How much heat is evolved in converting 1.00 mol of steam at 145.0 ∘c to ice at -55.0 ∘c? the heat capacity of steam is 2.01 j/(g⋅∘c) and of ice is 2.09 j/(g⋅∘c).

Heat evolved = 57.9 kJ i.e. -57.9 kJ

Explanation:

The transition from steam at 145 C to ice at -55 C involves the following steps:

Step 1: Heat involved in the change from steam at 145 C to steam at 100 C

Moles of steam (H2O)= 1 mole

Molar mass of H2O = 18 g/mol

Step 2: Phase change from steam at 100 C to water at 100 C

where ΔH(cond) = heat of condensation = -40.7 kJ/mol

n = number of moles

Step 3: Heat involved in the change from water at 100 C to water at 0 C

Step 4: Phase change from water at 0 C to ice at 0 C

where ΔH(fusion) = -6.01 kJ/mol

n = number of moles

Step 5: Heat involved in the change from ice at 0 C to ice at -55 C

Step 6: Total heat evolved

q = -1.628 -40.7 -7.524-6.01-2.069 = -57.9 kJ

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.