Cryoscopic Constant given Latent Heat of Fusion Calculator

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Depression in Freezing Point

Clausius-Clapeyron Equation

Elevation in Boiling Point

Gibb's Phase Rule

Immiscible Liquids

Important Formulas of Clausius-Clapeyron Equation

Important Formulas of Colligative Properties

Osmotic Pressure

Relative Lowering of Vapour Pressure

Van't Hoff Factor

✖Solvent Freezing Point for Cryoscopic Constant is the temperature at which the solvent freezes from liquid to solid state.ⓘ Solvent Freezing Point for Cryoscopic Constant [T_f]			+10% -10%
✖The Latent Heat of Fusion is the amount of heat required to convert one unit amount of substance from the solid phase to the liquid phase — leaving the temperature of the system unaltered.ⓘ Latent Heat of Fusion [L_fusion]			+10% -10%

✖The Cryoscopic Constant is described as the freezing point depression when a mole of non-volatile solute is dissolved in one kg of solvent.ⓘ Cryoscopic Constant given Latent Heat of Fusion [k_f]

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Formula

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Cryoscopic Constant given Latent Heat of Fusion

Formula

`"k"_{"f"} = ("[R]"*"T"_{"f"}^2)/(1000*"L"_{"fusion"})`

Example

`"6.2234K*kg/mol"=("[R]"*("500K")^2)/(1000*"334J/kg")`

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Cryoscopic Constant given Latent Heat of Fusion Solution

STEP 0: Pre-Calculation Summary

Formula Used

Cryoscopic Constant = ([R]*Solvent Freezing Point for Cryoscopic Constant^2)/(1000*Latent Heat of Fusion)
k_f = ([R]*T_f^2)/(1000*L_fusion)
This formula uses 1 Constants, 3 Variables

Constants Used

[R] - Universal gas constant Value Taken As 8.31446261815324

Variables Used

Cryoscopic Constant - (Measured in Kelvin Kilogram per Mole) - The Cryoscopic Constant is described as the freezing point depression when a mole of non-volatile solute is dissolved in one kg of solvent.
Solvent Freezing Point for Cryoscopic Constant - (Measured in Kelvin) - Solvent Freezing Point for Cryoscopic Constant is the temperature at which the solvent freezes from liquid to solid state.
Latent Heat of Fusion - (Measured in Joule per Kilogram) - The Latent Heat of Fusion is the amount of heat required to convert one unit amount of substance from the solid phase to the liquid phase — leaving the temperature of the system unaltered.

STEP 1: Convert Input(s) to Base Unit

Solvent Freezing Point for Cryoscopic Constant: 500 Kelvin --> 500 Kelvin No Conversion Required
Latent Heat of Fusion: 334 Joule per Kilogram --> 334 Joule per Kilogram No Conversion Required

STEP 2: Evaluate Formula

Substituting Input Values in Formula

k_f = ([R]*T_f^2)/(1000*L_fusion) --> ([R]*500^2)/(1000*334)

Evaluating ... ...

k_f = 6.22340016328835

STEP 3: Convert Result to Output's Unit

6.22340016328835 Kelvin Kilogram per Mole --> No Conversion Required

FINAL ANSWER

6.22340016328835 ≈ 6.2234 Kelvin Kilogram per Mole <-- Cryoscopic Constant

(Calculation completed in 00.004 seconds)

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< 23 Depression in Freezing Point Calculators

Depression in Freezing Point given Vapour Pressure

Go Depression in Freezing Point = ((Vapour Pressure of Pure Solvent-Vapour Pressure of Solvent in Solution)*[R]*(Solvent Freezing Point^2))/(Vapour Pressure of Pure Solvent*Molar Enthalpy of Fusion)

Depression in Freezing Point given Elevation in Boiling Point

Go Depression in Freezing Point = (Molar Enthalpy of Vaporization*Elevation in Boiling Point*(Solvent Freezing Point^2))/(Molar Enthalpy of Fusion*(Solvent Boiling Point^2))

Relative Lowering of Vapour Pressure given Depression in Freezing Point

Go Relative Lowering of Vapour Pressure = (Molar Enthalpy of Fusion*Depression in Freezing Point)/([R]*Solvent Freezing Point*Solvent Freezing Point)

Molar Enthalpy of Fusion given Freezing point of solvent

Go Molar Enthalpy of Fusion = ([R]*Solvent Freezing Point*Solvent Freezing Point*Molar Mass of Solvent)/(1000*Cryoscopic Constant)

Cryoscopic Constant given Molar Enthalpy of Fusion

Go Cryoscopic Constant = ([R]*Solvent Freezing Point*Solvent Freezing Point*Molar Mass of Solvent)/(1000*Molar Enthalpy of Fusion)

Molar Mass of Solvent given Cryoscopic Constant

Go Molar Mass of Solvent = (Cryoscopic Constant*1000*Molar Enthalpy of Fusion)/([R]*Solvent Freezing Point*Solvent Freezing Point)

Depression in Freezing Point given Osmotic Pressure

Go Depression in Freezing Point = (Osmotic Pressure*Molar Volume*(Solvent Freezing Point^2))/(Temperature*Molar Enthalpy of Fusion)

Solvent Freezing Point given Molal Freezing Point Lowering Constant

Go Solvent Freezing Point = sqrt((Molal freezing point constant*Molal Heat of Fusion*1000)/([R]*Molecular Weight))

Freezing Point of Solvent given Cryoscopic Constant and Molar Enthalpy of Fusion

Go Solvent Freezing Point = sqrt((Cryoscopic Constant*1000*Molar Enthalpy of Fusion)/([R]*Molar Mass of Solvent))

Depression in Freezing Point given Relative Lowering of Vapour Pressure

Go Depression in Freezing Point = (Relative Lowering of Vapour Pressure*[R]*(Solvent Freezing Point^2))/Molar Enthalpy of Fusion

Solvent Molecular Weight given Molal Freezing Point Lowering Constant

Go Solvent Molecular Weight = (Molal freezing point constant*Molal Heat of Fusion*1000)/([R]*(Solvent Freezing Point^2))

Molal Freezing Point Lowering Constant

Go Molal freezing point constant = ([R]*(Solvent Freezing Point^2)*Molecular Weight)/(Molal Heat of Fusion*1000)

Latent Heat of Fusion given Freezing Point of Solvent

Go Latent Heat of Fusion = ([R]*Solvent Freezing Point*Solvent Freezing Point)/(1000*Cryoscopic Constant)

Freezing Point of Solvent given Cryoscopic Constant and Latent Heat of Fusion

Go Solvent Freezing Point = sqrt((Cryoscopic Constant*1000*Latent Heat of Fusion)/[R])

Cryoscopic Constant given Latent Heat of Fusion

Go Cryoscopic Constant = ([R]*Solvent Freezing Point for Cryoscopic Constant^2)/(1000*Latent Heat of Fusion)

Van't Hoff Factor of Electrolyte given Depression in Freezing Point

Go Van't Hoff Factor = Depression in Freezing Point/(Cryoscopic Constant*Molality)

Cryoscopic Constant given Depression in Freezing Point

Go Cryoscopic Constant = Depression in Freezing Point/(Van't Hoff Factor*Molality)

Molality given Depression in Freezing Point

Go Molality = Depression in Freezing Point/(Cryoscopic Constant*Van't Hoff Factor)

Van't Hoff equation for Depression in Freezing Point of electrolyte

Go Depression in Freezing Point = Van't Hoff Factor*Cryoscopic Constant*Molality

Molal Freezing Point Constant given Freezing Point Depression

Go Molal freezing point constant = Depression in Freezing Point/Molality

Molality given Freezing Point Depression

Go Molality = Depression in Freezing Point/Molal freezing point constant

Depression in Freezing Point of Solvent

Go Depression in Freezing Point = Cryoscopic Constant*Molality

Freezing Point Depression

Go Depression in Freezing Point = Cryoscopic Constant*Molality

< 22 Important Formulas of Colligative Properties Calculators

Van't Hoff Osmotic Pressure for Mixture of Two Solutions

Go Osmotic Pressure = ((Van't Hoff Factor of Particle 1*Concentration of Particle 1)+(Van't Hoff Factor of Particle 2*Concentration of Particle 2))*[R]*Temperature

Osmotic Pressure given Vapour Pressure

Go Osmotic Pressure = ((Vapour Pressure of Pure Solvent-Vapour Pressure of Solvent in Solution)*[R]*Temperature)/(Molar Volume*Vapour Pressure of Pure Solvent)

Osmotic Pressure given Depression in Freezing Point

Go Osmotic Pressure = (Molar Enthalpy of Fusion*Depression in Freezing Point*Temperature)/(Molar Volume*(Solvent Freezing Point^2))

Relative Lowering of Vapour Pressure

Go Relative Lowering of Vapour Pressure = (Vapour Pressure of Pure Solvent-Vapour Pressure of Solvent in Solution)/Vapour Pressure of Pure Solvent

Van't Hoff Osmotic Pressure for Electrolyte

Go Osmotic Pressure = Van't Hoff Factor*Molar Concentration of Solute*Universal Gas Constant*Temperature

Ebullioscopic Constant using Latent Heat of Vaporization

Go Ebullioscopic Constant of Solvent = ([R]*Solvent BP given Latent Heat of Vaporization^2)/(1000*Latent Heat of Vaporization)

Osmotic Pressure given Concentration of Two Substances

Go Osmotic Pressure = (Concentration of Particle 1+Concentration of Particle 2)*[R]*Temperature

Ostwald-Walker Dynamic Method for Relative Lowering of Vapour Pressure

Go Relative Lowering of Vapour Pressure = Loss of Mass in Bulb Set B/(Loss of Mass in bulb set A+Loss of Mass in Bulb Set B)

Relative Lowering of Vapour Pressure given Number of Moles for Concentrated Solution

Go Relative Lowering of Vapour Pressure = Number of Moles of Solute/(Number of Moles of Solute+Number of Moles of Solvent)

Osmotic Pressure given Relative Lowering of Vapour Pressure

Go Osmotic Pressure = (Relative Lowering of Vapour Pressure*[R]*Temperature)/Molar Volume

Cryoscopic Constant given Latent Heat of Fusion

Go Cryoscopic Constant = ([R]*Solvent Freezing Point for Cryoscopic Constant^2)/(1000*Latent Heat of Fusion)

Van't Hoff Relative Lowering of Vapour Pressure given Molecular Mass and Molality

Go Colligative Pressure given Van't Hoff factor = (Van't Hoff Factor*Molality*Molecular Mass Solvent)/1000

Ebullioscopic Constant given Elevation in Boiling Point

Go Ebullioscopic Constant of Solvent = Boiling Point Elevation/(Van't Hoff Factor*Molality)

Van't Hoff Equation for Elevation in Boiling Point of Electrolyte

Go Boiling Point Elevation = Van't Hoff Factor*Ebullioscopic Constant of Solvent*Molality

Cryoscopic Constant given Depression in Freezing Point

Go Cryoscopic Constant = Depression in Freezing Point/(Van't Hoff Factor*Molality)

Van't Hoff equation for Depression in Freezing Point of electrolyte

Go Depression in Freezing Point = Van't Hoff Factor*Cryoscopic Constant*Molality

Total Concentration of Particles using Osmotic Pressure

Go Molar Concentration of Solute = Osmotic Pressure/([R]*Temperature)

Osmotic Pressure for Non Electrolyte

Go Osmotic Pressure = Molar Concentration of Solute*[R]*Temperature

Osmotic Pressure given Density of Solution

Go Osmotic Pressure = Density of Solution*[g]*Equilibrium Height

Relative Lowering of Vapour Pressure given Number of Moles for Dilute Solution

Go Relative Lowering of Vapour Pressure = Number of Moles of Solute/Number of Moles of Solvent

Boiling Point Elevation

Go Boiling Point Elevation = Molal Boiling Point Elevation Constant*Molality

Freezing Point Depression

Go Depression in Freezing Point = Cryoscopic Constant*Molality

Cryoscopic Constant given Latent Heat of Fusion Formula

Cryoscopic Constant = ([R]*Solvent Freezing Point for Cryoscopic Constant^2)/(1000*Latent Heat of Fusion)
k_f = ([R]*T_f^2)/(1000*L_fusion)

What is Latent Heat of Fusion?

The latent heat of fusion is the enthalpy change of any amount of substance when it melts. When the heat of fusion is referenced to a unit of mass, it is usually called the specific heat of fusion, while the molar heat of fusion refers to the enthalpy change per amount of substance in moles.

How to Calculate Cryoscopic Constant given Latent Heat of Fusion?

Cryoscopic Constant given Latent Heat of Fusion calculator uses Cryoscopic Constant = ([R]*Solvent Freezing Point for Cryoscopic Constant^2)/(1000*Latent Heat of Fusion) to calculate the Cryoscopic Constant, The Cryoscopic Constant given Latent Heat of Fusion is described as the freezing point depression when a mole of non-volatile solute is dissolved in one kg of solvent. The cryoscopic constant is denoted by kf. Cryoscopic Constant is denoted by k_f symbol.

How to calculate Cryoscopic Constant given Latent Heat of Fusion using this online calculator? To use this online calculator for Cryoscopic Constant given Latent Heat of Fusion, enter Solvent Freezing Point for Cryoscopic Constant (T_f) & Latent Heat of Fusion (L_fusion) and hit the calculate button. Here is how the Cryoscopic Constant given Latent Heat of Fusion calculation can be explained with given input values -> 6.2234 = ([R]*500^2)/(1000*334).

FAQ

What is Cryoscopic Constant given Latent Heat of Fusion?

The Cryoscopic Constant given Latent Heat of Fusion is described as the freezing point depression when a mole of non-volatile solute is dissolved in one kg of solvent. The cryoscopic constant is denoted by kf and is represented as k_f = ([R]*T_f^2)/(1000*L_fusion) or Cryoscopic Constant = ([R]*Solvent Freezing Point for Cryoscopic Constant^2)/(1000*Latent Heat of Fusion). Solvent Freezing Point for Cryoscopic Constant is the temperature at which the solvent freezes from liquid to solid state & The Latent Heat of Fusion is the amount of heat required to convert one unit amount of substance from the solid phase to the liquid phase — leaving the temperature of the system unaltered.

How to calculate Cryoscopic Constant given Latent Heat of Fusion?

The Cryoscopic Constant given Latent Heat of Fusion is described as the freezing point depression when a mole of non-volatile solute is dissolved in one kg of solvent. The cryoscopic constant is denoted by kf is calculated using Cryoscopic Constant = ([R]*Solvent Freezing Point for Cryoscopic Constant^2)/(1000*Latent Heat of Fusion). To calculate Cryoscopic Constant given Latent Heat of Fusion, you need Solvent Freezing Point for Cryoscopic Constant (T_f) & Latent Heat of Fusion (L_fusion). With our tool, you need to enter the respective value for Solvent Freezing Point for Cryoscopic Constant & Latent Heat of Fusion and hit the calculate button. You can also select the units (if any) for Input(s) and the Output as well.

How many ways are there to calculate Cryoscopic Constant?

In this formula, Cryoscopic Constant uses Solvent Freezing Point for Cryoscopic Constant & Latent Heat of Fusion. We can use 3 other way(s) to calculate the same, which is/are as follows -

Cryoscopic Constant = ([R]*Solvent Freezing Point*Solvent Freezing Point*Molar Mass of Solvent)/(1000*Molar Enthalpy of Fusion)
Cryoscopic Constant = Depression in Freezing Point/(Van't Hoff Factor*Molality)
Cryoscopic Constant = Depression in Freezing Point/(Van't Hoff Factor*Molality)

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