Answer:
95.54mL
Explanation:
To calculate the volume that would have that mass, what is needed to be done is to use the formula that relates mass, density and volume.
Mathematically,
mass = density * Volume
But in this particular question we are to calculate the volume, we already have the mass and the density.
Rearranging the equation gives the following:
volume = mass/density
Our mass here is 75.0g while our density is 0.785g/mL
Hence, volume = 75/0.785 = 95.54mL
Explanation:
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Explanation:
It is known that the maximum value of ml is equal to the vale of l. But the minimum value of n is as follows.
n = l + 1
where, n = principle quantum number
l = azimuthal quantum number
Values of n can be 1, 2, 3, 4 and so on. Whereas the values of l can be 0, 1, 2, 3, and so on.
Also, "m" is known as magnetic quantum number whose values can be equal to -l and +l.
So, when n = 1 then l = 0 and m = 0.
When n = 2 then l = 1 and values of m will be equal to -1, 0, +1. As it is given that the magnetic quantum number ml = -1. Hence, it is only possible when n = 2.
Thus, we can conclude that the smallest possible value of the principal quantum number n of the state is 2.
<u>Answer:</u> The final temperature will be 
<u>Explanation:</u>
Calculating the heat released or absorbed for the process:
In a system, the total amount of heat released is equal to the total amount of heat absorbed.
OR
......(1)
where,
C = heat capacity of water = 
= mass of water of sample 1 = 100.0 g
= mass of water of sample 2 = 71.0 g
= final temperature of the system = ?
= initial temperature of water of sample 1 = 
= initial temperature of the water of sample 2 = 
Putting values in equation 1, we get:
Hence, the final temperature will be
Answer:
Option 1 is correct.
ΔH for the condensation of 1 kg of Acetone is - 501 KJ.
Explanation:
Molar mass of acetone = 58.08 g/mol
Number of moles of acetone that condenses = mass/molar mass = 1000/58.08 = 17.22 moles
1 mole of Acetone vaporizer with an enthalpy change of 29.1 KJ.
1 mole of Acetone will condense with an enthalpy change of - 29.1 KJ (since condensation is the exact reverse of vaporization)
That is, vaporization is given by,
Acetone(l) ----> Acetone(g) ΔH = 29.1 KJ
Then condensation will be given by,
Acetone(g) ----> Acetone(l) ΔH = -29.1 KJ
So,
1 mole of Acetone will condense with an enthalpy change of - 29.1 KJ
17.22 moles of Acetone will condense with an enthalpy change of 17.22 × - 29.1 KJ = - 501 KJ.
The first option is correct.
