the question. Which of the following correctly describes aimiting reactant?b) Calculate the theoretical yield in moles CO2 from the complete combustion of29.3 grams CH4 according to the following balanced chemical equation: 1CH:(g) + 2 O2(g) → 1 CO:(g) + 2 H:O(1)c) Calculate the theoretical yield in moles CO2 from the complete reaction of81.7 grams O2 according to the following balanced chemical equation:CH:(g) + 2 O2(g)→ CO:(g) + 2 H:O(1)d) Which of the following is the limiting reactant?e) What is the mass in grams of the excess CH. remaining after the partialcombustion in 81.7 grams O2?rchDELL

“Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for you. To get remaining sub-part solved please repost the complete question and mention the sub-parts to be solved.” In a chemical reaction, the limiting agent is the one that completely consumes in the reaction to furnish the products. The overall yield of the reaction is determined by the moles of the limiting agent. The amount of the product formed by the complete consumption of the limiting agent is termed as the theoretical yield. The ratio of the actual yield to the theoretical yield multiplied by 100 is furnished as the percent yield. a) Determine the number of moles of each species of the reactants by dividing the mass and its molar mass. The substance that is present in the lowest mole value is termed as the limiting agent. Calculate the theoretical yield based on the moles of the limiting agent. b) Determine the number of moles of methane (nM) consumed in the reaction when the oxygen is present in an excess quantity. nM=29.3 g16.04 g/mol=1.83 mol One mole of methane yields one mole of carbon dioxide. So, determine the moles of carbon dioxide (nC) formed by the reaction of 1.83 mol of methane. The mass of carbon dioxide (theoretical yield) produced is then calculated by relating the moles and their molar mass. nc=1 mol CO21 mol CH4×1.83 mol CH4=1.83 mol c) Determine the number of moles of oxygen (nO) when the moles of methane is an excess. nO=81.7 g32.00 g/mol=2.55 mol Two moles of oxygen yields one mole of carbon dioxide. So, determine the number of moles of carbon dioxide (nC) formed by relating the stoichiometric equation. nC=1 mol CO22 mol O2×2.55 mol O2=1.23 molHence the theoretical yield of carbon dioxide produces in options b and c are 1.83 mol and 1.23 mol respectively.

Science

Chemistry

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 CO. from the complete combustion of 29.3 grams CH: according to the following balanced chemical equation: 1 CH:(g) + 2 O2(g)→ 1 CO:(g) + 2 H:O(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 O2(g) → CO:(g) + 2 H:O(I)

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 CO. from the complete combustion of 29.3 grams CH: according to the following balanced chemical equation: 1 CH:(g) + 2 O2(g)→ 1 CO:(g) + 2 H:O(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 O2(g) → CO:(g) + 2 H:O(I)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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