1) Given the following “substances” and their normal boiling points, in celsius.
G:43.8 Celsius J:93.7 M:56.7
T: 83.5 R:63.6
Which set below correctly lists some of these liquids in order of increasing intermolecular forces at 20 oC?
a) G < R < J
b) J < T < R
c) R < T < G
d) G < J < M
e) J < R < M
I am not sure how to figure this out. Would the smallest temperature be the biggest?
I recommend you list these in increasing boiling point, then look at a and see if that satisfies the criteria.
To determine the order of increasing intermolecular forces, we need to understand the relationship between intermolecular forces and boiling points.
Generally, substances with stronger intermolecular forces have higher boiling points. Intermolecular forces can include van der Waals forces (London dispersion forces, dipole-dipole interactions) and hydrogen bonding.
In this case, we have the boiling points of different substances. To analyze the order of increasing intermolecular forces, we need to consider their relative boiling points: the higher the boiling point, the stronger the intermolecular forces.
Comparing the boiling points:
G: 43.8 °C
J: 93.7 °C
M: 56.7 °C
T: 83.5 °C
R: 63.6 °C
Let's analyze the options:
a) G < R < J: According to the boiling points, this option is incorrect because J has a higher boiling point than R.
b) J < T < R: According to the boiling points, this option is incorrect because J has a higher boiling point than both T and R.
c) R < T < G: According to the boiling points, this option is incorrect because R has a higher boiling point than both T and G.
d) G < J < M: According to the boiling points, this option is incorrect because M has a lower boiling point than G and J.
e) J < R < M: According to the boiling points, this option is correct because J has a higher boiling point than R, and R has a higher boiling point than M.
Therefore, the correct answer is option e) J < R < M.