Consider this reaction: Fe2O3(s)+3H2(g)=2Fe(s)+3H2O(g) =98.7kJ If this system was in closed container at equilibrium, and a small about of hydrogen gas was injected into the container, how would the reaction respond? Or which direction would the reaction “shift” towards? Options: 1) Making more reactants 2) making more products

If the element whose electric configuration ends in the d sublevel, the element is calssified as? a. inner transition b. noble gases c. representative d. transition

Consider the reduction reactions and their equilibrium constants. cu+(aq)+e−↽−−⇀cu(s)pb2+(aq)+2e−↽−−⇀ pb(s)fe3+(aq)+3e−↽−−⇀fe(=6.2×108=4. 0×10−5=9.3×10−3 cu + ( aq ) + e − ↽ − − ⇀ cu ( s ) k =6.2× 10 8 pb 2 + ( aq ) +2 e − ↽ − − ⇀ pb ( s ) k =4.0× 10 − 5 fe 3 + ( aq ) +3 e − ↽ − − ⇀ fe ( s ) k =9.3× 10 − 3 arrange these ions from strongest to weakest oxidizing agent.

Avogradoa number was calculated by determining the number of atoms in?