Warm Up (Sept 12) How will an atom change if you change the number of: a) Protons? b) Electrons? c) Neutrons? 1
CH3OS Warm Up (Sept 13) 1. What is an isotope? 2. Neon has two major isotopes, Neon 20 and Neon 22. If you took a sample of Neon atoms which isotope do you think there would be more atoms of? (Hint: look at your periodic table) 2
CH3OS Warm Up (Sept 13) Neon has two major isotopes, Neon 20 and Neon 22. You took a sample of 250 Neon atoms and found the following information: Out of 250 neon atoms, 225 were Neon 20 25 were Neon 22. What is the average atomic mass of Neon? 3
1. Name the following Chemicals: Warm Up (Sept 15) a) CF 4 b) N 3 F 2 c) NO 3 d) N 2 O 7 2. Write the formula for the following Chemicals: a) Dinitrogen pentoxide b) Silicon tetrachloride c) Sulphur hexafluoride d) Iodine 4
Warm Up (Sept 18) 1. Name the following Chemicals: a) NO 3 b) Cl 2 c) Al d) Na 2 S 2. Write the formula for the following Chemicals: a) Bromine b) Magnesium phosphide c) Aluminum nitride d) Beryllium hydride 5
Warm up (Sept 19) Nitrogen Lead (IV) sulphide Magnesium chloride Dinitrogen Heptoxide Cu 2 O P 4 PBr 3 K 2 O 6
Warm up (Sept 21) Hydrogen Copper (II) oxide Lead (II) sulphate Aluminum citrate Iron (III) hydroxide Nickel (II) carbonate Pb(OH) 2 CuCr 2 O 7 SO 4 Co(HCO 3 ) 2 BaCO 3 K 2 Cr 2 O 7 7
Warm up (Sept 22) Iron Copper (I) oxide Lead (II) persulphate magnesium citrate Iron (II) hydroxide Nickel (II) carbonite Pb(OH) 4 CuCrO 4 Pb(SO 5 ) 2 Mn(HCO 3 ) 2 BaCO 2 K 2 Cr 2 O 7 8
Warm up (Sept 25) Neon Tin (IV) hydrogen sulphite Lead (II) persulphate Nitrogen dinitrogen heptoxide Nickel (II) percarbonate PbO 2 Cu 2 SO 4 NO 3 Mg(HCO 3 ) 2 BaCO 2 NiO 9
Warm up (Feb 23) 1. Write the balanced reaction given the following word equations: a) Lead (II) Sulphate + Sodium Chloride > Sodium Sulphate + Lead(II) Chloride b) Propane (C 3 H 8 ) + Oxygen gas > Carbon dioxide + Water 10
Warm up (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 11
Warm Up (Sept 27) 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 12
Warm Up (Sept 28) 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
Warm Up (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 14
Warm Up (Oct 3) 1. Given Iron(II) hydroxide, find the: a) molecular mass b) Molar mass c) If you have about 45g of NaOH, how many moles would you have? 2. Write the balanced reaction between Bromine and sodium chloride. State the type of reaction. 15
Warm Up (oct 5) 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? 16
Warm Up (March 7) 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? 17
Warm Up (Oct 6) 1. Find the molar mass of Gold (III) Sulphide: 2. If you have 50g of Gold(III) sulphide, how many moles is this? 3. If you need 0.3moles of gold(iii) sulphide, how many grams would you weigh? 18
Warm Up (October 10) 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. Challenge: Use your answer in #3 to find how many atoms of oxygen there are. 19
Warm Up (October 11) 1. Find the molar mass of Lead(II) sulphide: 2. If you have 30g of lead(ii) sulphide, how many moles is this? 3. Use your answer in #2 to find how many molecules of lead(ii) Sulphide there are. 4. Use your answer in #3 to find how many atoms of sulphur there are. 20
Warm Up (Oct 12) 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? 21
Warm Up (Oct 13) 1. Write the complete, balanced reaction between the following a) Chromium (II) phosphate and aluminum b) Combustion of octane (C 8 H 18 ) 2. How many hydrogen atoms are in 18 grams of water? 3. How many moles of hydrogen are in 3 moles of water? 22
Warm Up (Oct 16) 1. How many moles are in 54 grams of Carbon Dioxide? 2. Determine the number of moles of Hydrogen and Oxygen atoms in 3 moles of water. 3. Challenge: Use your answer from #1 to find how many liters of Carbon dioxide gas there would be at STP. 23
Warm up (Oct 17) 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? 24
Warm Up (Oct 18) 1. Name the following Chemicals: a) CF 4 b) MgF 2 c) Fe 2 O 3 d) NO 3 2. Write the formula for the following Chemicals: a) Dinitrogen pentoxide b) Gold (III) oxide c) Strontium nitride d) Copper (I) phosphate 25
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. 26
Warm Up (Oct 18) 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
Warm Up (Mar 20) 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. 28
Warm Up (Oct 23) Happy Mole Day!!! 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. 3. Why did Avogadro stop going to a chiropractor on October 24th? 29
Warm Up (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. 30
Warm Up (Oct 24) 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? 31
Warm Up (Oct 25) 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 32
Warm Up (March 22) If 1.25g of Sodium bicarbonate reacts with hydrochloric acid according to the following reaction: NaHCO 3 + HCl > H 2 O + CO 2 + 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
Warm Up (oct 26) If 1.25g of Sodium bicarbonate reacts with hydrochloric acid according to the following reaction: NaHCO 3 + HCl > H 2 O + CO 2 + 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. 34
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) 35
Warm Up (October 31) If 0.75g of Sodium bicarbonate reacts with hydrochloric acid according to the following reaction: NaHCO 3 + HCl > H 2 O + CO 2 + NaCl 1. Determine the grams of salt that should be produced. 2. If 0.65g of salt were actually produced in the lab, determine the % yield. 36
Warm Up (Apr 4) 1. Balance: Ca(OH) 2 + H 3 PO 4 > Ca 3 (PO 4 ) 2 + H 2 O 2. Write the reaction for the burning of butane fuel (C 4 H 10 ) 3. Determine the empirical and molecular formula for a compound that has a molar mass of 227g/mol, and the following percent composition: 37.0% carbon, 2.20% hydrogen, 18.5% nitrogen and 42.3% oxygen. (3 marks) 37
Warm Up (Nov 1) Calculate the volume of carbon dioxide produced when 30g of propane (C 3 H 8 ) is burned. 38
Warm up (Nov 2) 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. 39
Warm up (Nov 6) When butane is burned, energy is produced. Given the following reaction 2C 2 H 6 + 7O 2 > 4CO 2 + 6H 2 O + 977 kj How many grams of butane is burned if we make 2700kJ of energy? 40
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Warm up (April 10) When propane is burned, energy is produced. Given the following reaction C 3 H 8 + 5O 2 > 3CO 2 + 4H 2 O H = 1377 kj How much energy is produced when 4000 grams of propane is burned? 42
Warm up (Nov 7) When propane is burned, energy is produced. Given the following reaction C 3 H 8 + 5O 2 > 3CO 2 + 4H 2 O + 1377 kj How much energy is produced when 4000 grams of propane is burned? 43
Warm Up (Nov 8) Calculate the mass of copper (II) sulphate produced when 30g Copper(II) chloride reacts with 30g of potassium sulphate 44
Warm Up (Nov 9) 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. 45
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. 46