For each of the following unbalanced chemical equations, suppose that exactly 1.90 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICl is expected (assuming that the limiting reactant is completely consumed). 2(s) + Cl2 (9) → ICI(9) Limiting reactant: Mass of ICl =

For the following unbalanced chemical equation, suppose that exactly 2.00 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). H2 (g) + MnO2 (s) → Mn0(s) + H2 O(1) Limiting reactant: Mass of H20 = For each of the following unbalanced chemical equations, suppose that exactly 1.90 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICI is expected (assuming that the limiting reactant is completely consumed). I2 (s) + Cl2 (9) → ICI(9) Limiting reactant: Mass of ICl =

Consider the following balanced equation for the combustion of butane, a fuel often used in lighters.2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(g)Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed.   Mass C4H10 Mass O2 Mass CO2 Mass H2O _____ 2.11 g _____ _____ 5.32 g _____ _____ _____ _____ _____ 13.12 g _____ _____ _____ _____ 8.44 g 252 mg _____ _____ _____ _____ _____ 198 mg _____

For the following unbalanced chemical equation, suppose that exactly 1.60 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of CO2 is expected (assuming that the limiting reactant is completely consumed). CS, (1) + 02 (9) → CO2(g) + SO2 (g) Limiting reactant: Mass of CO2 = For the following unbalanced chemical equation, suppose that exactly 1.45 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). NH3 (9) + CO2 (9) → CN, H,O(s) + H2O(1) Limiting reactant: Mass of H2O = b)

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. NaCl(s) + H₂SO4 (1) → HCl(g) + Na2SO4(s) Limiting reactant: Mass of excess reagent = g

For the following reaction, 0.358 moles of sulfuric acid are mixed with 0.228 moles of zinc hydroxide. sulfuric acid(aq) + zinc hydroxide(s) → zinc sulfate(aq) + water(e) What is the formula for the limiting reagent? What is the maximum amount of zinc sulfate that can be produced? moles

For the following reaction, 11.2 grams of glucose (C6H1206) are allowed to react with 15.5 grams of oxygen gas. glucose (C6H1206) + oxygen---> carbon dioxide + water What is the maximum amount of carbon dioxide that can be formed? Mass= __ g What is the FORMULA for the limiting reactant? What amount of the excess reactant remains after the reaction is complete? Mass= g

In the following reaction, which element is the limiting reactant? 2Fe(s) 3Cl2(g) → 2FeCl3(s) iron chlorine neither both Cannot be determined without the original starting mass of both reactants.

b For the following unbalanced chemical equation, suppose that exactly 6.10 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected (assuming that the limiting reactant is completely consumed). Enter the formula for the limiting reactant. MnO2 (s) + H2 SO4(ag) → Mn(SO4)2(s) + H2O(1) Limiting reactant: Mass of Mn(SO4)2 g Mass of H20 g

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