According to the following reaction, how many moles of chlorine gas are necessary to form 0.632 moles phosphorus trichloride? phosphorus (P4) (s) + chlorine (g) →phosphorus trichloride (I) moles chlorine gas Submit Answer Retry Entire Group 4 more group attempts remaining

In the following reaction, oxygen is the excess reactant.SiCl4 + O2 → SiO2 + Cl2The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2 1 150 g 200 g 49.2 g 2 75 g 50 g 25.2 g Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work. Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction.                     Source                  StylesNormal

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How many molecules of SO₃ can be formed from 0.31 moles of O₂ (assuming excess SO₂) from the following UNBALANCED equation? SO₂(g) + O₂(g) → SO₃(g)

if i react 3.8 moles of H 2 with excess N 2 how many moles of NH3 molecules will be formed ? N2 + 3H2 ---->2NH3

According to the following reaction, how many moles of ethane (C2H6) will be formed upon the complete reaction of 0.851 moles hydrogen gas with excess ethylene (C2H4)?hydrogen (g) + ethylene (C2H4) (g) ethane (C2H6) (g)

Consider the following reaction . How many moles of water will be produced when 6.00 moles of oxygen reacts with 1.50 moles of C3h7SH?  C3H7SH(l) + 6 O2 (g) --> 3CO2 )g) + SO2(g) + 4H2O (g)

The first step in the reaction of Alka–Seltzer with stomach acid consists of one mole of sodium bicarbonate (NaHCO3) reacting with one mole of hydrochloric acid (HCl) to produce one mole of carbonic acid (H2CO3), and one mole of sodium chloride (NaCl). Using this chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 33 mol NaHCO3 and 77 mol HCl.HCl. moles of carbonic acid :  ____________________mol   Which of the two reactants limits the number of moles of H2 CO3 that can be made? 1. HCl 2. NaHCO3   How much excess reactant remains after the reaction? excess reactant : ___________________mol

Some rockets in the 1960s used hydrazine (N2H4) as a fuel, and nitric acid (HNO3) asan oxidizer. The byproducts of this reaction were nitrogen gas and water. If you were tobalance this reaction, you would get the correct proportions if you used: a) 4 mol N2H4 for every 3 mol HNO3b) 2 mol of N2H4 for every 3 mol HNO3c) 10 mol of N2H4 for every 8 mol HNO3d) 8 mol N2H4 for every 6 mol HNO3e) 6 mol N2H4 for every 4 mol HNO3

can you solve these 2 and just provide the answer I solved most of the work I just couldnt get the answer right