Mole Fraction

Now, the concept of the mole fraction, which is represented by the variable X, represents the mold component divided by your total moles. Now, more component itself represents the element or compound. Who's more fraction You must determine taking this information. We now have our mole fraction formula. So mole fraction again, which is X equals your mole component. So what, they're asking to find the mole fraction off divided by your total moles. Now that we know the formula for mole fraction, continue on to the next video and let's take a look at an example question.

The apparatus shown consists of three temperature-jacketed 1.000-L bulbs connected by stopcocks. Bulb A contains a mixture of H2O1g2, CO21g2, and N21g2 at 25 °C and a total pressure of 564 mm Hg. Bulb B is empty and is held at a temperature of -70 °C. Bulb C is also empty and is held at a temperature of 190 °C. The stopcocks are closed, and the volume of the lines connecting the bulbs is zero. CO2 sublimes at -78 °C, and N2 boils at -196 °C.
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/2673e3fdd6f54e4a-1669404097243.jpg" alt="" />
(a) The stopcock between A and B is opened, and the system is allowed to come to equilibrium. The pressure in A and B is now 219 mm Hg. What do bulbs A and B contain?

Mole Fraction Example 1

in this example question. It says we have 25 g of decorum methane, which is ch two c l two, and it's dissolved in 125 g of water. They say here, what is the mole fraction of diet cola methane. So we're gonna start out with step one and step one. We have to convert all the masses given to us in two moles. Now, to avoid rounding errors, make sure you have at least four decimal places. When you convert two moles, we're gonna take the 25 g of declawed methane, and we're gonna say it's composed of one carbon to hydrogen and two Korans looking up their atomic masses from the periodic table and adding them. Together we get a combined mass of 84.926 g of ch two c l two for every one mole. So here the grams, cancel out and then I'll get 0.2944 moles, our diet cola, methane. Now take the 125 g of water. At this point, we've seen water so many times you know that the mass of two hydrogen and one oxygen is 18.16 g for every one mole of water. So again, our grants cancel out. And now we're gonna have 6.9383 moles for water. Step two, we're not gonna place the mole component as the numerator off the mole fraction formula. Remember the mole fraction off? The more component is based on who were asked to find the mole fraction off and were asked to find a little fraction of dick low methane. So we're going to stay here. Mole fraction equals the moles of declawed methane and then determine the total value of moles added together and place it as the denominator off the mole fraction formula. So here we're going to take the 0.2944 moles of dicho methane plus the moles of the water. And that will give you my total moles, which is 7.23 to 7. So those moles here go on the bottom. So again, this is our total moles from adding up the moles of declare methane and water together. Now, this is important. Your final answer should have no units because mole fraction is a unit list expression that makes sense because the moles here would cancel out. So when we do that, we'll get as our final answer point 04070 as our mole fraction. This has four sig figs, Just like 40.2944 moles had four sig figs. So this is all we need to do when it comes to the mole fraction formula. Just remember who you're more component is. It's based on who you need to determine the mole fraction for if you know that, that goes as you numerator and then just total moles on the bottom as a denominator and you'll get your mole fraction at the end.

(a) What are the mole fractions of H2 in a
mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?

How to Calculate Mole Fraction Examples, Explanation, Shortcut, Equation, Practice Problems

Fluorocarbons (compounds that contain both carbon
and fluorine) were, until recently, used as refrigerants.
The compounds listed in the following table are all gases
at 25 °C, and their solubilities in water at 25 °C and 1
atm fluorocarbon pressure are given as mass percentages.
(c) Infants born with severe respiratory problems are sometimes given liquid ventilation: They breathe a liquid that
can dissolve more oxygen than air can hold. One of these
liquids is a fluorinated compound, CF3(CF2)7Br. The solubility of oxygen in this liquid is 66 mL O2 per 100 mL liquid. In contrast, air is 21% oxygen by volume. Calculate the
moles of O
2 present in an infant’s lungs (volume: 15 mL)
if the infant takes a full breath of air compared to taking
a full “breath” of a saturated solution of O
2 in the fluorinated liquid. Assume a pressure of 1 atm in the lungs.
Fluorocarbon Solubility (mass %)
CF4 0.0015
CClF3 0.009
CCl2F2 0.028
CHClF2 0.30

How to Find the Mole Fraction of a Gas

The atmospheric concentration of CO2 gas is presently
407 ppm (parts per million, by volume; that is, 407 L of every
106 L of the atmosphere are CO2). What is the mole fraction
of CO2 in the atmosphere?

(a) What are the mole fractions of N2 in a
mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?

Mole Fraction Explained

ALEKS: Calculating mole fraction

A reaction vessel is composed of 20.3 g Cl2, 4.27 g N2 and 10.8 g Ne. Calculate the mole fraction of nitrogen.

A gaseous fuel mixture stored at 745 mmHg and 298 K contains
only methane (CH4) and propane (C3H8). When 11.7 L of this
fuel mixture is burned, it produces 769 kJ of heat. What is the
mole fraction of methane in the mixture? (Assume that the
water produced by the combustion is in the gaseous state.)

What is the mole fraction of oxygen gas in air (see Table 5.3)? What volume of air contains 10.0 g of oxygen gas at 273 K and 
1.00 atm?

Calculate the average molecular weight of air from the data
given in Table 10.1.

What is the mole fraction of each gas in the mixture described 
in Problem 10.83?

During a person’s typical breathing cycle, the CO2 concentration in the expired air rises to a peak of 4.6% by volume.
(a) Calculate the partial pressure of the CO2 in the expired
air at its peak, assuming 1 atm pressure and a body temperature of 37 °C.

The percent by volume of oxygen (20.95%) is constant throughout 
the troposphere. 
(a) Express this percentage as a mole fraction.

Determine the Mole Fraction in 1.00 L of 2.20 M NaCl

(a) What are the mole fractions of O2 in a
mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?

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Types of Aqueous Solutions

When an ionic solid dissolves, ions leave the solid and become dispersed in the solvent. Three possible aqueous solutions can be formed:saturated, unsaturated and supersaturated.

Boiling Point Elevation

Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.

Intro to Henry's Law

According to&nbsp;Henry's Law, at a constant temperature the amount of a gas dissolved in a solvent is directly proportional to its partial pressure when it is in equilibrium with its liquid phase.&nbsp;

Osmotic Pressure

Osmotic Pressure is the force that drives Osmosis from higher concentration to lower concentration.

Mole Fraction (X) relates the moles of solute and solvent within a solution.&nbsp;

The Colligative Properties

The&nbsp;Colligative Properties&nbsp;explain what happens to a pure solvent as it transitions to a solution.

Molality

Molality (m)&nbsp;represents the number of moles of solute dissolved per kilogram of solvent.&nbsp;

Freezing Point Depression

Freezing Point Depression is the phenomenon when adding a solute to a pure solvent results in decreased freezing point of the solvent.

Solutions: Solubility and Intermolecular Forces

Solutions are homogeneous mixtures that result from the dissolving of a solute by a solvent.

Vapor Pressure Lowering (Raoult's Law)

Vapor Pressure is the pressure exerted by a gas at equilibrium with its liquid phase at a specific temperature in a closed system.

Henry's Law Calculations

To calculate solubility of a dissolves gas, Henry's Law Constant and partial pressure are used.

Solutions: Mass Percent

Mass Percent represents grams of solute per grams of solution, multiplied by 100.

Osmosis

Osmosis is the net movement of solvent across a semipermeable membrane.

Parts per Million (ppm)

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Parts per Million (ppm) and Parts per Billion (ppb) are used to express extremely dilute solution concentrations.</div></div>

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