When 1.42g of iron reacts with 1.80g of chlorine, 3.22g of fecl2(s) and 8.60kj of heat is produced. what is the enthalpy change for the reaction when 1 mole of fecl2(s) is produced.

ΔH for 1 mole of FeCl2 is -338.58 kJ/mol

Explanation:

Step 1: Data given

Mass of iron = 1.42 grams

Mass of chlorine = 1.80 grams

Mass of FeCl2 = 3.22 grams

Heat produced = 8.60 kJ (ΔH = -8.60 kJ because the reaction is exothermic)

Molar mass of Fe = 55.845 g/mol

Molar mass of Cl2 = 70.9 g/mol

Molar mass of FeCl2 = 126.75 g/mol

Step 2: The balanced equation

Fe + Cl2 → FeCl2

Step 3: Calculate moles of FeCl2

Moles FeCl2 = Mass FeCl2 / Molar mass FeCL2

Moles FeCl2 = 3.22 grams / 126.75 g/mol

Moles FeCl2 = 0.0254 moles

Step 4: Calculate the enthalpy change for 1 mole of FeCl2

For 0.0254 moles of FeCl2 ΔH is -8.60 kJ

For 1 mole of FeCL2 ΔH = -8.60 / 0.0254mol = -338.58 kJ/mol

ΔH for 1 mole of FeCl2 is -338.58 kJ/mol

the answer is c.the valence of the atoms combine .

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.