Calculate how many grams of the second reactant would be required to react completely with 13.36 moles of the first reactant. Cu(s) + O2(g) → Cu2O(s) Molar Mass: Cu: 63.55 g/mol O: 16 g/mol  Round off your answer to 2 decimal places.

For each of the following balanced reactions, suppose exactly 5.00 moles of each reactant are 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) + 2H2O(l) ® Ca(OH)2(s) + C2H2(g) 3AgNO3(aq) + Al(s) ® 3Ag(s) + Al(NO3)3(aq)

Solutions of sodium hypochlorite (NaClO) are sold as laundry bleach. This compound is made by the following balanced reaction. 2 NaOH + Cl2 ==> NaCl + NaClO + H2O How many g of NaClO are made if 6.23 g NaOH completely react?  Give your answer to 2 decimal places.   Molar Mass, g/mol NaOH 40.00 Cl2 70.91 NaCl 58.44 NaClO 74.44 H2O 18.02

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