In the reaction, A + B→C + D, if element B is in excess, then: O both A & B are limiting reactants. O A is the limiting reactant. O Cis the limiting reactant. O B is the limiting reactant.

There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: 2 Cu₂ S(s) + 3 0₂(g) →2 Cu₂O(s) +2 SO₂ (g) In the second step, copper(I)oxide and carbon react to form copper and carbon monoxide: Cu₂O(s) + C(s)→2 Cu(s)+CO(g) Write the net chemical equation for the production of copper from copper(I) sulfide, oxygen and carbon. Be sure your equation is balanced. ローロ 06

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

[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.

Balance the following chemical equation (using the number "1" if the blank normally is left unfilled). Na (s) + NaF (s) F₂ (g) ---->

Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P,(s) + 50,(g) 2 P,0; (g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid (H,PO,): P,0;(g) + 3H,0(1) 2 H;PO, (1) Suppose the yield of the first step is 77.% and the yield of the second step is 67.%. Calculate the mass of phosphorus required to make 6.0 kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

When exposed to air, aluminum metal, AlAl, reacts with oxygen, O2O2, to produce a protective coating of aluminum oxide, Al2O3Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3 a) What is the theoretical yield of aluminum oxide if 3.00 molmol of aluminum metal is exposed to 2.55 molmol of oxygen? Express your answer with the appropriate units.

For the reaction between solid tetraphosphorus trisulfide andoxygen gas to form solid tetraphosphorus decaoxide and sulfurdioxide gas, write a balanced equation. Show the equation  in terms of (a) molecules, (b) moles, and (c) grams

Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) Calculate the number of grams of NO produced as a byproduct of the reaction of 118.17 grams of Ag with excess HNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol

According to the following reaction, how many grams of nitrogen monoxide will be formed upon the complete reaction of 24.6 grams of oxygen gas with excess nitrogen gas? N₂ (g) + O₂ (g) →→→2NO (g) grams nitrogen monoxide