Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s) + 3Cl2 (g)→2AICI3 (s) You are given 31.0 g of aluminum and 36.0 g of chlorine gas.

A 50.6 grams sample of magnesium hydroxide (Mg(OH)2) is reacted with 45.0 grams of hydrochloric acid (HCl). What is the theoretical yield of magnesium chloride (MgCl2)?

3 CuO(s) + 2 Al(s) → 3 Cu(s) + Al2O3(s) 25.0 g of copper(II) oxide are combined with 25.0 g of Al , and the mixture is heated strongly to react. molar masses (g/mol):  CuO - 79.55    Al - 26.98    Cu - 63.55   If 18.2 g of Cu metal is recovered from the reaction, what is the percent yield of the reaction?  Do not include the percent sign (%) on your submitted answer.

Copper reacts with nitric acid via the following equation: 3 Cu(s) + 8 HNO3(aq) → 3 Cu(NO3)2 (aq) + 2 NO(g) + 4H₂O(l) What mass of NO can be formed when 27.7 g of Cu reacts with 77.9 g HNO3? g NO

Chloroform, CHCl3, reacts with chlorine, Cl2, to form carbon tetrachloride, CCl4, and hydrogen chloride, HCl. In an experiment 25 grams of chloroform and 0.36 mol of chlorine were mixed. Which is the limiting reactant?  The equation is given as                                               CHCl3       +      Cl2         =     CCl4      +     HCl

A sample of unknown hydrate, AC·XH2O, has a mass of 1.000 g before heating and a mass of 0.781 g after heating.   If the molar mass of the anhydrous compound (AC) is 195.5 g/mol, what is the water of crystallization for the formula of the unknown hydrate? In other words, what is the X in the formula:  AC·XH2O?

P4(s) + 6Cl2(g) → 4PCl3(l) Given an initial mass of 19.14 g P4, an excess of Cl2, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of PCl3 produced by the reaction. g

For the following reaction, 26.0 grams of bromine are allowed to react with 16.5 grams of chlorine gas. bromine (g) + chlorine(g) → bromine monochloride(g) What is the maximum mass of bromine monochloride that can be formed? Mass= g What is the FORMULA for the limiting reactant? What mass of the excess reagent remains after the reaction is complete? Mass= g

A sample of brass weighing 1.203 grams was analyzed. Brass is an alloy composed of copper, Cu, and zinc,  Zn. The zinc in the alloy was reacted with 35.123 grams of hydrochloric acid, HCl, in excess, according to the following balanced equation:  Zn(s) + 2 HCl (aq) → H2 (g) + ZnCl2 (aq)  After all of the zinc reacted, the mass of the remaining solution weighed 36.309 grams.   What mass of hydrogen gas was produced?   What mass of zinc reacted?   What was the percentage of zinc (by mass) in the alloy?

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.