heat 2 Al(s) + Fe,O,(s) Al,0,(s) + 2 Fe(1) - If 16.3 kg Al reacts with an excess of Fe,O,, how many kilograms of Al, O, will be produced?

Nitrogen (N2)and hydrogen (H2) react to form ammonia(NH3). Consider the mixture of N2 and H2 shown in theaccompanying diagram. The blue spheres represent N, andthe white ones represent H. (a) Write the balanced chemicalequation for the reaction. (b) What is the limiting reactant?(c) How many molecules of ammonia can be made, assumingthe reaction goes to completion, based on the diagram?(d) Are any reactant molecules left over, based on the diagram?If so, how many of which type are left over?

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7.) A Sample Of 13.3g of Fe₂03 reacts with 16.89 CO со to yield Fe and Co₂. The balanced equation Fe₂O3 (s) + 3 C0g 2 Fe (5) + 300₂ (g) is Which Substance is the limiting reactant? What is the theoretical yield of Fe ? If the actual experimental yield for Fe is 8.41g what is the percent yield of Fe?

Consider the following unbalanced chemical equation. LIOH(s) + CO,(g) → Li,CO3(s) + H,0(1) If 68.1 grams of lithium hydroxide reacts with excess carbon dioxide, what mass of lithium carbonate will be produced?

6. Copper(1) iodide, Cul, is not stable enough to last long in storage, so it is generally made just prior to use. In can be prepared from copper sulphate and hydriodic acid by the following reaction: 2 Cuso,(s) + 4 HI(aq) - a) If 10.4 grams of CuSO, is used, calculate the number of grams of HI needed and the ---> 2 Cul(s) + 2 H,So,(aq) + L,(s) number of grams of each of the products that are produced. Show that the mass data are in accordance with the law of conservation of mass in chemical reactions. b) If 10.4 grams of copper(I) iodide were isolated from the reaction above, what is the percent yield of the reaction?

For the following unbalanced reaction, suppose exactly 5.85 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. CaC₂ (s) + H₂O(1) → Ca(OH)2 (s) + C₂H₂ (9) Limiting reactant: Mass of excess reagent =

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo

A chemist invents a new combustion analysis instrument that uses less O2(g) which saves money on each analysis. The improvement is that instead of CO2(g) being formed and trapped, CO(g) is formed and trapped. H2O (g) is also formed and trapped when substances that contain hydrogen are analyzed.(a) The chemist places 2.184 g of an unknown compound of carbon and hydrogen in the new analyzer. 4.627 g of CO (g) and 1.795 g of H2O (g) are produced. Find the empirical formula for the compound.(Molar masses (g/mol): CO = 28.0104, H2O = 18.015) (b) Despite the best efforts of the chemist, the molar mass of the compound cannot be determined (using this method). Clearly explain why this prevents the determination of the molecular formula

What is the limiting reagent and excess reactant?