May 26, 2022 • How do you find the molar mass of aspartame?
• How many moles are in 10 grams of aspartame?
• Which element is most abundant in aspartame C14H18N2O5?
• How many years would it take to count to a mole?
• What is the mole of CU?
• Why is it not possible to directly count the number of particles in a mole?
• What does Avogadro’s law mean?
• How do you demonstrate Avogadro’s law?
• What is N in combined gas law?
• What does N mean in PV nRT?
• What is a real life example of combined gas law?
• What is a real-life example of Avogadro’s law?
• What is an example of Boyle’s Law in real-life?
• How is Dalton’s law used in real-life?

## How do you find the molar mass of aspartame?

Mass of aspartame = 5 mg = 0.005 grams. Also, molar mass of aspartame = 294.3 grams. Now, moles of aspartame = {eq}frac{mass}{molar Mass of aspartame = 5 mg = 0.005 grams.

0.034 moles

## Which element is most abundant in aspartame C14H18N2O5?

Percent composition by element

Element Symbol Mass Percent
Hydrogen H 6.165%
Carbon C 57.135%
Nitrogen N 9.519%
Oxygen O 27.182%

7 The Mole • 1 dozen cookies = 12 cookies • 1 mole of cookies = 6.02 X 1023 cookies • 1 dozen cars = 12 cars • 1 mole of cars = 6.02 X 1023 cars • 1 dozen Al atoms = 12 Al atoms • 1 mole of Al atoms = 6.02 X 1023 atoms Note that the NUMBER is always the same, but the MASS is very different!

## How many years would it take to count to a mole?

rate of 10 million per second, it would take about 2 billion years to count the atoms in one mole.

## What is the mole of CU?

Solution: The mass of 1 mole (6.022 x 1023 atoms) of copper is 63.55 g.

## Why is it not possible to directly count the number of particles in a mole?

Atoms and molecules are incredibly small and even a tiny chemical sample contains an unimaginable number of them. Therefore, counting the number of atoms or molecules in a sample is impossible. To determine the chemical amount of a sample, we use the substance’s molar mass, the mass per mole of particles.

## What does Avogadro’s law mean?

Avogadro’s law, a statement that under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules.

## How do you demonstrate Avogadro’s law?

Implications of Avogadro’s Law If pressure and temperature of a gas are constant, when the amount of gas increases, the volume increases. If pressure and temperature of a gas are constant, when the amount of gas decreases, the volume decreases. You prove Avogadro’s Law every time you blow up a balloon.

## What is N in combined gas law?

n = # of moles (mol) R = the Ideal Gas Law Constant. T = Temperature in Kelvin (K) The value n is the amount of the gas measured as moles.

## What does N mean in PV nRT?

The ideal gas law is: pV = nRT, where n is the number of moles, and R is universal gas constant.

## What is a real life example of combined gas law?

One example of the combined gas law applies to scuba diving. In scuba divers, human lungs are the container that hold the gas. The pressure in water is greater than pressure in air, and water pressure increases with depth. With each additional foot that divers descend, water pressure rises.

## What is a real-life example of Avogadro’s law?

A flat tire takes up less space than an inflated tire, because it contains less air. Lungs expand as they fill with air. Exhaling decreases the volume of the lungs. A balloon filled with helium weighs much less than an identical balloon filled with air.

## What is an example of Boyle’s Law in real-life?

You can observe a real-life application of Boyle’s Law when you fill your bike tires with air. When you pump air into a tire, the gas molecules inside the tire get compressed and packed closer together. This increases the pressure of the gas, and it starts to push against the walls of the tire.

## How is Dalton’s law used in real-life?

Dalton’s law refers to the effects of which partial pressure might have on scuba divers. Whenever there is an increase in the partial pressure of nitrogen, this will cause a higher concentration of nitrogen to be dissolved in the blood of the diver, which can cause nitrogen narcosis, a common side effect.