You start with 23.00g of aluminum and 55.00g of NH4ClO4. What is the limiting reagent? 10Al(s) + 6NH4ClO4(s) --> 4Al2O3(s) + 2AlCl3(s) + 12H2O(g) + 3N2(g).
10Al(s) + 6NH4ClO4(s) --> 4Al2O3(s) + 2AlCl3(s) + 12H2O(g) + 3N2(g).
according to balanced reaction
10x 27 g AL reacts with 6 x 117.49 g NH4ClO4
23.0 g Al reacts with 23 x 6 x 117.49 / 10 x 27 = 60.05 g NH4ClO4
but we have 55.0 g NH4ClO4.
so limiting reagent = NH4ClO4
You start with 23.00g of aluminum and 55.00g of NH4ClO4. What is the limiting reagent? 10Al(s)...
The solid rocket boosters of the space shuttle employed the following oxidation/reduction reaction: 10 Al (s) +6NH4CLO4 (s) --> 4Al2O3 (s) +2AlCl3 (s) + 12 H2o (g) + 3N2 (g) ?Hf 0 for NH4ClO4= -295.3 KJ/mol Al=0 KJ/mol Al2O3= -1676 KJ/mol AlCl3= -704.2 KJ/mol H2O= -241.82 KJ/mol N2= 0 KJ/mol Calculate the standard enthalpy of this reaction. How much energy is released when 100,000 kg of ammonium perchlorate (and excess aluminum) is burned?
25) Which is the limiting reagent in the following reaction given that you start with 15.5 g of Na2S and 12.1 g CusO4? Reaction: Na2S+ CuSO4Na2SO4+Cus A) Na2S B) CuSO4 C) Na2SO4 D) CuS E) not enough information
·00 | Limiting Reagent Using Mass Example Problem 4 What is the limiting reagent when Silver metal reacts with sulfur to form silver sulfide. If you have 50 grams of Silver and 10 g of Sulfur. 12
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)?2AlCl3(s) What is the maximum mass of aluminum chloride that can be formed when reacting 27.0 g of aluminum with 32.0 g of chlorine?
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)→2AlCl3(s) You are given 16.0 g of aluminum and 21.0 g of chlorine gas. If you had excess aluminum, how many moles of aluminum chloride could be produced from 21.0 g of chlorine gas, Cl2? Express your answer to three significant figures and include the appropriate units.
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)?2AlCl3(s) What is the maximum mass of aluminum chloride that can be formed when reacting 17.0g of aluminum with 22.0g of chlorine?
Aluminum reacts with chlorine gas to form aluminum chloride. 2Al(s)+3Cl2(g)→2AlCl3(s) What minimum volume of chlorine gas (at 298 KK and 217 mmHgmmHg) is required to completely react with 8.48 gg of aluminum?
Consider the following UNBALANCED equation: Na(s) + Cl2(g) -> NaCl(s). a.) Calculate the limiting reagent when 55.0 g of react with 67.2 g of Cl2. (Show all work, and clearly state which is the limiting reagent.) b.) What is the theoretical yield, in grams, of NaCl? c.) If 105g of NaCl is produced from the reaction, what is the percent yield of NaCl?
a. 2Al(s)+3Cl2(g)→2AlCl3(s) You are given 19.0 g of aluminum and 24.0 g of chlorine gas.If you had excess aluminum, how many moles of aluminum chloride could be produced from 24.0 g of chlorine gas, Cl2? b. Determine the balanced chemical equation for this reaction. C8H18(g)+O2(g)→CO2(g)+H2O(g) c. 3H2(g)+N2(g)→2NH3(g) 1.08 g H2 is allowed to react with 10.3 g N2, producing 1.04 g NH3. What is the theoretical yield for this reaction under the given conditions? What is the percent yield for...
BaCl2 +Na2SO4 = BaSO4(s) + 2Na +2Cl Calculate the mass of the limiting reagent that reacted in the experiment for each trial. Hints: Your limiting reagent is either BaCl2 or Na2SO4 calculate # of moles of your limiting reagent from the mass of your precipitate Trial data: Mass of unknown: 1.104 g Actual mass weighted of Na2SO4: 1.425 g Mass of precipitate: 0.137 g