If the amount of product made (FeO) was determined to be 4.82 moles of FeO, how many MOLES of iron atoms are expected to be in the product?  How many MOLES of oxygen atoms are expected to be in the product?

During a laboratory experiment, a student initiated a reaction with 19.5 g of NaBH4 and excess BF3. When the reaction was complete, the student had collected 7.00 g of B2H6 gas. From this data, calculate the percent yield of B2H6.

A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields 15.40 mg CO2 and 7.88 mg H2O. The molar mass of the compound is 122.1 g/mol. What are the empirical and molecular formulas of the compound?

Consider the balanced chemical equation when 18.3 g Al is reacted with 113 g I₂ to form AlI₃(g). a. Calculate the theoretical yield in grams AlI₃ from the complete reaction of 18.3 grams Al according to the following balanced chemical equation: 2 Al(s) + 3 I₂(s) → 2 AlI₃(s) b. Calculate the theoretical yield in grams AlI₃ from the complete reaction of 113 grams I₂ according to the following balanced chemical equation: 2 Al(s) + 3 I₂(s) → 2 AlI₃(s) c. Which of the following substances is the limiting reactant? 2 Al(s) + 3 I₂(g) → 2 AlI₃(g) d. What is the mass in grams of the excess Al remaining after the partial reaction of 18.3 g Al with 113 g I₂? 2 Al(s) + 3 I₂(g) → 2 AlI₃(g)

Nitesh

Consider the following balanced chemical reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g) What is the maximum mass (in grams) of ammonia (NH3) that can be produced from 9.36 g of N2 and 4.92 g of H2?

8. Butane, a natural gas used in lighters, has a molar mass of 58.12 g/mol. How many particles are present inside a lighter if there is 1.00 gram of butane in it? 6.02 · 1023 particles 1.75 · 1020 particles 3.50 · 1020 particles O 1.04 · 1022 particles

If 36.0 g of C3H8 and 112 g of O2 are placed in a closed container and the mixture is ignited, what is the maximum mass of CO2 that could be produced? The other product of the reaction is water.     68.9 g     74.7 g     86.8 g     92.4 g     108 g

Lithium reacts with nitrogen to form lithium nitride. 6 Li(s) + N2(g) → 2 Li3N(s) In one experiment 3.0 mole of Li is combined with 1.0 mole of N2. In another experiment 13.88 g of Li reacts completely with excess N2. What mass of Li3N (34.83 g mol–1) is formed?   11.6 g   23.2 g   55.6 g

In an experiment, 3.250 g of NH3 reacted with 3.50 g of O₂. Supposed that the reaction produced 2.13 g NO, what is the percent yield of the reaction if the predicted amount is 3.51 g of NO?