Chemistry Chapter 10

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What is is the volume of 1 mole at STP?

1 mole = 22.4 L

The sum of the percentage in the percent compositions of a substance equals?

100

Calculate the volume of 76.1 g SO2 at STP?

26.6 L SO2

What is the empirical formula of a compound whose molecular formula is C2Cl6?

CCl3

What is molecular formula?

the actual ratio the elements can be found in a compound

What's in a mole of formula units?

the label of formula units is used with ionically bonded atoms

What's in a mole of atoms?

this label is used when dealing with elements by themselves

Just like solids have a molar mass, gases have what two things?

a molar volume and STP

What is the mole?

a way to count particles

How do you find out the number of atoms? For example, how many atoms are in 1 mole of H20?

add together the subscripts, there are 3 moles of atoms in H2O

What is the mole central to?

all of our calculation, so we can covert everything to the mole

What is the label/units for formula mass?

amu, atomic mass units

What does amu stand for?

atomic mass units

How is molar mass calculated?

calculated the same way as formula mass, just different units (g/mol) (1 mol= __________g)

What is formula mass?

defined as teh sum of the atomic masses of all the atoms in a compound

Why was atomic mass units developed?

developed because the actual mass of an atom was so small

The _____ is the simplest whole-number ratio of atoms in a compound?

empirical formula

What are the three steps to find percent composition?

find the molar mass of the compound mass of the element divided by the molar mass multiply by 100% get percentages

The sum of the atomic masses of all the atoms in a compound is called the?

formula mass

What kind of particle is represented by a formula unit ?

ionic

The molar mass of a compound depends upon the ?

mass of each element in the compound

The molecular formula of a compound can be determined by comparing the empirical formula mass with the?

molar mass of the compound

The actual number of atoms of each element in a molecular compound is given by the ___?

molecular formula

A mole of carbon dioxide contains 6.02 x 10^23 _____?

molecules because it is covalently bonded

What are the three way to describe the makeup of chemicals?

percent composition, empirical formula, and molecular formula

What does STP stand for?

standard temperature and pressure

What is percent composition?

tells what percent the elements are in a compound

What is molar volume?

the amount of gas one mole occupies at STP

What's in a mole of molecules?

the label of molecule is used with covalently bonded atoms

What is atomic mass?

the mass of each atom in amu

What is molar mass?

the mass of one mole of a substance

What is empirical formula?

the smallest ratio the elements can be found in (reduced down)

Can empirical formulas be hte same as molecular formulas?

they can be the same, but this isn't always true

How many formula units are in 3.51 grams of Silver Nitrate?

1.24 x 10^22 formula units AgNO3

How many moles of Chlorine ions are in 1 mole of CaCl2?

2 moles of Cl- ions

The molar volume of a gas at STP is?

22.4 L/mol

A sample of ammonia contains 7.22 moles of ammonia. How many molecules of ammonia are in the sample?

4.35 x 10^24 molecules NH4

What does 1 mole of an elements equal?

6.02 x 10^23 atoms

What is 1 mole of ionic substance equal to?

6.02 x 10^23 formula units

What does 1 mole of a molecule equal?

6.02 x 10^23 molecules

Besides being 1 mole, what is 6.02 x 10^23 called?

Avogadro's number

Which is a possible molecular formula of a compound whose empirical formula is CH?

C2H2

What are the 3 basic steps to finding the Empirical Formula of a compound?

Convert % of each element to grams Convert grams to moles of each element Divide by the smallest number of moles If the number is a whole number, use it as the subscript for that element If the number isn't a whole number, multiply it to get a whole number (you have to multiply all number by the same number)- then use it as a subscript

What are the 4 basic steps to find molecular formula from the empirical formula?

Find the Empirical Formula Calculate the Empirical Formula mass (add it up and find the molar mass) Divide the molar mass (that was given to you) by the empirical formula mass This should give you a whole number, so use this number to multiply the subscripts of the empirical formula

What is standard temperature and pressure (STP)?

0 degrees Celsuis 1 atmosphere (1 atm)

Standard pressure is _____?

1 atm


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