For each of the following unbalanced chemical equations, suppose 10.0 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. a. C3 Hs (g) + O2 (9) → CO2 (g) + H2O(g) b. Al(s) + Cl2 (g) → AICI3 (s) c. NaOH(s) + C02 (g) → Na2 CO3 (s) + H20(1)

1. Complete and Balance the reaction. Include all states. If there is no reaction, write NO REACTION. Ca(s)+N2(g)T 2. What is the mass (in grams) of 4.25 x 1022 molecules of Mg3N2? T 3. Determine the empirical formula a molecule has the following elemental analysis: T 18.02% Carbon, 2.02 % Hydrogen, and 79.96% Bromine T (US) E O Fo MacBook Ain 吕0 O00 F4 F8 F9 F5 F6 F7 F3 & * %24

a. For the following unbalanced chemical equation, suppose 10.4 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. Enter the formula for the limiting reactant. C3H8 (9) + O2(g) → CO₂ (g) + H₂O(g) Limiting reactant: Mass of CO₂ Mass of H₂O = b. For the following unbalanced chemical equation, suppose 10.1 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. Al(s) + Cl₂ (g) → AlCl3 (s) = = g Limiting reactant: Mass of AlCl3 c. For the following unbalanced chemical equation, suppose 10.4 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. NaOH(s) + CO2(g) → Na2CO3 (s) + H₂O(1) Limiting reactant: Mass of Na2CO3 Mass of H₂O = = g g

12. Iron metal can be obtained from iron(III) oxide by reaction with carbon monoxide at elevated temperature according to the following equation. Fe203 + 3CO → 2Fe + 3CO2 a. How many moles of iron can be obtained from 1 mole of iron(III) oxide? b. How many grams of Fe2O3 are necessary to make 50 g of iron by this reaction?

26. The equation for the complete combustion of ethene (C2H4) is C2H4(9) + 302(9) → 2CO2(g) + 2H20(g) If 2.70 mol C2H4 reacts with 6.30 mol O2, identify the limiting reagent.

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Balance the equation c.

1.0 chem q

For the following unbalanced equation, calculate how many grams of each product would be produced by complete reaction of 34.2 g of SiH4. Indicate clearly the mole ratio used for the conversion. SiH (9) + NH3 (9)→ Si;N4 (s) + H2 (g) g SizN4 g H2

a. For the following unbalanced chemical equation, suppose 10.6 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. Enter the formula for the limiting reactant. C3H8 (9) + O2(g) → CO₂ (g) + H₂O(g) Limiting reactant: Mass of CO2: Mass of H₂O = b. For the following unbalanced chemical equation, suppose 10.1 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. Al(s) + Cl₂ (g) → AlCl3 (s) = Limiting reactant: = g Mass of AlCl3 c. For the following unbalanced chemical equation, suppose 10.6 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. NaOH(s) + CO2 (g) → Na2CO3(s) + H₂O(1) Limiting reactant: Mass of Na2CO3 Mass of H₂O = = g