The standard molar heat of fusion of ice is 6020 j/mol. calculate q, w, and ∆e for melting 1.00 mol of ice at 0◦c and 1.00 atm pressure. 1. q = 6020 j/mol

Answer :    q = 6020 J, w = -6020 J, Δe = 0

Solution : Given,

Molar heat of fusion of ice = 6020 J/mole

Number of moles = 1 mole

Pressure = 1 atm

Molar heat of fusion : It is defined as the amount of energy required to melt 1 mole of a substance at its melting point. There is no temperature change.

The relation between heat and molar heat of fusion is,

 (in terms of mass)

or,     (in terms of moles)

Now we have to calculate the value of q.

When temperature is constant then the system behaves isothermally and Δe is a temperature dependent variable.

So, the value of

Now we have to calculate the value of w.

Formula used :    

where, q is heat required, w is work done and is internal energy.

Now put all the given values in above formula, we get

w = -6020 J

Therefore, q = 6020 J, w = -6020 J, Δe = 0

Trial 1 (20.61 mL HCl):  

⇒ 0.121 M

Trial 2 (20.06 mL HCl):  

⇒ 0.125 M

Trial 3 (19.67 mL HCl):  

⇒ 0.122 M

the answer for the next question, Compute the average concentration (molarity) of HCl for all three trials, is 0.123 M.

Explanation: