between liquid cyclohexane (C6H12) and oxygen gas. Another product of this combination is water as shown in the chemical equation below:   2 C6H12 + 5 O2 = 2 H2C6H8O4 + 2 H2O   If your target percent yield is at least 85% of the 25.0 g theoretical yield, how much of the starting materials (cyclohexane and oxygen gas) should you have? Express both reactants in (a) moles and (b) grams.

Potassium chlorate, KClO 3 , decomposes upon heating in the presence of a catalyst according to the reaction below. 2KClO 3 (s) 2KCl(s)+3O 2 (g) In a certain experiment 40.0gKClO3 is heated until it completely decomposes. The experiment performed and the oxygen gas is collected and its mass is found to be 10.8g . What is the percent yield? Answer in standard notation, rounded to the nearest tenth of a percent

Glucose, C6H1206, can be represented by the molecular model shown below. If 1.00 mol of glucoseis submitted to combustion analysis, how many moles of CO2 and how many moles of H2O wouldbe formed?

Please help fill out the table in the attached picture with the given information.

One method of purifying nitrogen oxide (NO) before it is released from a smoke stack is to react it with ammonia (NH3). The products created from this reaction are nitrogen gas and water. Consider the balanced equation below. Assuming there is excess NO, how many grams of H2O will be produced from 5.538 g of NH3? 4 NH3  +   6 NO   -->   5 N2   +   6 H2O

The first step in the reaction of Alka–Seltzer with stomach acid consists of one mole of sodium bicarbonate (NaHCO3) reacting with one mole of hydrochloric acid (HCl) to produce one mole of carbonic acid (H2CO3), and one mole of sodium chloride (NaCl). Using this chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 33 mol NaHCO3 and 77 mol HCl.HCl. moles of carbonic acid :  ____________________mol   Which of the two reactants limits the number of moles of H2 CO3 that can be made? 1. HCl 2. NaHCO3   How much excess reactant remains after the reaction? excess reactant : ___________________mol

Balance the chemical equation below using the smallest possible whole number stoichiometric coefficie C(s) + H₂(g) → C₂H, (g) - G X Do 3

One method of purifying nitrogen oxide (NO) before it is released from a smoke stack is to react it with ammonia (NH3). The products created from this reaction are nitrogen gas and water.  Consider the balanced equation below. Assuming there is excess NO, how many grams of H2O will be produced from 3.089 g of NH3? 4 NH3  +   6 NO   -->   5 N2   +   6 H2O

Ethanol (C₂H₆O) is combusted in air according to the following reaction: C₂H₆O(l) + O₂(g) → CO₂(g) + H₂O(l) How many grams of water would be produced by the complete combustion of 6.45 moles of ethanol in the presence of excess oxygen?

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g).  Calculate the percent yield if the reaction of one mole of methane produces 40. grams of carbon dioxide in the presence of excess oxygen.