2.5 mol Na, 1 mol Br2 Express your answer as a chemical formula. ΑΣφ

For the reaction Ti(s) + 2 F2 (g) → TIF4(s) compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.

According to the following reaction, how many grams of ammonia will be formed upon the complete reaction of 23.1 grams of hydrogen gas with excess nitrogen gas?nitrogen (g) + hydrogen (g) ammonia (g)

For the reaction shown, find the limiting reactant for each of the initial quantities of reactants.   2.2 g Al and 1.8 g O2

Consider the following reaction between sulfur trioxide and water: SO3(g)+H2O(l)→H2SO4(aq) A chemist allows 61.5 g of SO3SO3 and 11.2 g of H2O to react. When the reaction is finished, the chemist collects 56.2 g of H2SO4 Determine the percent yield for the reaction.         Express your answer to three significant figures.

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)

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 =

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. Al(s) + Cl2(g) → AlCl3(s)limiting reagent AlCl2     AlCl3 produced

For the reaction below, find the limiting reactant for each of the initial amounts of reactants. 2 Na(s) + Br2(g) ------> 2 NaBr(s)a. 2 mol Na, 2 mol Br2

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