There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: →+2Cu2Ss  3O2g + 2Cu2Os  2SO2g In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: →+Cu2Os  Cs + 2Cus  COg Suppose the yield of the first step is 86.%  and the yield of the second step is  64.% . Calculate the mass of copper(I) sulfide required to make  2.0kg  of copper.

What is Keq? The equilibrium constant, Kea, expresses the relationship between the reactants and products for a reaction at equilibrium. There are two types of equilibrium reactions: Homogenous: The states of matter are all the same. Heterogeneous: The states of matter differ. 1. Classify the following reactions as homogeneous or heterogeneous (highlight one) a. 2 SO₂(g) + O₂(g) = 2 SO³(g) homogeneous or heterogeneous b. 2NaHCO3(s) Na₂CO3(s) + H₂O(g) + CO₂(g) homogeneous or heterogeneous c. 3 H₂(g) + N₂(g) = 2 NH3(g) homogeneous or heterogeneous homogeneous or heterogeneous d. H₂O(g) + C(s) = H₂(g) + CO(g) homogeneous or heterogeneous e. Cu(s) + 2 AgCl(aq) = CuCl,(aq) + 2 Ag(s) riting Equilibrium Constants - Homogeneous Reactions is the universal equilibrium constant for reactions. It is a ratio of the amount of product to e amount of reactant in the reaction mixture. To write an equilibrium constant expression: Put the products on top and the reactants on bottom. contrations in…

Propane can be turned into hydrogen by the two-step reforming process. In the first step, propane and water react to form carbon monoxide and hydrogen: C,Hg(9)+3 H,0(9) --3 CO(g)+7H,(9) In the second step, carbon monoxide and water react to form hydrogen and carbon dioxide: Co(g)+H,0(9)-H,(9)+CO,(9) Write the net chemical equation for the production of hydrogen from propane and water. Be sure your equation is balanced.

The thermite reaction,Fe2O3 + Al S Al2O3 + Feproduces so much heat that the Fe product melts. This reactionis used industrially to weld metal parts under water,where a torch cannot be employed. It is also a favorite chemicaldemonstration in the lecture hall (on a small scale).(a) Balance the chemical equation for the thermite reaction,and include the proper states of matter.(b) Calculate how many grams of aluminum are needed tocompletely react with 500.0 g of Fe2O3 in this reaction.(c) This reaction produces 852 kJ of heat per mole of Fe2O3reacted. How many grams of Fe2O3 are needed to produce1.00 * 104 kJ of heat?(d) If you performed the reverse reaction— aluminum oxideplus iron makes iron oxide plus aluminum—would thatreaction have heat as a reactant or a product?