Given the reaction: 2Al (s)+ 3Cl2 (g) ---->2AlCl3 (s)
1. Find the limiting reactant if 82.5g of Al and 247g of Cl2 are used?
2. What is the theoretical yield?
Someone, please help me understand this, I tried the problem on my own, I just need to make sure I went about it the right way!
Given the reaction: 2Al (s)+ 3Cl2 (g) ---->2AlCl3 (s) 1. Find the limiting reactant if 82.5g...
2Al(s) + 3Cl2(g) → 2AlCl3(s) Determine the mass (in g) of AlCl3 formed if 74.6 g of Al reacts with 74.6 g of Cl2.
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s References] TUTOR Limiting Reactants: Compare Reactant Moles The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product Consider the reaction: 2 Fe(s) +3 Cl2(g) 2 FeCl3(s) If 19.85 g Fe is mixed with 14.22 g Cl2, calculate the theoretical yield (g) of FeCl3 produced by the reaction g Show Approach Show Tutor Steps Submit
For the following reaction, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants: 2Al(s)+3Cl2(g)→2AlCl3(s) Part B 7.4 g Al and 25.2 g Cl2 Express your answer using three significant figures. Part C 0.235 g Al and 1.10 g Cl2 Express your answer using three significant figures.
For the reaction shown, compute the theoretical yield of product (in grams) for each of the following initial amounts of reactants. 2Al(s)+3Cl2(g)→2AlCl3(s) Part B 7.4 g Al, 25.0 g Cl2 Express your answer using three significant figures. Part C 0.235 g Al, 1.20 g Cl2 Express your answer using three significant figures.
2. ( pls.) Limiting Reactant and Theoretical Yield (7 pts.) 2Na (s) + Cl2 (g) → 2NaCl (s) You are given 84.9 g Na and 53.2 g Cl2. Find the limiting reactant, and calculate the theoretical yield in grams from the reaction shown above. (Box your answers!) Na = 22.990 g/mol; CI = 35.453 g/mol PACA