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The number of atoms or molecules in exactly 1.000 mole of a substance, and is equal to 6.022 x 1023

The number of atoms or molecules in exactly 1.000 mole of a substance, and is equal to 6.022 x 1023

Avogrado’s Number

atoms of the same element that have different numbers of neutrons, which means that atoms of the same element can have different masses

Atoms neutrons, which means that atoms of the same element can have different massesof the same element that have different numbers of neutrons, which means that atoms of the same element can have different masses

- Isotope

The SI unit for amount of a substance. neutrons, which means that atoms of the same element can have different masses

The SI unit for amount of a substance. neutrons, which means that atoms of the same element can have different masses

Mole

a chemical formula that shows the simplest ratio of atoms in a compound

Emperical Formula

Which will have the greater number of ions, 1 mol of nickel (II) or 1 mol of copper (I)?

Which will have the greater number of ions, 1 mol of nickel (II) or 1 mol of copper (I)?

They will be the same they both are 1 mole, so each would have 6.022 x 1023 ions

Without making a (II) or 1 mol of copper (I)?calculation,is 1.11 mol Pt more of less than 6.022 x 1023 atoms?

Without making a (II) or 1 mol of copper (I)?calculation,is 1.11 mol Pt more of less than 6.022 x 1023 atoms?

It would be more because 1 mole would = 6.022 x 1023, and there are 1.11 moles Pt, so it would be larger than avogadro’s number

Find the mass in grams in (II) or 1 mol of copper (I)?4.30 x 1016 atoms of He, 4.00 g/mol

Find the mass in grams in (II) or 1 mol of copper (I)?4.30 x1016 atoms of He, 4.00 g/mol

4.30 x 1016 atomsHe 1 mol 4.00 g = 2.86 x 10 -7

6.022 x 1023 atoms 1 mol grams He

How many atoms are in two moles of mercury? (II) or 1 mol of copper (I)?

- 1.204 x 1022
- 1.204 x 1023
- 1.204 x 1024
- 6.022 x 1023

How many atoms are in two moles of mercury? (II) or 1 mol of copper (I)?

1.204 x 1024

How many atoms are in a mole of barium chloride, BaCl (II) or 1 mol of copper (I)?2?

- 6.022 x 1026
- 1.806 x 1024
- 1.204 x 1024
- 6.022 x 1023

How many molecules are in a mole of barium chloride, BaCl (II) or 1 mol of copper (I)?2?

- 6.022 x 1023

An element has one isotope with an atomic mass of 27.94 the element?amu. Another isotope has an atomic mass of 28.96 amu. The average atomic mass of the element is 28.02 amu. The isotope that makes up the larger percent of a sample of the element is the isotope with a mass of

27.94 amu

28.96 amu

28.02 amu

An element has one isotope with an atomic mass of 27.94 the element?amu. Another isotope has an atomic mass of 28.96 amu. The average atomic mass of the element is 28.02 amu. The isotope that makes up the larger percent of a sample of the element is the isotope with a mass of

27.94 amu, because it is closes to averageatomic mass of 28.02 amu

What is the molar mass of C the element?6H12O6?

What is the molar mass of C the element?6H12O6?

180.16 g

Simply add up the masses from the periodic table

Boron has an isotope with a mass of 10.013 the element?amu that makes up 19.8% of all boron. Its other isotope has a mass of 11.009 amu and makes up 80.2%. What is the average atomic mass of boron.

Boron has an isotope with a mass of 10.013 the element?amu that makes up 19.8% of all boron. Its other isotope has a mass of 11.009 amu and makes up 80.2%. What is the average atomic mass of boron.

Boron -10 = (.198) x 10.013 = 1.983

Boron – 11 = (.802) x 11.009 = 8.83

1.983+8.83 =10.81 amu

How many moles of hydrogen are in one mole of C the element?2H6?

How many moles of hydrogen are in one mole of C the element?2H6?

6

How many hydrogen atoms are present in one formula unit of ammonium hydrogen phosphate, (NH4)2HPO4?

How many hydrogen atoms are present in one formula unit of ammonium hydrogen phosphate, (NH4)2HPO4?

8

A compound is 5.94% H and 94.06% O. What is its empirical formula?

5.94% = 5.94 g H

94.06% = 94.06 g O

5.94g H 1 mol = 5.89 mol H

1.0079g 5.88

94.06g O 1 mole =5.88 mol O

15.999 g 5.88 HO

The first set of calculations in determining an empirical formula from masses of elements produces the subscripts of 1.67 and 1.00. What do you need to do to find the actual subscripts?

- Round of both numbers
- Round off 1.67, and use 1.00 as it is
- Multiply both subscipts by 3
- Multiply both subsripts by 6

The first set of calculations in determining an empirical formula from masses of elements produces the subscripts of 1.67 and 1.00. What do you need to do to find the actual subscripts?

- Round off 1.67, and use 1.00 as it is

A compound’s empirical formula is CH. If the formula from masses of elements produces the subscripts of 1.67 and 1.00. What do you need to do to find the actual subscripts?formula mass is 79.12 g/mol, what is the molecular formula?

A compound’s empirical formula is CH. If the molar mass is 79.12 g/mol, what is the molecular formula?

Formula mass of compound = 79.12 g

Molar mass of CH = 13.019

Molar mass of compound = 79.12 =6.07

Molar mass of CH 13.019

Multiply each by 6 to find the molecular formula = C6H6

What is the percentage of chlorine in 79.12 g/mol, what is the molecular formula?NaCl?

What is the percentage of chlorine in 79.12 g/mol, what is the molecular formula?NaCl?

Molar mass of Na = 22.990g

Molar mass of Cl = 35.453 g

Molar mass of NaCl = 58.443g

% of sodium = 22.990/58.443 x 100 = 39%

% of chlorine = 35.453/583443 x 100 = 61%

Match each equation with the correct type of reaction. 79.12 g/mol, what is the molecular formula?

- Ca(ClO3)2 CaCl2 +O2
- CaO + H2O Ca(OH)2
- C8H18 + O2 CO2 + H2O
- Decomposition
- Combustion
- Synthesis

Match each equation with the correct type of reaction. 79.12 g/mol, what is the molecular formula?

- Ca(ClO3)2 CaCl2 +O2
- CaO + H2O Ca(OH)2
- C8H18 + O2 CO2 + H2O
- Decomposition (1)
- Combustion(3)
- Synthesis ( 2)

Balance the following equation: 79.12 g/mol, what is the molecular formula?

ZnS + O2 ZnO + SO2

Balance the following equation: 79.12 g/mol, what is the molecular formula?

2ZnS + 3O2 2ZnO + 2SO2

Match each equation with the correct type of reaction. 79.12 g/mol, what is the molecular formula?

- AgNO3 + AlCl3 AgCl + Al(NO3)2
- C8H18 + O2 CO2 + H2O
- Ca(ClO3)2 CaCl2 +O2
- NaOH + HCl NaCl + HOH
- CaO + H2O Ca(OH)2
- Ni(ClO3)2 NiCl2 + O2
- Decomposition
- Combustion
- Synthesis
- Single Replacement
- Double Replacement – Precipitation
- Double Replacement – Acid/Base

Match each equation with the correct type of reaction. 79.12 g/mol, what is the molecular formula?

- AgNO3 + AlCl3 AgCl + Al(NO3)2
- C8H18 + O2 CO2 + H2O
- Ca(ClO3)2 CaCl2 +O2
- NaOH + HCl NaCl + HOH
- CaO + H2O Ca(OH)2
- Ni(ClO3)2 NiCl2 + O2
- Decomposition (6), (3)
- Combustion ( 2)
- Synthesis (5)
- Single Replacement
- Double Replacement – Precipitation (1)
- Double Replacement – Acid/Base (4)

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