Unit 2: Chemical Reactions
... and numbers. • The subscript number tells how many atoms of the element are present in the compound • Example: CO2 = Carbon Dioxide – Di = 2 – 1 Carbon atom and 2 oxygen atoms ...
... and numbers. • The subscript number tells how many atoms of the element are present in the compound • Example: CO2 = Carbon Dioxide – Di = 2 – 1 Carbon atom and 2 oxygen atoms ...
3. What is the empirical formula of a compound that is
... As you learned in health and biology, food energy typically comes from carbohydrates, proteins and fats. The amount of energy that the body can use per gram of these substances is not the same. The following balanced exothermic reaction represents combustion (respiration) of glucose (a carbohydrate) ...
... As you learned in health and biology, food energy typically comes from carbohydrates, proteins and fats. The amount of energy that the body can use per gram of these substances is not the same. The following balanced exothermic reaction represents combustion (respiration) of glucose (a carbohydrate) ...
Problem Set: Empirical and Molecular Formulas
... 1molAl (OH )3 34.0g HCl needs 24.2 g Al(OH)3 to react completely, 12.0g Al(OH)3 is not enough 3. Ammonia, NH3, is used throughout the world as a fertilizer. To manufacture ammonia, nitrogen, N2, is combined with hydrogen, H2, in a synthesis reaction. a) Write a balanced chemical equation for the for ...
... 1molAl (OH )3 34.0g HCl needs 24.2 g Al(OH)3 to react completely, 12.0g Al(OH)3 is not enough 3. Ammonia, NH3, is used throughout the world as a fertilizer. To manufacture ammonia, nitrogen, N2, is combined with hydrogen, H2, in a synthesis reaction. a) Write a balanced chemical equation for the for ...
Writing and Balancing Chemical Equations
... Solid iron (III) sulfide reacts with gaseous hydrogen chloride to form iron (III) chloride and hydrogen sulfide gas. Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water. ...
... Solid iron (III) sulfide reacts with gaseous hydrogen chloride to form iron (III) chloride and hydrogen sulfide gas. Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water. ...
What are the general types of reactions?
... – Magnesium and Hydrogen Chloride make Hydrogen and Magnesium Chloride – Ethylene (C2H4) burns with Oxygen to produce Carbon Dioxide and Water. – Hydrogen and Chlorine combine to make Hydrogen Chloride ...
... – Magnesium and Hydrogen Chloride make Hydrogen and Magnesium Chloride – Ethylene (C2H4) burns with Oxygen to produce Carbon Dioxide and Water. – Hydrogen and Chlorine combine to make Hydrogen Chloride ...
South Pasadena · AP Chemistry
... Calculate the mass percent (percent composition by mass) of a substance based on its molecular formula. Give examples of empirical formulas and molecular formulas. Identify a formula as empirical or molecular. Calculate the empirical formula from mass percentages or mass data. Determine th ...
... Calculate the mass percent (percent composition by mass) of a substance based on its molecular formula. Give examples of empirical formulas and molecular formulas. Identify a formula as empirical or molecular. Calculate the empirical formula from mass percentages or mass data. Determine th ...
Sample Paper - Army Public School Jammu Cantt
... 3. Amongst the isomeric alkanes of molecular formula C5H12, identify the one that on photochemical chlorination yields a single monochloride. 4. Give the IUPAC name and structure of the amine obtained when 3-chlorobutanamide undergoes Hoffmann –bromamide reaction. ...
... 3. Amongst the isomeric alkanes of molecular formula C5H12, identify the one that on photochemical chlorination yields a single monochloride. 4. Give the IUPAC name and structure of the amine obtained when 3-chlorobutanamide undergoes Hoffmann –bromamide reaction. ...
Chapter 8
... matter can neither be created nor destroyed, but it can change forms chemical equations must show that matter was conserved ...
... matter can neither be created nor destroyed, but it can change forms chemical equations must show that matter was conserved ...
Unit 13 Worksheet Answers
... b. What happens to the amount of N 2 O 4 when the temperature is increased? decrease c. What happens to the amount of NO 2 when N 2 O 4 is added? Increase d. In what direction will the equilibrium shift when the volume of the container is decreased? right e. Is this reaction endothermic or exothermi ...
... b. What happens to the amount of N 2 O 4 when the temperature is increased? decrease c. What happens to the amount of NO 2 when N 2 O 4 is added? Increase d. In what direction will the equilibrium shift when the volume of the container is decreased? right e. Is this reaction endothermic or exothermi ...
I. Structure of Matter
... • At a certain temperature, the vapor pressure of benzene is 0.930 atm. A solution prepared by dissolving 10.0 g of a molecular, nonvolatile solute in 78.11 g benzene at that temperature has a vapor pressure of 0.900 atm. Determine the MM of the solute. • A 0.350 g sample of a large biomolecule was ...
... • At a certain temperature, the vapor pressure of benzene is 0.930 atm. A solution prepared by dissolving 10.0 g of a molecular, nonvolatile solute in 78.11 g benzene at that temperature has a vapor pressure of 0.900 atm. Determine the MM of the solute. • A 0.350 g sample of a large biomolecule was ...
Review Packet
... 80. A sample of a molecular compound was analyzed and found to contain 25.9g Nitrogen and 74.1g Oxygen. Determine the empirical formula of the compound. ...
... 80. A sample of a molecular compound was analyzed and found to contain 25.9g Nitrogen and 74.1g Oxygen. Determine the empirical formula of the compound. ...
chemical*equations
... Hydrogen'and'Oxygen'react'vigorously'to'form'water.'If' 275'hydrogen'molecules'are'reacted'with'125'oxygen' molecules'in'a'closed'container,'how'many'hydrogen,' oxygen,'and'water'molecules'will'remain'after'the' reaction'is'complete?' (a)'150'hydrogen'+'0'Oxygen'+'125'water' (b)'0'hydrogen'+'25'oxyg ...
... Hydrogen'and'Oxygen'react'vigorously'to'form'water.'If' 275'hydrogen'molecules'are'reacted'with'125'oxygen' molecules'in'a'closed'container,'how'many'hydrogen,' oxygen,'and'water'molecules'will'remain'after'the' reaction'is'complete?' (a)'150'hydrogen'+'0'Oxygen'+'125'water' (b)'0'hydrogen'+'25'oxyg ...
Chapter 5 - U of L Class Index
... All of the equations we’ve seen so far have assumed that 100% of product was formed. In reality, this is rarely the case. Side reactions or the equilibrium can prevent reactions from going to completion. When chemists perform reactions, there are two things they want to know; a) what is the theoreti ...
... All of the equations we’ve seen so far have assumed that 100% of product was formed. In reality, this is rarely the case. Side reactions or the equilibrium can prevent reactions from going to completion. When chemists perform reactions, there are two things they want to know; a) what is the theoreti ...
Stoichiometry: Calculations with Chemical Formulas and
... of a compound that comes from each of the elements in the compound by using this equation: (number of atoms)(atomic weight) % element = ...
... of a compound that comes from each of the elements in the compound by using this equation: (number of atoms)(atomic weight) % element = ...
Unit 3 - sotochem
... Be able to balance chemical equations and know why balancing is important: ➢ Equations should be balanced in order to satisfy the law of conservation of mass (matter can neither be created nor destroyed, just changed in form) - same # of each kind of atom on both sides of the equation ➢ When bala ...
... Be able to balance chemical equations and know why balancing is important: ➢ Equations should be balanced in order to satisfy the law of conservation of mass (matter can neither be created nor destroyed, just changed in form) - same # of each kind of atom on both sides of the equation ➢ When bala ...
Gas Stoichiometry
... reacts with excess hydrogen gas at 3.00 atm and 25 oC. (Hint: you have to do the stoichiometry AND use the Ideal Gas Law because this is not at STP. The important thing is that you need to moles of nitrogen!) ...
... reacts with excess hydrogen gas at 3.00 atm and 25 oC. (Hint: you have to do the stoichiometry AND use the Ideal Gas Law because this is not at STP. The important thing is that you need to moles of nitrogen!) ...
Lecture 2 - Chemistry at Winthrop University
... • A Complete Ionic Equation shows all chemical species present in the reaction • A Net Ionic Equation shows the net change taking place in the reaction – The Net Ionic Equation is made by taking the Spectator Ions out of the complete ionic equation ...
... • A Complete Ionic Equation shows all chemical species present in the reaction • A Net Ionic Equation shows the net change taking place in the reaction – The Net Ionic Equation is made by taking the Spectator Ions out of the complete ionic equation ...
H 2 and H 2 + O 2 g H 2 O and H 2 O Hydrogen + Oxygen g Water
... Measure out 50ml of hydrochloric acid (HCl) into a beaker (find its ...
... Measure out 50ml of hydrochloric acid (HCl) into a beaker (find its ...
a) air c) milk f) beer
... When two elements form more than one compound, the masses of one element in these compounds for a fixed mass of the other element are in ratios of small whole numbers. ...
... When two elements form more than one compound, the masses of one element in these compounds for a fixed mass of the other element are in ratios of small whole numbers. ...
Describing Chemical Reactions
... Of what? – chemical formulas In what state? – physical state Letters in parentheses indicate the physical state of each substance involved in the reaction (g) gas ; (l) liquid ; (s) solid ; (aq) aqueous solution ...
... Of what? – chemical formulas In what state? – physical state Letters in parentheses indicate the physical state of each substance involved in the reaction (g) gas ; (l) liquid ; (s) solid ; (aq) aqueous solution ...
Stoichiometry
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.