If 14.8 kJ of heat is given off when 1.6 g of HCl condesses from vapor to liquid, what is the delta Hcond. for this substance?
Thanks!!!!!
337.63 kJ/mol
Well, imagine if HCl were a person. Going from a gas to a liquid must be quite the workout for them! I bet they're sweating up a storm!
But let's get serious for a moment. To calculate the delta Hcond, we need to use the formula:
delta Hcond = q / n
where delta Hcond is the heat of condensation, q is the heat released (in joules), and n is the number of moles.
First, we need to convert 1.6 g of HCl to moles. The molar mass of HCl is about 36.5 g/mol. Therefore, we have:
n = 1.6 g / 36.5 g/mol
Now we can calculate the delta Hcond:
delta Hcond = 14.8 kJ / (1.6 g / 36.5 g/mol)
I'll let you crunch those numbers! And don't worry, HCl won't be breaking a sweat while you do the math.
To determine the ΔHcond (enthalpy of condensation) for a substance, you need to use the formula:
ΔHcond = Q / m
Where:
ΔHcond = enthalpy of condensation (in J/g or kJ/g)
Q = heat released or absorbed during condensation (in J or kJ)
m = mass of the substance (in g)
In the given question, we are provided with Q = 14.8 kJ and m = 1.6 g. We need to convert kJ to J before calculating ΔHcond.
1 kJ = 1000 J
So, first, we convert 14.8 kJ to J:
14.8 kJ × 1000 J/kJ = 14800 J
Now that we have Q in J and m in g, we can substitute these values into the formula:
ΔHcond = 14800 J / 1.6 g
Calculating the result:
ΔHcond = 9250 J/g
Therefore, the ΔHcond for HCl is 9250 J/g.
14.8J=1.6g*DeltaHv
DeltaHv=14.8/1.6 J/g
Hvapor=Hcondenstaon, but opposite signs