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

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.

2b2t

explanation:

2b2t