For each of the following reactions, calculate the grams of indicated product when 17.2 g of the first reactant and 10.5 g of the second reactant are used.
Part B:
Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l)
Calculate the mass of Fe.
Part C
Al2S3(s)+6H2O(l)→2Al(OH)3(aq)+3H2S(g)
Calculate the mass of H2S
For each of the following reactions, calculate the grams of indicated product when 17.2 g of...
For each of the following reactions, calculate the grams of indicated product when 16.4 g of the first reactant and 10.1 g of the second reactant are used. You may want to reference (Pages 253 - 258) Section 7.9 while completing this problem. AlzS3 (s) + 6H2O(1)——2Al(OH)3 (aq) + 3H2S(g) Calculate the mass of H2S. .: HÅR O 2 ? mass of (H2S) = Value Units Submit Submit Request Answer Learning Goal: To calculate theoretical and percent yields, given the...
Determine which of the following chemical equations are correctly balanced. Fe2O3(s)+CO(g)→2Fe(s)+CO2(g) Al2S3(s)+H2O(l)→2Al(OH)3(s)+3H2S(g) 2Cr(s)+3O2(g)→Cr2O3(s) SiO2(s)+4HF(aq)→SiF4(g)+2H2O(l)
For each of the following reactions, calculate the grams of indicated product when 27.0 g of the first reactant and 40.0 g of the second reactant is used: 3Fe(s)+4H2O(l)→Fe3O4(s)+4H2(g) find(H2)
Balance the chemical equations. Express your answer as a chemical equation. Fe2O3(s)+CO(g)→2Fe(s)+CO2(g) Al2S3(s)+H2O(l)→2Al(OH)3(s)+3H2S(g) 2Cr(s)+3O2(g)→Cr2O3(s)
determine the theoretical yield in H2S (in moles) of 16 mol Al2S3 and 16 mol H2O are reacted according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17g/mol. Al2S3(s) + 6H2O(l) --> 2Al(OH)3(s) + 3H2S(g)
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?
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)
Calculate the maximum numbers of moles and grams of H2S that can form when 153.0 g of aluminum sulfide reacts with 143.0 g of water: Al2S3 + H2O → Al(OH)3 + H2S [unbalanced] ______ mol H2S ______ g H2S What mass of the excess reactant remains? ______ g excess reactant
Question 4 [10] Predict the value of AS for the following reactions. (a) Au2S3(s) + 3H2(g) + 3H2S(g) + 2Au(s) AS is Not yet answered Marked out of 10.00 (b) UO2(s) + 4HF(0) + UF4(s) + 2H2O(0) AS is (c) 4KO2 (s) + 2H2O(g) + 4 CO2(g) → 4KHCO3(s) + 302(g) AS is (d) 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s) AS is (e) C2H3CI() + 5/2O2(g) → 2C02(g) + H2O(g) + HCl(9) AS is Previous nane Navtinac
For each of the reactions, calculate the mass (in grams) of the product formed when 15.46 g of the BOLD reactant completely reacts. Assume that there is more than enough of the other reactant. Express your answer using four significant figures. Part A 2K(s)+Cl2(g)––––––→2KCl(s) Answer: m= ? g Part B. 2K(s)+Br2(l)––––––→2KBr(s) Answer: m= ? g Part C 4Cr(s)+3O2(g)––––––→2Cr2O3(s) Answer: m= ? g Part D 2Sr(s)–––––+O2(g)→2SrO(s) Answer: m= ? g