🤓 Based on our data, we think this question is relevant for Professor Sheehan's class at JJAY CUNY.
We are given an equation, CH4 + 2O2 → CO2 + 2H2O, and asked to answer several questions:
Part A. We are asked to determine the limiting reagent, given the number of moles of each reactant (2.55 moles of methane and 4.50 moles of oxygen).
Part B. We are asked to calculate how many grams of products (carbon dioxide and water) are produced from the mixture in Part A.
Part C. We are asked to calculate the actual yield, given the percent yield, 95.0%.
Part D. We are asked to calculate how many grams of the excess (if there is any) will remain unreacted.
Given this equation: CH4 + 2O2 → CO2 + 2H2O
a) If 2.55 moles of methane reacts with 4.50 moles of oxygen, what is the limiting reagent?
b) From this mixture of reactants, how many grams of carbon dioxide and how many grams of water can be produced?
c) If the percent yield for this reaction is 95.0%, what actual yield can you expect?
d) How many grams of the excess reagent (if there is one) will remain unreacted?