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Molar Mass of Solvent given Cryoscopic Constant Formula

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The Molar Mass of Solvent is the molar mass of the medium in which the solute is dissolved. Check FAQs

M solvent = \frac{k f \cdot 1000 \cdot ΔH fusion}{[R] \cdot T fp \cdot T fp}

M_solvent - Molar Mass of Solvent?k_f - Cryoscopic Constant?ΔH_fusion - Molar Enthalpy of Fusion?T_fp - Solvent Freezing Point?[R] - Universal gas constant?

Molar Mass of Solvent given Cryoscopic Constant Example

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Here is how the Molar Mass of Solvent given Cryoscopic Constant equation looks like with Values.

Here is how the Molar Mass of Solvent given Cryoscopic Constant equation looks like with Units.

Here is how the Molar Mass of Solvent given Cryoscopic Constant equation looks like.

1.4426 = \frac{6.65 \cdot 1000 \cdot 333.5}{8.3145 \cdot 430 \cdot 430}

1.4426kg = \frac{6.65K*kg/mol \cdot 1000 \cdot 333.5kJ/mol}{8.3145 \cdot 430K \cdot 430K}

1.4426 = \frac{6.65 \cdot 1000 \cdot 333.5}{8.3145 \cdot 430 \cdot 430}

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Depression in Freezing Point » fx Molar Mass of Solvent given Cryoscopic Constant

Molar Mass of Solvent given Cryoscopic Constant Solution

Follow our step by step solution on how to calculate Molar Mass of Solvent given Cryoscopic Constant?

FIRST Step Consider the formula

M solvent = \frac{k f \cdot 1000 \cdot ΔH fusion}{[R] \cdot T fp \cdot T fp}

Next Step Substitute values of Variables

∴

M solvent = \frac{6.65K*kg/mol \cdot 1000 \cdot 333.5kJ/mol}{[R] \cdot 430K \cdot 430K}

Next Step Substitute values of Constants

∴

M solvent = \frac{6.65K*kg/mol \cdot 1000 \cdot 333.5kJ/mol}{8.3145 \cdot 430K \cdot 430K}

Next Step Convert Units

∴

M solvent = \frac{6.65K*kg/mol \cdot 1000 \cdot 333500J/mol}{8.3145 \cdot 430K \cdot 430K}

Next Step Prepare to Evaluate

∴

M solvent = \frac{6.65 \cdot 1000 \cdot 333500}{8.3145 \cdot 430 \cdot 430}

Next Step Evaluate

∴

M solvent = 1.4426015262568kg

LAST Step Rounding Answer

∴

M solvent = 1.4426kg

Molar Mass of Solvent given Cryoscopic Constant Formula Elements

Variables

Constants

Molar Mass of Solvent

The Molar Mass of Solvent is the molar mass of the medium in which the solute is dissolved.

Symbol: M_solvent

Measurement: WeightUnit: kg

Note: Value can be positive or negative.

Formulas to find Molar Mass of Solvent

Cryoscopic Constant

The Cryoscopic Constant is described as the freezing point depression when a mole of non-volatile solute is dissolved in one kg of solvent.

Symbol: k_f

Measurement: Cryoscopic ConstantUnit: K*kg/mol

Note: Value should be greater than 0.

Formulas to find Cryoscopic Constant

Molar Enthalpy of Fusion

The Molar Enthalpy of Fusion is the amount of energy needed to change one mole of a substance from the solid phase to the liquid phase at constant temperature and pressure.

Symbol: ΔH_fusion

Measurement: Molar EnthalpyUnit: kJ/mol

Note: Value should be greater than 0.

Formulas to find Molar Enthalpy of Fusion

Solvent Freezing Point

Solvent Freezing Point is the temperature at which the solvent freezes from liquid to solid state.

Symbol: T_fp

Measurement: TemperatureUnit: K

Note: Value can be positive or negative.

Formulas to find Solvent Freezing Point

Universal gas constant

Universal gas constant is a fundamental physical constant that appears in the ideal gas law, relating the pressure, volume, and temperature of an ideal gas.

Symbol: [R]

Value: 8.31446261815324

Other formulas in Depression in Freezing Point category

Go Depression in Freezing Point of Solvent

ΔT f = k f \cdot m

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

ΔT f = i \cdot k f \cdot m

Go Molality given Depression in Freezing Point

m = \frac{ΔT f}{k f \cdot i}

Go Cryoscopic Constant given Molar Enthalpy of Fusion

k f = \frac{[R] \cdot T fp \cdot T fp \cdot M solvent}{1000 \cdot ΔH fusion}

How to Evaluate Molar Mass of Solvent given Cryoscopic Constant?

Molar Mass of Solvent given Cryoscopic Constant evaluator uses Molar Mass of Solvent = (Cryoscopic Constant*1000*Molar Enthalpy of Fusion)/([R]*Solvent Freezing Point*Solvent Freezing Point) to evaluate the Molar Mass of Solvent, The Molar Mass of solvent given Cryoscopic Constant is obtained by summing the molar masses of its component atoms. A cryoscopic constant is described as the freezing point depression when a mole of non-volatile solute is dissolved in one kg of solvent. Molar Mass of Solvent is denoted by M_solvent symbol.

How to evaluate Molar Mass of Solvent given Cryoscopic Constant using this online evaluator? To use this online evaluator for Molar Mass of Solvent given Cryoscopic Constant, enter Cryoscopic Constant (k_f), Molar Enthalpy of Fusion (ΔH_fusion) & Solvent Freezing Point (T_fp) and hit the calculate button.

FAQs on Molar Mass of Solvent given Cryoscopic Constant

What is the formula to find Molar Mass of Solvent given Cryoscopic Constant?

The formula of Molar Mass of Solvent given Cryoscopic Constant is expressed as Molar Mass of Solvent = (Cryoscopic Constant*1000*Molar Enthalpy of Fusion)/([R]*Solvent Freezing Point*Solvent Freezing Point). Here is an example- 0.401976 = (6.65*1000*333500)/([R]*430*430).

How to calculate Molar Mass of Solvent given Cryoscopic Constant?

With Cryoscopic Constant (k_f), Molar Enthalpy of Fusion (ΔH_fusion) & Solvent Freezing Point (T_fp) we can find Molar Mass of Solvent given Cryoscopic Constant using the formula - Molar Mass of Solvent = (Cryoscopic Constant*1000*Molar Enthalpy of Fusion)/([R]*Solvent Freezing Point*Solvent Freezing Point). This formula also uses Universal gas constant .

Can the Molar Mass of Solvent given Cryoscopic Constant be negative?

Yes, the Molar Mass of Solvent given Cryoscopic Constant, measured in Weight can be negative.

Which unit is used to measure Molar Mass of Solvent given Cryoscopic Constant?

Molar Mass of Solvent given Cryoscopic Constant is usually measured using the Kilogram[kg] for Weight. Gram[kg], Milligram[kg], Ton (Metric)[kg] are the few other units in which Molar Mass of Solvent given Cryoscopic Constant can be measured.

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