Consider the stoichiometry of the reaction provided in the question(s) below. a. A laboratory student started with 0.0812 grams of Reactant A (benzaldehyde, m.w. 106.12 g/mol). How many millimoles of Reactant A did the student add to the reaction mixture? b. A laboratory student started with 0.162 grams of Reactant B (sodium chromate, m.w. 161.97 g/mol). How many millimoles of reactant B did the students add to the reaction mixture?

Consider the reaction. 2 Рb's) + O,(g) — 2 PЬО(s) An excess of oxygen reacts with 451.4 g of lead, forming 348.1 g of lead(II) oxide. Calculate the percent yield of the reaction. percent yield: % * TOOLS x10

A student weighed 0.550 g of lithium chloride, LiCl, to use in a reaction. How many moles is this? Group of answer choices 42.39 5.11 0.0130 23.31 77.08

a. For the following unbalanced chemical equation, suppose 10.6 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. Enter the formula for the limiting reactant. C3H8 (9) + O2(g) → CO₂ (g) + H₂O(g) Limiting reactant: Mass of CO2: Mass of H₂O = b. For the following unbalanced chemical equation, suppose 10.1 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. Al(s) + Cl₂ (g) → AlCl3 (s) = Limiting reactant: = g Mass of AlCl3 c. For the following unbalanced chemical equation, suppose 10.6 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. NaOH(s) + CO2 (g) → Na2CO3(s) + H₂O(1) Limiting reactant: Mass of Na2CO3 Mass of H₂O = = g

Milk of magnesia (Maalox) contains magnesium hydroxide. Magnesium hydroxide can be reacted with hydrochloric acid to form magnesium chloride and water, as seen in the reaction below. Using this reaction, how many grams of hydrochloric acid are needed to fully react 355g magnesium hydroxide?

If a reaction is run that is supposed to produce 125 g (theoretical yield) of product and the actual yield of product that was produced was 73.5 g, what is the percent of yield of this reaction?   A. 170%   B. 1.70%   C. 73.5%   D. 58.8%

For the following reaction, 9.90 grams of benzene (C,Hg) are allowed to react with 15.2 grams of oxygen gas. benzene (C,H6) (1) + oxygen (g)- →carbon dioxide (g) + water (g) What is the maximum amount of carbon dioxide that can be formed? | grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? | grams

ABS plastic is a polymer consisting of three monomer units: acrylonitrile (C₃H₃N), butadiene (C₄H₆), and styrene (C₈H₈). A sample of ABS plastic contains 13.7% N by mass. It took 1.56 g of Br₂ to react completely with a 2.00 g sample of ABS plastic. Bromine reacts 1:1 (by moles) with the butadiene units in the polymer and nothing else, so bromination is a method for determining the quantity of butadiene in the polymer. What is the percent by mass of styrene in the polymer?

For the following reaction, 33.5 grams of calcium hydroxide are allowed to react with 28.9 grams of hydrochloric acid. calcium hydroxide(aq) + hydrochloric acid(aq)  calcium chloride(aq) + water(ℓ) 1.- What is the maximum mass of calcium chloride that can be formed? ___g 2.- What is the FORMULA for the limiting reagent? 3.-What mass of the excess reagent remains after the reaction is complete? ____g

3. In a neutralization reaction, 50.00 mL of 0.750 M phosphoric acid reacts with 2.500 g of magnesium hydroxide producing magnesium phosphate and water. Write a balanced equation for the reaction. b. What is the limiting reactant? C. How much of the excess reactant remains after the limiting reactant is completely consumed? d. What is the theoretical yield of magnesium phosphate (in grams)? e. If 2.552 g of magnesium phosphate are produced in an experiment, then what is the percent yield? a. lected