Chemical Reactions Warm­ups.notebook
November 10, 2016
CH3OS Warm­Up (Sept 14)
Neon has two major isotopes, Neon­20 and Neon­22. You took a sample of 250 Neon atoms and found the following information:
Out of every 250 neon atoms, ­ 225 were Neon­20
­ 25 were Neon­22. What is the average atomic mass of Neon?
1
Chemical Reactions Warm­ups.notebook
November 10, 2016
CH3OS Warm­Up (Sept 14)
Neon has two major isotopes, Neon­20 and Neon­22. You took a sample of 250 Neon atoms and found the following information:
Out of every 250 neon atoms, ­ 225 were Neon­20
­ 25 were Neon­22. What is the average atomic mass of Neon?
2
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Sept 15)
1. Name the following Chemicals:
a) CF4
b) N3F2
c) NO3
d) N2O7
2. Write the formula for the following Chemicals:
a) Dinitrogen pentoxide
b) Silicon tetrachloride
c) Sulphur hexafluoride
d) Iodine
3
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Sept 15)
1. Name the following Chemicals:
a) CF4
b) N3F2
c) NO3
d) N2O7
2. Write the formula for the following Chemicals:
a) Dinitrogen pentoxide
b) Silicon tetrachloride
c) Sulphur hexafluoride
d) Iodine
4
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Sept 16)
1. Name the following Chemicals:
a) NO3
b) Cl2
c) Al d) Na2S
2. Write the formula for the following Chemicals:
a) Bromine
b) Magnesium phosphide
c) Aluminum nitride
d) Beryllium hydride
5
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Sept 16)
Nitrogen
________
Lead (IV) sulphide
__________
Magnesium chloride __________
Dinitrogen Heptoxide __________
Cu2O
_______________
P4
_______________
PBr3
_______________
K2O
_______________
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Sept 19)
Hydrogen ________
Copper (II) oxide __________
Lead (II) sulphate __________
Aluminum citrate_______
Iron (III) hydroxide__________
Nickel (II) carbonate __________
Pb(OH)2
SO4
_______________
_______________
BaCO3 _______________
CuCr2O7
_______________
Co(HCO3)2 _______________
K2Cr2O7
_______________
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Sept 20)
Iron
________
Copper (I) oxide __________
Lead (II) persulphate __________
magnesium citrate_______
Iron (II) hydroxide__________
Nickel (II) carbonite __________
Pb(OH)4
CuCrO4 _______________
Pb(SO5)2
_______________
_______________
BaCO2 _______________
Mn(HCO3)2 _______________
K2Cr2O7
_______________
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Sept 22)
Neon ________
Tin (IV) hydrogen sulphite__________
Lead (II) persulphate __________
Nitrogen _______
dinitrogen heptoxide __________
Nickel (II) percarbonate __________
PbO2
Cu2SO4 _______________
NO3
_______________
_______________
BaCO2 _______________
Mg(HCO3)2 _______________
NiO _______________
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Sept 23)
1. Write the balanced reaction given the following word equations:
a) Lead (II) Sulphate + Sodium Chloride ­­> Sodium Sulphate + Lead(II) Chloride
b) Propane (C3H8) + Oxygen gas ­­> Carbon dioxide + Water
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Sept 26)
1. Write the balanced reaction given the following word equations:
a) Lead (II) Nitrate + Sodium oxide ­­> Sodium Nitrate + Lead(II) Oxide
b) Zinc + Magnesium Phosphate ­­> Zinc Phosphate + Magnesium
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Feb 29)
Lead (II) nitrate reacts with Magnesium phosphate to produce Lead(II) phosphate and magnesium nitrate. Write the balanced reaction and state the type of reaction
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Sept 27)
1. Calculate the average atomic mass of chlorine given the following relative abundances:
Cl‐35 ‐‐> 75%
Cl‐37 ‐‐> 25%
2. Write the complete balanced reaction between lead (II) nitrate and Potassium iodide. 13
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Sept 29)
Write the balanced equation, state the type of reaction and name the products for the following:
Calcium phosphite reacts with silver perchlorate.
For the compound NaOH find the:
a) Molecular mass
b) Molar mass
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 3)
1. For the compound NaOH find the:
a) molecular mass
b) Molar mass
c) If you have 20g of NaOH, how many moles would you have?
2. Write the balanced reaction between Bromine and sodium chloride. State the type of reaction.
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 4)
1. What is the molar mass of potassium phosphate?
2. If you have about 212g of potassium phosphate, how many moles would you have?
3. If you needed 2mol of potassium phosphate, how many grams would you need to weigh?
4. If you have about 106g of postassium phosphate, how many moles would that be?
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 5)
1. What is the molar mass of magnesium nitrate?
2. If you have 100g of magnesium nitrate, how many moles would you have?
3. If you needed 2.5mol of magnesium nitrate, how many grams would you need to weigh?
4. If you have about 56g of magnesium nitrate, how many moles would that be?
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 6)
1. Find the molar mass of Chromium (III) oxide:
2. If you have 30g of chromium(III) oxide, how many moles is this?
3. Use your answer in #2 to find how many molecules of chromium(III)oxide there are.
4. Use your answer in #3 to find how many atoms of oxygen there are.
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 6)
1. Find the molar mass of Chromium (III) oxide:
2. If you have 30g of chromium(III) oxide, how many moles is this?
3. Use your answer in #2 to find how many molecules of chromium(III)oxide there are.
4. Use your answer in #3 to find how many atoms of oxygen there are.
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (oct 7)
1. How many atoms of oxygen are in 50g of iron(III) sulphate?
2. You have 1 million hydrogen atoms. How many grams of water can you make?
20
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 11)
1. How many moles are in 54 grams of water?
2. Use the moles calculated in #1 to determine the number of moles of Hydrogen and Oxygen atoms.
3. Use the moles of atoms calculated in #2 to determine the number of atoms of hydrogen and oxygen.
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Chemical Reactions Warm­ups.notebook
1.
November 10, 2016
Warm‐Up (Oct 12)
Write the complete, balanced reaction between the following
a) Chromium (II) phosphate and aluminum
b) Combustion of octane (C8H18)
2. How many hydrogen atoms are in 18 grams of water? 3. How many moles of hydrogen are in 3 moles of water?
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Oct 13)
1. Find the volume of 100g of hydrogen gas.
2. Find the mass of 100L of carbon tetrachloride
3. Find the volume of 20g of water vapour.
3. A sample of sugar contains 10g of oxygen ATOMS. how many moles of oxygen ATOMS are there in the sample of sugar?
23
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (March 18)
1. Name the following Chemicals:
a) CF4
b) MgF2
c) Fe2O3
d) NO3
2. Write the formula for the following Chemicals:
a) Dinitrogen pentoxide
b) Gold (III) oxide
c) Strontium nitride
d) Copper (I) phosphate
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm‐Up (Oct 13)
1. Determine the mass of 0.200mol of aluminum oxide.
2. How many moles are there in 8.64g of dinitrogen pentoxide gas?
3. Calculate the volume of the dinitrogen pentoxide gas from question 2.
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 17)
An organic compound was analyzed and the following data were produced. In a 4.479 g sample;
Mass of carbon = 3.161 g
Mass of hydrogen = 0.266 g
Mass of oxygen = 1.052 g
a) Calculate the empirical formula for the organic compound. b) If analysis revealed that the molar mass of the compound is 136 g/mol, determine the molecular formula for the compound. 26
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 17)
An organic compound was analyzed and the following data were produced. In a 4.479 g sample;
Mass of carbon = 3.161 g
Mass of hydrogen = 0.266 g
Mass of oxygen = 1.052 g
a) Calculate the empirical formula for the organic compound. b) If analysis revealed that the molar mass of the compound is 136 g/mol, determine the molecular formula for the compound. 27
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 18)
A sample of copper chloride weighs 7.7g and 4.0g of the sample is chlorine.
1. How many grams of Copper would be in the sample?
2. Use the mass of copper and chlorine to determine the empirical formula of copper chloride.
28
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 18)
A sample of copper chloride weighs 7.7g and 4.0g of the sample is chlorine.
1. How many grams of Copper would be in the sample?
2. Use the mass of copper and chlorine to determine the empirical formula of copper chloride.
29
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 19)
Write the balanced reaction between potassium iodide with lead(II) nitrate.
If you had 2 molecules of lead(II) nitrate, how many molecules of lead(II) iodide do you think could be made?
If you had 2 moles of lead(II) nitrate, how many moles of lead(II) iodide do you think could be made?
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Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 20)
Write the reaction between potassium sulphate and Iron(III) nitrate.
how many moles of iron (III) sulphate can be made from 2 moles of potassium sulphate
31
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 26)
If 1.25g of Sodium bicarbonate reacts with hydrochloric acid according to the following reaction: NaHCO3 + HCl ­­> H2O + CO2 + NaCl
1. Determine the number of moles of sodium bicarbonate used.
2. Use your answer to determine the number of moles of salt that should be produced.
3. Use your answer to determine the grams of salt that should be produced.
4. If 0.8g of salt were actually produced in the lab, determine the % yield.
32
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Oct 26)
If 1.25g of Sodium bicarbonate reacts with hydrochloric acid according to the following reaction: NaHCO3 + HCl ­­> H2O + CO2 + NaCl
1. Determine the number of moles of sodium bicarbonate used.
2. Use your answer to determine the number of moles of salt that should be produced.
3. Use your answer to determine the grams of salt that should be produced.
4. If 0.8g of salt were actually produced in the lab, determine the % yield.
33
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm‐Up (Oct 27)
Calculate the mass of copper (I) sulphate produced when 10g of copper (I) chloride reacts with excess potassium sulphate. (2 marks)
34
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Oct 31)
Determine the volume of hydrogen gas produced when 2.5g of zinc react with excess hydrochloric acid (HCl)
If this experiment is performed and 0.7L of hydrogen gas is ACTUALLY produced, determine the percent yield.
35
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (april 4)
Calculate the volume of carbon dioxide produced when 30g of propane (C3H8) is burned.
36
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Nov 1)
When propane is burned, energy is produced. Given the following reaction C3H8 + 5O2 ­­> 3CO2 + 4H2O H = ­1377 kJ
How much energy is produced when 4000 grams of propane is burned?
37
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Nov 2)
When butane is burned, energy is produced. Given the following reaction 2C2H6 + 7O2 ­­> 4CO2 + 6H2O + 977 kJ
How many grams of butane is burned if we make 2700kJ of energy?
38
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­up (Nov 4)
When propane is burned, energy is produced. Given the following reaction C3H8 + 5O2 ­­> 3CO2 + 4H2O + 1377 kJ
How much energy is produced when 4000 grams of propane is burned?
39
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Nov 3)
Calculate the mass of copper (II) sulphate produced when 30g Copper(II) chloride reacts with 30g of potassium sulphate
40
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm­Up (Nov 4)
1. 45.0g of Iron (II) sulphide and 30.0g of hydrochloric acid (HCl) are mixed. How many grams of Iron(II) Chloride will be formed?
2. A compound contains 57.54% C, 3.45% H, and 39.01% F. What is its empirical formula?
If the molar mass of the actual compound is 438.15g/mol, determine the molecular formula.
41
Chemical Reactions Warm­ups.notebook
November 10, 2016
Warm‐Up (Nov 7)
A compound contains 57.54% C, 3.45% H, and 39.01% F. What is its empirical formula?
If the molar mass of the actual compound is 438.15g/mol, determine the molecular formula.
42