How much heat (in kJ}) is required to vaporize it? (Assume a density of 1.00 g/mL )
I have this
60.0ML/ 1.00 g/ml = 60grams
60/153/81 g/mol = .3900916715 moles
.3900916715 moles / 43.9 kj/mol = 17.122
And it keeps telling me the answer is wrong.
See my response to your first post below.
To find the amount of heat required to vaporize a substance, you need to use the formula:
Q = m * ΔHv
Where:
Q is the heat required (in kJ)
m is the mass of the substance (in grams)
ΔHv is the molar heat of vaporization (in kJ/mol)
Let's go through the calculation step by step:
1. First, you correctly determined the mass of the substance:
60.0 mL / 1.00 g/mL = 60 g
2. However, your subsequent calculations have a mistake. The number you divided by, 43.9 kJ/mol, shouldn't be used because it seems unrelated to determining the molar heat of vaporization.
To rectify this, you'll need to find the molar mass of the substance and look up the molar heat of vaporization from a reliable source such as a reference book or online database.
Once you have the correct molar heat of vaporization, you can continue with the calculation:
3. Determine the molar mass of the substance (in g/mol).
For example, let's say the molar mass is 50 g/mol (just a hypothetical value for illustration).
4. Calculate the moles of the substance.
60 g / 50 g/mol = 1.2 moles
5. Use the given molar heat of vaporization to calculate the heat required.
Assuming the molar heat of vaporization is 30 kJ/mol (again, just a hypothetical value), the calculation would be:
Q = 1.2 moles * 30 kJ/mol = 36 kJ
Remember to plug in the actual molar heat of vaporization value for an accurate result.
I hope this helps you calculate the correct answer!