If 1176 grams of FeS2 is allowed to react with 704 grams of O2 according to the following unbalanced equation, how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2
1. Consider the following reaction at equilibrium. 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g) a. What will happen if the pressure increased? b. What will happen if the concentration of FeS2(s) is decreased? 2) The following reaction is exothermic: What direction will the equilibrium shift if the following changes are made? 2 SO2(g) + O2(g) ⇌ 2 SO3(g) a) Raising the temperature b) Adding SO3 c) Removing O2 d) Decreasing the volume
Determine the volume of SO2 gas in liters formed from the reaction of 96.7g of FeS2. Assume the reaction is done at 183 torr and 310K. 4 FeS2(s) + 11 O2(g) --> 2 Fe2O3(s) + 8 SO2(g)
1. What will happen in the following reaction if FeS2 is added to the reaction? 4 FeS2 (s) + 11 O2(g) = 2 Fe2O3 (s) + 8 SO2 (g) The equilibrium constant will increase. The equilibrium will change in the direction of the reactants. The equilibrium will change in the direction of the products. No change in equilibrium is observed. The equilibrium constant will decrease.
A) An aqueous solution of SO2 reduces aqueous KMnO4 to MnSO4(aq). Write balanced equation for this reaction. Express your answer as a chemical equation. Identify all of the phases in your answer. B) An aqueous solution of SO2 reduces acidic aqueous Cr2O72− to aqueous Cr3+. Write balanced equation for this reaction. Express your answer as an ionic equation. Identify all of the phases in your answer. C) An aqueous solution of SO2 reduces aqueous Hg2(NO3)2 to mercury metal. Write balanced...
Based on the balanced reaction 4 Fe + 3 O2 → 2 Fe2O3, a student starts this reaction with these amounts of chemicals: 12 mol Fe, 15 mol O2, and 0 mol Fe2O3. What chemical is the limiting reactant?
Based on the balanced reaction 4 Fe + 3 O2 → 2 Fe2O3, a student starts this reaction with these amounts of chemicals: 12 mol Fe, 15 mol O2, and 0 mol Fe2O3. What chemical is the excess reactant? SHOW WORK
Consider the following reaction at equilibrium. What will happen if SO2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g) A.) The equilibrium will change in the direction of the products. B.) The equilibrium constant will increase. C.) The equilibrium will change in the direction of the reactants. D.) The equilibrium constant will decrease. E.) No change in equilibrium is observed.
to P4.22 Calculate the standard enthalpy of formation of FeS2(s) at 550.°C from the data tables and the following data at 298.15 K. Assume that the heat capacities are independent of temperature. Substance Fe(s) FeS2(s) Fe2O3(s) S(rhombic) SO2(g) AfHⓇ (kJ mol-l) -296.81 Cp.m/R 3.02 7.48 2.72 -824.2 You are also given that for the reaction 2FeS2(s) + 11/202(g) ► Fe2O3(s) + 4802(g), A,Hº = -1655 kJ mol-!
Please show your work Section 5.1 #9 Given the balanced chemical equation Fe2O3(s) + 3SO3(g) → Fe2(SO4)3 how many molecules of Fe2(SO4)3 are produced if 321 atoms of S are reacted? Section 5.2#19 How many moles are present in 1.223 g of SF6? Section 5.3 #7 Write the balanced chemical reaction for the combustion of C5H12 (the products are CO2 and H2O) and determine how many moles of H2O are formed when 5.8 mol of O2 are reacted.