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.
First, note the correct spelling of chemistry. Second, I don't know what "it" is. Third, what about just typing in the problem and we can go from there.
It seems like you are trying to calculate the amount of heat required to vaporize a substance. However, the calculations you have shown are incorrect. Let me guide you through the correct steps to obtain the answer.
First, you correctly found the mass of the substance:
60.0 mL / 1.00 g/mL = 60.0 grams
Next, to find the number of moles, we need to divide the mass by the molar mass. Assuming you are referring to a specific substance, it would be helpful to know the name or formula of the substance. However, for the purpose of this explanation, let's assume you are referring to water (H2O). The molar mass of water is approximately 18 g/mol. Therefore:
60.0 grams / 18 g/mol ≈ 3.33 moles
Now let's assume you are given the heat of vaporization for water as 40.7 kJ/mol. To calculate the total heat required to vaporize the substance, we multiply the number of moles by the heat of vaporization:
3.33 moles × 40.7 kJ/mol = 135.231 kJ
So, the correct answer is approximately 135.231 kJ of heat required to vaporize the given amount of substance.
Please note that these values and calculations are specific to water (H2O), and if you are dealing with a different substance, you would need to adjust the molar mass and heat of vaporization accordingly.