1. C2H2(g) + 5/2 O2(g) à 2 CO2(g) + H2O(l) ΔH = -1299.5 kJ

C(s) + O2(g) à CO2(g) ΔH = -393.5 kJ

H2+ ½ O2(g) à H2O(l) ΔH = -285.8 kJ

Calculate ΔHrxnfor the following reaction:

2 C(s) + H2(g) à C2H2(g) ΔH = ???

2.

Oxidation is a common reaction for many metals. Given the following equations, first balance them, then determine which species are oxidized and which are reduced. Then look at the “activity series” table in your textbook and determine whether the reaction can happen or not.

a) Fe(s) + Ag2SO4(aq) à FeSO4(aq) + Ag(s)

b) Mg(NO3)2(aq) + Li (s) à LiNO3(aq) + Mg(s)

c) Cu(MnO4)2(aq) + K(s) à KMnO4(aq) + Cu(s)

3.The reaction between potassium superoxide, KO2, and CO2is used as a source of O2and absorber of CO2in self-contained breathing equipment used by rescue workers. A) If 40.0 grams of KO2and 40.0 grams of CO2are present in the container, how many grams of O2are produced? B) Calculate the percent yield if 10 g of O2were actually used until the tank was empty.

4 KO2+ 2 CO2à 2 K2CO3+ 3 O2

Best Answer