any help? thanks EXAM #2 2. 20.0 g of AlzS3 and 20.0 g of H20 are reacted according to the following reaction: Al S...
Al253 (s) + 6H20 (0) --> 2Al(OH)3 (aq) + 3H2S (8) How many grams of H2S will be produced from 30.0 g of Al S3 and 20.0 g of H2O? Which of these reactants is the limiting reactant?
If 20 g of Na2SO4 is reacted with 20 g of Al(NO3)3 according to the following equation: 3 Na2SO4 + 2 Al(NO3)3 --> Al2(SO4)3 + 6 NaNO3 How many grams of the excess reactant will remain after the reaction, assuming that all of the limiting reactant reacts to form the products?
Determine the theoretical yield of H2S (in grams) if 76.0 g Al2S3 and 53.0 g H2O are reacted according to the following balanced reaction. Identify the limiting reactant. Al2S3 (s) + 6H2O (l) ---> 2 Al(OH)3 (s) + 3 H2S (g)
Phosphoric acid can be prepared from calcium phosphate according to the following reaction: Ca3(PO4)2 (s) + 3 H2SO4 (l) → 3 CaSO4 (s) + 2 H3PO4 (l) 310. g/mol 98.0 g/mol 136 g/mol 98.0 g/mol [a] If 0.664 mole of Ca3(PO4)2 are combined with 1.53 mole of H2SO4, how many grams of H3PO4 can be produced? [4 pts] [b] If 62.6 g of H3PO4 is actually produced in the above reaction, what is the percent yield for the reaction? [2...
1. Aluminum reacts with oxygen according to the following reaction: 4 Al(s) + 3 O2(g) -> 2 Al2O3 If 8.00 moles of oxygen are reacted with 8.00 moles of aluminum to completion, which is the excess reactant?
Aluminum oxide (Al2O3) is produced according to the following equation. 4 Al(s) + 3 O2(g) → 2 Al2O3(s) If the reaction occurs with an 82.4% yield, what mass of aluminum should be reacted with excess oxygen to produce 45.0 grams of Al2O3? a. 54.6 g Al b. 37.9 g Al c. 35.1 g Al d. 23.8 g Al e. 28.9 g Al How do we solve this problem
2. what is the limiting reactant if 0.5g Al is reacted with 3.5g CuCl2? Take into account CuCl2 is a dihydrate when calculating the molecular weight is this EC? Limiting Reactant and Percent Yield Lab Objectives: top 5 colors • Learn to determine the limiting reagent of a reaction. • Learn how to calculate theoretical, actual, and percent yield of a reaction. Background: During a chemical reaction when two substances react, often times one reactant will be consumed before the...
please help with all questions! Fall 2109 CHE 151-01 Exam 2 Chapter 4-6 Question 5 Question 6 (21 Points) Al2S3 + H2O - Al(OH)3 + H2S Suppose 316.0 g aluminum sulfide reacts with 0.493 kg of water. a) Write the balanced equation (2 Points) b) What % of Al(OH)3 is Al by mass? (2 Points) c) Identify the limiting and excess reagents (2Points) d) Calculate the number of moles and the mass in (g) after the reaction is complete for:...
According to the following reaction, what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol, H2O = 18.02 g/mol. Al2S3(s) + 6 H2O(l) ? 2 Al(OH)3(s) + 3 H2S(g) a)14.00 g b)8.33 g c)19.78 g d)17.22 g e)28.33 g
2. a. Nitrogen dioxide and hydrogen are reacted in the gas phase, in the presence of a catalyst, to produce ammonia and water; write a balanced equation for this reaction. (2 pts) b. If 73.2 g of nitrogen dioxide and 10.6 g of hydrogen are mixed together and react to form ammonia, identify the limiting reactant and calculate the theoretical yield (in grams) of ammonia produced. (6 pts) c. 12.9 g of ammonia is actually produced in this reaction; based...