Iron reacts with oxygen in the air in a combination to produce iron (III) oxide (or rust) according to the following reaction:  4  Fe (s)  +   3 O2 (g)  →  2 Fe2O3 (s)    If a 29.0 g iron pipe is left outside, allowing it to react with excess oxygen in the air until it is all converted to rust, what is the mass of Fe2O3 produced?

Consider the reaction below: H2S (g) + Cl2 (g) → S (s) + 2 HCl (g) The element                   is undergoing oxidation and                     is the oxidizing agent.

A system performs 111 kJ of work on its surroundings and gains 89 kJ of heat. What is the value of ΔE (in kJ) for the system?

231 mL of water is added to 19 mL of 7.0 M AgNO3 What is the concentration, in M, of the resulting solution? Hint:  Vwater = V2 (final volume) – V1 (initial volume)

A system performs 111 kJ of work on its surroundings and releases 89 kJ of heat. What is the value of ΔE (in kJ) for the system?

A system releases 43 kJ of heat and has 94 kJ of work done on it. What is the value of ΔE (in kJ) for the system?

Of the following, the heat of formation,  ΔH°f, is zero for              .  

Consider the reaction of iron (III) oxide with carbon to form iron metal and carbon dioxide gas: 2 Fe2O3 (s) + 3 C (c) →  4 Fe (s) +  3 CO2 (g)            

Based on the activity series, which of the following solutions would result in a spontaneous single displacement reaction with lead metal?

Consider the reaction where hydrogen gas reacts with bromine gas to form hydrogen bromide gas: H2 (g) + Br2 (g) →  2 HBr (g)