Consider the solutions, 0.04 m urea [(NH2)2C=O)], 0.04 m AgNO3 and 0.04 m CaCl2. Which has (i) the highest osmotic pressure, (ii) the lowest vapor pressure, (iii) the highest boiling point?
Answers
Answer:
i) Highest osmotic pressure: CaCl2
ii) lower vapor pressure : CaCl2
iii) highest boiling point : CaCl2
Explanation:
The colligative properties depend upon the number of solute particles in a solution.
The following four are the colligative properties:
a) osmotic pressure : more the concentration of the solute, more the osmotic pressure
b) vapor pressure: more the concentration of the solute, lesser the vapor pressure.
c) elevation in boiling point: more the concentration of the solute, more the boiling point.
d) depression in freezing point: more the concentration of the solute, lesser the freezing point.
the number of particle produced by urea = 1
the number of particle produced by AgNO3 = 2
the number of particle produced by CaCl2 = 3
As concentrations are same, CaCl2 will have more number of solute particles and urea will have least
i) Highest osmotic pressure: CaCl2
ii) lower vapor pressure : CaCl2
iii) highest boiling point : CaCl2
Final answer:
The solution with the highest number of particles in solution (CaCl2 in this case), experiences the highest osmotic pressure, lowest vapor pressure and highest boiling point due to the principles of colligative properties.
Explanation:
The question pertains to the colligative properties of solutions, which would be governed by the number of particles in the solution. The solutions are 0.04 m urea [(NH2)2C=O)], 0.04 m AgNO3, and 0.04 m CaCl2. For (i) Highest osmotic pressure, the solution with the highest ion count would yield the highest osmotic pressure. CaCl2 dissociates into three ions (Ca²+, and 2 Cl¯), therefore, it would exhibit the highest osmotic pressure. For (ii) Lowest vapor pressure, this would coincide with the solution with the highest osmotic pressure, again making it CaCl2, due to the greatest decrease in vapor pressure. For (iii) the highest boiling point, this too would be CaCl2 for the reasons stated above. The presence of more particles in a solution interferes more with the evaporation process, requiring more energy (higher temperature) to achieve boiling.
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Answers
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Learn more: brainly.com/question/284565
Answers
Answer : The value of of the reaction is, 480.29 KJ.
Explanation :
Formula used :
where,
= internal energy of the reaction = ?
= enthalpy of the reaction = 483.6 KJ/mole = 483600 J
= change in the moles of the reaction = Moles of product - Moles of reactant = 3 - 2 = 1 mole
R = gas constant = 8.314 J/mole.K
T = temperature =
Now put all the given values in the above formula, we get:
Therefore, the value of of the reaction is, 480.29 KJ.
2 H2O(g) → 2 H2(g) + O2(g)
You can see that there are 2 moles of gas in the reactants and 3 moles of gas in the products.
1 moles of ideal gas occupies the same volume as 1 mole of any other ideal gas under the same conditions of temp and pressure.
Since it is done under constant temp and pressure that means the volume change will be equal to the volume of 1 mole of gas
2 moles reacts to form 3 moles
The gas equation is
PV = nRT
P = pressure
V = volume (unknown)
n = moles (1)
R = gas constant = 8.314 J K^-1 mol^-1
- the gas constant is different for different units of temp and pressure (see wikki link) in this case temp and pressure are constant, and we want to put the result in an equation that has Joules in it, so we select 8.314 JK^-1mol^-1)
T = temp in Kelvin (kelvin = deg C + 273.15
So T = 403.15 K
Now, you can see that PV is on one side of the equation, and we are looking to put PdV in our dE equation. So we can say
dE = dH -dnRT (because PV = nRT)
Also, since the gas constant is in the unit of Joules, we need to convert dH to Joules
dH = 483.6 kJ/mol = 483600 Joules/mol
dE = 483600 J/mol - (1.0 mol x 8.314 J mol^-1K-1 x 403.15 K)
dE = 483600 J/mol - 3351.77 J
dE = 480248.23 J/mol
dE = 480.2 kJ/mol
Answers
Answer:
The correct answer is B) the C=O bond is polar; the O atom bears a partial negative charge.
Explanation:
In a C=O bond, the oxygen (O) atom is more electronegative than the carbon (C) atom. Electronegativity is the ability of an atom to attract electrons towards itself in a chemical bond. Oxygen has a higher electronegativity than carbon, so it pulls the shared electrons in the C=O bond closer to itself.
As a result, the oxygen atom gains a partial negative charge (δ-) because it has a higher electron density around it, while the carbon atom gains a partial positive charge (δ+) because it has less electron density around it.
This uneven distribution of electron density in the C=O bond leads to polarity, making the bond polar. The oxygen atom, being more electronegative, attracts the shared electrons more strongly, creating a partial negative charge on the oxygen atom and a partial positive charge on the carbon atom.
In summary, the C=O bond is polar, and the oxygen atom bears a partial negative charge (δ-).
B. Ionic solids have higher melting points than molecular solids.
C. Molecular solids have higher melting points than all other types of solids.
D. It is impossible for solids to melt; therefore solids do not have melting points.
Answers
This is because the rest are false, as solids are able to melt, and do have melting points. Also, not all solids have the same melting points.
8.71 x 10^-4
8.71 x 10^-7
8.71 x 10^-10
Answers
E=mc^2
plug the values,
The amount of mass in kilograms would be lost is 8.71 x 10^-10
Answer : The mass lost would be,
Solution : Given,
Energy released =
Speed of light 'c' =
Formula used :
where,
E = energy
m = mass
c = speed of light
Now put all the given values in the above formula, we get
Therefore, the mass lost would be,