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)
For each of the following reactions, calculate the grams of indicated product when 27.0 g of...
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
Consider the following reaction: Fe3O4(s) + 4H2(g) --heat--> 3Fe(s) + 4H2O(l) What mass (in g) of Fe3O4 is needed to consume 2.17 g of H2? Enter only the numeric value of your answer (no units).
Consider the following reaction: Fe3O4(s) + 4H2(g) --heat--> 3Fe(s) + 4H2O(l) What mass (in g) of Fe3O4 is needed to consume 1.52 g of H2? Enter only the numeric value of your answer (no units).
Consider the following reaction: 3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g) How many grams of steam must react to produce 370. g of Fe,O ?
Consider the following reaction: Fe3O4(s) + 4H2(g) --heat--> 3Fe(s) + 4H2O(l) What mass (in g) of Fe3O4 is needed to consume 1.05 g of H2? Enter only the numeric value of your answer (no units).
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...
1.) Consider the reaction: Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.48 moles of Fe3O4(s) react at standard conditions. G°rxn = kJ 2.)Consider the reaction: H2(g) + Cl2(g)2HCl(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.750 moles of H2(g) react at standard conditions. G°rxn = kJ
Consider the reaction: Fe3O4(s) + 4H2(g)—>3Fe(s) + 4H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.79 moles of Fe3O4(s) react at standard conditions. ASºsystem = J/K
For each of the reactions, calculate the mass (in grams) of the product formed when 15.34 g of the bolded reactant completely reacts. Assume that there is more than enough of the other reactant. 1. 2K(s)+Cl2(g)−−−−−→2KCl(s) 2. 2K(s)+Br2(l)−−−−−→2KBr(s) 3. 4Cr(s)+3O2(g)−−−−−→2Cr2O3(s) 4. 2Sr(s)−−−−+O2(g)→2SrO(s)
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