Consider this equation for the heated decomposition of potassium chlorate: 2KClO↓3(s) > 2KCl(s) + 3O↓2(g), ΔH = ?

Given these enthalpy of formation values:

KClO3: ΔHf = -391kJ/mol; KCl: ΔHf = -433kJ/mol

Calculate the enthalpy of the above reaction in kilojoules per mole of reactant.
Reference: ΔH = sum(HΔproducts) - sum(ΔHreactants)

What happens to isotopes that are unstable?

For the reaction, 4 a(g) + 3 b(g) => 2 c(g), the following data were obtained at constant temperature. experiment initial[a],mol/l initial [b],mol/l initial rate,m/min 1 0.200 0.150 5.00 2 0.400 0.150 10.0 3 0.200 0.300 10.0 4 0.400 0.300 20.0 which of the following is the correct rate law for the reaction? 1. rate = k[a]2[b]2 2. rate = k[a][b] 3. rate = k[a]2[b] 4. rate = k[a][b]2

Which of the following are sources of revenue for media companies? a. direct sales to producers b.advertising and subscriptions c. online purchase d. capital investments