Compared to the freezing point of 1.0 M KCl(aq) at standard pressure, the freezing point of 1.0 M CaCl2(aq) at standard pressure is(1) lower
(2) higher
(3) the same
Answers
Answer : The correct option is, (1) lower
Explanation :
Formula used for lowering in freezing point :
where,
= change in freezing point
= freezing point constant
m = molality
i = Van't Hoff factor
According to the question, we conclude that the molality of the given solutions are the same. So, the freezing point depends only on the Van't Hoff factor.
Now we have to calculate the Van't Hoff factor for the given solutions.
(a) The dissociation of will be,
So, Van't Hoff factor = Number of solute particles = 1 + 1 = 2
(b) The dissociation of will be,
So, Van't Hoff factor = Number of solute particles = 1 + 2 = 3
The freezing point depends only on the Van't Hoff factor. That means higher the Van't Hoff factor, lower will be the freezing point and vice-versa.
Thus, compared to the freezing point of 1.0 M at standard pressure, the freezing point of 1.0 M
at standard pressure is lower.
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B. volume and temperature only
C. volume and pressure only
D. pressure, volume, and temperature
Answers
Answer:
The correct option is D
Explanation:
The combined gas law is a combination of the three gas laws; Boyle's law, Charles' law and Gay-Lussac's law. It describes the relationship of the product of the pressure, volume and temperature of a gas to a constant as shown in the formula below
P₁V₁/T₁ = P₂V₂/T₂
Where P₁ is the initial pressure
V₁ is the initial volume
T₁ is the initial temperature (in Kelvin)
P₂ is the final pressure
V₂ is the final volume
T₂ is the final temperature (in Kelvin)
Answer is volume and pressure only
B- The electrons spend more time around the oxygen atom because oxygen is more electronegative than hydrogen.
C- There is a partial positive charge on each hydrogen atom and two partial negative charges on the oxygen atom in a water molecule.
D- Attractions form between opposite partial charges.
Answers
Answer:- Water is an electronegative molecule.
Explanation:
A molecule cannot be electronegative. Rather the atoms in a molecule may be electronegative. This first statement does not account for the hydrogen bonding in water at all because it is incorrect. However, the other statements in the question sheds more light on the nature of hydrogen bonding in water molecule.
Final answer:
Options B, C, and D are correct explanations for why water molecules form hydrogen bonds.
Explanation:
The correct option that does not help to explain why water molecules form hydrogen bonds is A- Water is an electronegative molecule. Hydrogen bonds form between a hydrogen atom in one water molecule and an electronegative atom, such as oxygen or nitrogen, in another water molecule. This attraction occurs because the electronegative atom pulls the shared electrons closer to itself, creating a partial positive charge on the hydrogen atom. The presence of partial positive and negative charges on the molecule is crucial for hydrogen bond formation. Therefore, options B, C, and D all contribute to explaining why water molecules form hydrogen bonds.
Learn more about Hydrogen bonds here:
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A) NaCl + AgNO3 - NaNO3 + AgCl
Answers
Answer:
chemical equation balance.
Explanation:
if you need more explanation , comment.
Answers
How many moles of NH3 can be produced from 13.5mol of H2 and excess N2??
9 moles NH3
4.5 × 10^-4.
Answers
Initial concentration = 0.311
C = -x,x,x
E = 0.311-x,x,x
KNO2 ====>K+ + NO2-
Initial concentration = 0.189
C= -0.189,0.189,0.189
E = 0,0.189,0.189