A.) Consider the combustion of hydrogen to make water. If you start with 2.47 grams of H2 and 12.02 grams of O2, what is the limiting reactant and the theoretical yield of water? b.) The balanced chemical equations below represents the burning of carbon monoxide in oxygen to form carbon dioxide. If you have 1.000 g each of CO and O2, determine the limiting reactant and the theoretical yield in grams.

2CO(g) + O2(g) → 2CO2(g)

Plzz a sample of table sugar (sucrose, c12h22o11) has a mass of 7.801 g. ● a) calculate the number of moles of c12h22o11 in the sample b) calculate the number of moles of each element in c12h22o11 (number of moles of c, number of moles of h & number of moles of o) in the sample. (use your answer from part a as your starting point.) show your work and highlight your final answer. calculate the number of atoms of each element in c12h22o11 (number of atoms of c, number of atoms of h & number of atoms of o) in the sample. (use your answers from part b as your starting for each element.) show your work and highlight your final answer.