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Chemistry B Quizzes. The number of atoms or molecules in exactly 1.000 mole of a substance, and is equal to 6.022 x 10 23. The number of atoms or molecules in exactly 1.000 mole of a substance, and is equal to 6.022 x 10 23. Avogrado’s Number.

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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 10 23
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 10 231
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
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 substance1
The SI unit for amount of a substance. neutrons, which means that atoms of the same element can have different masses

Mole





Which will have the greater number of ions 1 mol of nickel ii or 1 mol of copper i1
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 calculation is 1 11 mol pt more of less than 6 022 x 10 23 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?


Without making a calculation is 1 11 mol pt more of less than 6 022 x 10 23 atoms1
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 4 30 x 10 16 atoms of he 4 00 g mol
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 4 30 x10 16 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
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 mercury1
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 2
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 2
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 6 h 12 o 6
What is the molar mass of C the element?6H12O6?


What is the molar mass of c 6 h 12 o 61
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 hydrogen atoms are present in one formula unit of ammonium hydrogen phosphate nh 4 2 hpo 4
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 nh 4 2 hpo 41
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 formula1
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
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 nacl
What is the percentage of chlorine in 79.12 g/mol, what is the molecular formula?NaCl?


What is the percentage of chlorine in nacl1
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
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 reaction1
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
Balance the following equation: 79.12 g/mol, what is the molecular formula?

ZnS + O2 ZnO + SO2


Balance the following equation1
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 reaction2
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 reaction3
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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