Aluminum sulfate has many uses in industry. It can be prepared by reacting aluminum hydroxide and sulfuric acid: 2 Al(OH)3+3 H2504 AlZ(SO4)3+6 H2O(a) When 35.0 g of Al(OH)3 and 35.0 g of H2SO4 are reacted, how many moles of Al2(SO4) 3 can be produced? Which substance is the limiting reactant? (b) When 45.0 g of H2S04 and 25.0 g of A(OH)3 are reacted, how many grams of Al2(SO4)3 are produced? Which reactant is in excess? (c) In a reaction vessel, 2.5 mol of Al(OH)3 and 5.5 mol of H2SO4 react. Determine which substances will be present in the container when the reaction goes to completion and how many moles of each

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

1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction.  b) What mass of acetic acid is in the aqueous solution?  c) Which of the reactants is the limiting reagent? Justify your answer.  d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction?  f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?      please answer d, e and f

Balance each reaction, then suppose exactly 13.3 g of each reactant is taken. Indicate which reactant is the limiting reagent. Calculate the mass of each product that is expected. (c) NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l)limiting reagent? NaOHCO2     Na2CO3 produced  g H2O produced  g

A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, CgH5Br, and HBr. C6H6 + Br2 --> C6H5Br + HBr What is the theoretical yield of bromobenzene in this reaction when 29.2 g of benzene reacts with 70.5 g of bromine? grams Which chemical is the limiting reactant? Select an answer If the actual yield of bromobenzene was 39.5 g, what was the percent yield?

Iron (200.0g reacts with chlorine gas (200.0g) to form 150.0 g of solid Iron (III) Chloride. The balanced chemical equation is: Fe(III)(s) + 3Cl2(g) = Fe(III)(Cl2)3 Identify the limiting reactant. Assuming that only 150.0 g of Fe(III) chloride are formed. Which reactant is in excess and by how much?

The rocket boosters of the space shuttle Discovery, launched on July 26, 2005, used a fuel mixture containing primarily solid ammonium perchlorate, NH4ClO4, and aluminum metal. The unbalanced chemical equation for the reaction is given below. (Hint: Balance the elements in the order Cl, H, O, Al, N.) Al(s) + NH4CIO4(s) Al₂O3(s) + AlCl3(s) + H₂O(l) + N₂(g) What is the mass (in kilograms) of NH4ClO4 consumed per kilogram of Al, assuming a percent yield of 87.20%? (Answer with two decimal places.)

Consider the balanced chemical equation: 3 H₂(g) + N₂(g) → 2 NH₃(g) If 46.8 g H₂ and 179.4 g N₂ are mixed to form NH₃, which of the following substances is the limiting reactant?   A) nitrogen (N₂) B) hydrogen (H₂) C) ammonia (NH₃)

A sample of 4.00g of methane (CH4) is mixed with 15.0g of chlorine (Cl2). Determine which is the limiting reactant according to the following equation: CH4(g) + 4Cl2(g)> CCl4(e) + 4HCl(g)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s)In a particular experiment, 3.50 g samples of each reagent are reacted.a) What is the limiting reagent?b) What is the theoretical yield in grams of lithium nitride?c) If only 4.25 grams of lithium nitride is produced in the reaction, what is the percent yield?