Ammonia gas can be prepared by the reaction of a metal oxide such as calcium oxide with ammonium chloride. CaO(s) + 2 NH, CI(s) → 2 NH3(g) +H2O(g) + CaCl2 (s) If 102 g of CaO and 241 g of NH4C1 are mixed, what is the limiting reactant, and what mass of NH3 can be produced? The limiting reactant is Cao Mass of NH3 =

A fictitious metal called Oscium (MM = 72.4 g· mol) reacts with nitrogen gas according to the following reaction: 6 Oc (s) + N2(g) + 2 OC3N(s)

For the following reaction, 37.3 grams of sulfuric acid are allowed to react with 42.5 grams of zinc hydroxide. sulfuric acid (aq) + zinc hydroxide(s) → zinc sulfate (aq) + water (1) What is the maximum amount of zinc sulfate that can be formed? Mass= What is the formula for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? Mass= g.

Determine the maximum (theoretical) and actual yield of CaCO3, in grams, that can be produced from the precipitation reaction given 105.99 mol of Na2CO3.  Na2CO3 (aq) + CaCl2 ⋅2H2O → CaCO3 (s) + 2NaCl(aq) + 2H2O(aq)

of 15 Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese (IV) oxide. 4 HCl(aq) + MnO₂ (s)→ MnCl₂ (aq) + 2 H₂O(1) + Cl₂(g) A sample of 39.9 g MnO, is added to a solution containing 44.5 g HCI. B d > What is the limiting reactant? E HCI O MnO₂ What is the theoretical yield of Cl₂? theoretical yield: If the yield of the reaction is 86.1%, what is the actual yield of chlorine? D $ 4 I R C с F % 5 V T G MacBook Pro 6 7 I I Y H B - N 4 8 J I 1 M 9 K O < F H O L P command Question F { [ option 8 Cl₂ ? 1 delete

Chlorine gas can be produced in the laboratory by adding concentrated hydrochloric acid, HCl, to manganese(IV) oxide according to the following reaction: MnO2 (s)   +   4 HCl (aq)   →   MnCl2 (aq)   +   2 H2O (l)   +   Cl2 (g) What mass of MnO2 is required to produce 48.4 g Cl2 by the following reaction? Be sure to enter a unit with your answer.

For the following reaction, 0.557 moles of potassium hydroxide are mixed with 0.224 moles of phosphoric acid. potassium hydroxide(aq)+phosphoric acid(aq)= potassium phosphate(aq)+water(l)   What is the formula for the limiting reagent? What is the maximum amount of potassium phosphate that can be produced?

Small quantities of oxygen gas can be generated in the laboratory by heating potassium chlorate. 2 KClO3(s) → 2 KCl(s) + 3 O2(g) If 5.10 g of potassium chlorate is heated, what theoretical mass of oxygen gas should be produced? If only 1.68 g of oxygen is actually obtained, what is the percent yield?

Iron(II) sulfide reacts with hydrochloric acid according to the reaction FeS(s)+2HCl(aq)→FeCl2(aq)+H2S(s) A reaction mixture initially contains 0.218 mol FeS and 0.636 mol HCl. Once the reaction has reached completion, what amount (in moles) of the excess reactant is left?

A sample of calcium metal with a mass of 2.00 was reacted with excess oxygen. The following equation represents the reaction that took place: 2Ca(s)+O2(g)-> 2CaO(s) the isolated product CaO weighed 2.26g. What was the percent yield of the reaction?