The amount of stearic acid (in grams), required to add in the given amount of acetone to prepare a solution having given vapor pressure, is to be calculated. Concept Introduction: The Raoult’s law gives the relationship between the partial vapor pressure of solution and solvent. This law states that the partial pressure of the solvent in the solution ( P 1 ) is equivalent to the product of mole fraction of the solvent ( χ 1 ) , and to the partial pressure of pure solvent ( P 1 ° ) . It is expressed as follows: P 1 = χ 1 P 1 ° Mole fraction of a component is defined as the ratio between the number of moles of that component and the sum of number of moles of all the components present in the mixture. The relationship between mole fraction ( χ ) and moles ( n ) of component is as follows: χ 1 = n 1 n 1 + n 2 + ....
The amount of stearic acid (in grams), required to add in the given amount of acetone to prepare a solution having given vapor pressure, is to be calculated. Concept Introduction: The Raoult’s law gives the relationship between the partial vapor pressure of solution and solvent. This law states that the partial pressure of the solvent in the solution ( P 1 ) is equivalent to the product of mole fraction of the solvent ( χ 1 ) , and to the partial pressure of pure solvent ( P 1 ° ) . It is expressed as follows: P 1 = χ 1 P 1 ° Mole fraction of a component is defined as the ratio between the number of moles of that component and the sum of number of moles of all the components present in the mixture. The relationship between mole fraction ( χ ) and moles ( n ) of component is as follows: χ 1 = n 1 n 1 + n 2 + ....
Solution Summary: The author explains the Raoult's law, which gives the relationship between the partial vapor pressure of solution and solvent.
The amount of stearic acid (in grams), required to add in the given amount of acetone to prepare a solution having given vapor pressure, is to be calculated.
Concept Introduction:
The Raoult’s law gives the relationship between the partial vapor pressure of solution and solvent. This law states that the partial pressure of the solvent in the solution (P1) is equivalent to the product of mole fraction of the solvent (χ1), and to the partial pressure of pure solvent (P1°). It is expressed as follows:
P1=χ1P1°
Mole fraction of a component is defined as the ratio between the number of moles of that component and the sum of number of moles of all the components present in the mixture. The relationship between mole fraction (χ) and moles (n) of component is as follows:
(ME EX1) Prblm #9/10
Can you explain in detail (step by step) I'm so confused with these problems. For turmber 13 can u turn them into lewis dot structures so I can better understand because, and then as well explain the resonance structure part. Thanks for the help.
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