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What is the freezing of adding p-nitromethylbenzene to the freezing point of naphthalene?
When p-nitromethylbenzene is added to naphthalene, it can lower the freezing point of the solution due to colligative properties, specifically freezing point depression. The presence of p-nitromethylbenzene disrupts the orderly arrangement of naphthalene molecules as they freeze, requiring a lower temperature to achieve solidification. The extent of this freezing point depression depends on the concentration of p-nitromethylbenzene in the solution.
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What is the effect of adding p nitrotoluene to the freezing point of naphthalene?
Adding p-nitrotoluene to naphthalene will lower the freezing point of the mixture. This is due to the phenomenon of freezing point depression, where the presence of a solute lowers the freezing point of the solvent. The greater the concentration of the solute in the solvent, the lower the freezing point will be.
Why does the freezing point decrease when naphthalene is added in camphor?
When naphthalene is added to camphor, it disrupts the crystalline structure of camphor by interfering with the intermolecular forces between camphor molecules. This disruption causes the camphor molecules to have a harder time coming together in an organized manner for freezing, resulting in a decrease in the freezing point.
Does adding more solute to a solvent raise its freezing point lower its boiling point raise its boiling point or does not affect its boiling point?
Adding more solute to a solvent raises its boiling point and lowers its freezing point. This is known as boiling point elevation and freezing point depression. The presence of solute particles disrupts the organization of solvent molecules, making it more difficult for them to change phase.
Is there a difference between freezing point depression and freezing point?
This is simply because the evaporation enthalpy is bigger than the enthalpy of fusion. ΔTf = -Kf · m (m= molality) ΔTb = Kb · m (m= molality) what is important is that Kf is proportional to 1/Enthalpy of fusion and the sam is true for Kb (with enthalpy of evaporation)
What effect does adding a solute have on freezing point of a soultion?
Adding a solute to a solution lowers its freezing point, a phenomenon known as freezing point depression. This occurs because the solute particles disrupt the formation of a solid lattice structure in the solvent, requiring a lower temperature to achieve freezing. The extent of this depression depends on the concentration of the solute and the properties of the solvent. As a result, solutions freeze at temperatures lower than the pure solvent's freezing point.
What is the effect of adding p nitrotoluene to the freezing point of naphthalene?
Adding p-nitrotoluene to naphthalene will lower the freezing point of the mixture. This is due to the phenomenon of freezing point depression, where the presence of a solute lowers the freezing point of the solvent. The greater the concentration of the solute in the solvent, the lower the freezing point will be.
What does a Graph of melting point and freezing point of naphthalene look like?
The graph of the melting point and freezing point of naphthalene would show a plateau at the melting point, as the solid naphthalene transitions into the liquid phase, and a plateau at the freezing point, as the liquid naphthalene transitions back into the solid phase. The melting point and freezing point of naphthalene are the same at approximately 80 degrees Celsius.
Why does the freezing point decrease when naphthalene is added in camphor?
When naphthalene is added to camphor, it disrupts the crystalline structure of camphor by interfering with the intermolecular forces between camphor molecules. This disruption causes the camphor molecules to have a harder time coming together in an organized manner for freezing, resulting in a decrease in the freezing point.
What is the freezing point depression constant for naphthalene?
The freezing point depression constant for Naphthalene is 6.9 degrees Celsius/mhttp://en.wikipedia.org/wiki/Freezing-point_depression
What is the Hypothesis of the melting and freezing point of naphthalene?
The hypothesis for the melting and freezing point of naphthalene could be that the melting point of naphthalene will be higher than its freezing point due to the typical behavior of most substances where solids melt at higher temperatures than they freeze. The hypothesis may also include factors like the purity of the naphthalene sample affecting its melting and freezing points.
What happens to the temperature of naphthalene during melting?
Lab: Melting / Freezing Point of NaphthaleneObjective: In this lab, you will investigate the melting and freezing point of the substance, naphthalene (moth ball flakes). You will heat solid naphthalene and record temperature changes and examine the graph to determine the melting point of the substance. You will then cool naphthalene and record temperature changes in order to determine the Freezing point of the substance Part A: What happens to temperature as naphthalene melts?Objective: As heat is applied to liquid naphthalene, the temperature rises. As the temperature rises, the naphthalene will eventually start to melt. This lab experiment tries to answer the question: what happens to the temperature of naphthalene as it melts? In this lab, you will heat the liquid naphthalene, and record the temperature changes. You will graph the temperature changes before drawing any conclusions.Part B: Determining the freezing point of naphthaleneObjective: Freezing point is a characteristic property of matter. As heat is taken away from a liquid, the temperature of that liquid decreases as the substance begins to freeze. This lab experiment tries to answer the question: what is the freezing point of an unknown liquid (naphthalene)? In this lab, you will cool liquid naphthalene, and record the temperature changes. You will graph the temperature changes before drawing any conclusions.
What does adding antifreeze to water do?
It lowers the freezing point.
The freezing point of benzene is 5.5C What is the freezing point of a solution of 5.00 g of naphthalene C10H8 in 444g of benzene Kf of benzene 4.90Cm?
ΔTf = Kf * molality Molar mass of naphthalene = 128.17 g/mol Moles of naphthalene = 5.00 g / 128.17 g/mol = 0.039 mol Molality = moles of naphthalene / kg of solvent = 0.039 mol / 0.444 kg = 0.088 mol/kg ΔTf = 4.90°C/m * 0.088 mol/kg = 0.432°C Freezing point of benzene is 5.5°C, so the freezing point of the solution is 5.5°C - 0.432°C = 5.068°C.
The freezing point of water can be lowered by adding?
By adding any "foreign" molecules or ions. Such as if u add sugar or salt to water, it will lower the freezing point of water.
What is the boiling and freezing point when it is 1.92 mole of naphthalene C10H8 in 16.8 mole of chloroform?
The boiling point elevation and freezing point depression of a solution are colligative properties that depend on the molality of the solute particles. Given the information provided, you would need the constants for the boiling point elevation and freezing point depression of the solvent (chloroform) to calculate the new boiling and freezing points.
How does adding salt to water affect the temperature?
It does not affect the temperature of the water, but solutes raise the boiling point and lower the freezing point.
Does adding more solute to a solvent raise its freezing point lower its boiling point raise its boiling point or does not affect its boiling point?
Adding more solute to a solvent raises its boiling point and lowers its freezing point. This is known as boiling point elevation and freezing point depression. The presence of solute particles disrupts the organization of solvent molecules, making it more difficult for them to change phase.
