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 ...
Too Hot to Handle Lab
... reaction. The word exothermic comes from the root – “thermic”, which refers to heat, and the prefix – “exo” which means out of. Heat comes out of, or is released from, a reacting substance during an exothermic reaction. A reaction that involves burning, or a combustion reaction, is an example of an ...
... reaction. The word exothermic comes from the root – “thermic”, which refers to heat, and the prefix – “exo” which means out of. Heat comes out of, or is released from, a reacting substance during an exothermic reaction. A reaction that involves burning, or a combustion reaction, is an example of an ...
Review Packet
... _____ 56. Equation obey the laws of conservation of mass if they’ve been properly ___. _____ 57. A solid product. _____ 58. A number within a formula representing the number of atoms of each element present in the formula. _____ 59. A solid compound dissolved in water. _____ 60. Elements that do not ...
... _____ 56. Equation obey the laws of conservation of mass if they’ve been properly ___. _____ 57. A solid product. _____ 58. A number within a formula representing the number of atoms of each element present in the formula. _____ 59. A solid compound dissolved in water. _____ 60. Elements that do not ...
File
... 1. Write separate equations for oxidation and reduction half reactions 2. For each half-reaction A. balance all the elements B. balance oxygen using H2O C. balance hydrogen using H+ D. balance the charge using electrons 3. if necessary, multiply one or both half-reactions by an integer to equalize t ...
... 1. Write separate equations for oxidation and reduction half reactions 2. For each half-reaction A. balance all the elements B. balance oxygen using H2O C. balance hydrogen using H+ D. balance the charge using electrons 3. if necessary, multiply one or both half-reactions by an integer to equalize t ...
study guide and review for first semester final
... from percentage composition to determine the compound’s empirical formula. Ex. A compound with 0.90 g Ca and 1.6 g Cl has what empirical formula? (CaCl2) Ex. A white powder used in paints, enamels and ceramics has the following percentage composition: Ba 69.6 %; C 6.09%; O 24.3 %. What is its empiri ...
... from percentage composition to determine the compound’s empirical formula. Ex. A compound with 0.90 g Ca and 1.6 g Cl has what empirical formula? (CaCl2) Ex. A white powder used in paints, enamels and ceramics has the following percentage composition: Ba 69.6 %; C 6.09%; O 24.3 %. What is its empiri ...
Chapter 4 - WordPress.com
... • Theoretical yield – the maximum amount of product expected in a chemical reaction. • In reality, most chemical reactions produce less product than the theoretical yield predicts. The actual amount of product obtained from a chemical reaction is the actual yield. The actual yield is only determined ...
... • Theoretical yield – the maximum amount of product expected in a chemical reaction. • In reality, most chemical reactions produce less product than the theoretical yield predicts. The actual amount of product obtained from a chemical reaction is the actual yield. The actual yield is only determined ...
rules for predicting products of chemical reactions
... - If a compound contains at least one of the ions that is proven soluble, then the compound will be at least moderately soluble - One product must be soluble and one product must be insoluble o The insoluble product is the precipitate that forms when the reaction takes place o Usually a precipitate ...
... - If a compound contains at least one of the ions that is proven soluble, then the compound will be at least moderately soluble - One product must be soluble and one product must be insoluble o The insoluble product is the precipitate that forms when the reaction takes place o Usually a precipitate ...
Document
... Which statement is true if 12 moles of CO and 12 moles of Fe2O3 are allowed to react? 3CO(g) + Fe2O3(s) 2Fe(s) + 3CO2(g) a. The limiting reactant is CO and 8.0 mol Fe will be formed. b. The limiting reactant is Fe2O3 and 24 mol Fe will be formed. c. The limiting reactant is CO and 3.0 mol CO2 will ...
... Which statement is true if 12 moles of CO and 12 moles of Fe2O3 are allowed to react? 3CO(g) + Fe2O3(s) 2Fe(s) + 3CO2(g) a. The limiting reactant is CO and 8.0 mol Fe will be formed. b. The limiting reactant is Fe2O3 and 24 mol Fe will be formed. c. The limiting reactant is CO and 3.0 mol CO2 will ...
Chapter 12 - "Chemical Formulas and Equations"
... – The molecular ratio leads to the concept of the mole ratio since any number of molecules can react as long as they are in the correct ratio – Since 6.02 X 1023 molecules is the number of particles in a mole, the coefficients therefore represent the number of moles involved in a chemical reaction. ...
... – The molecular ratio leads to the concept of the mole ratio since any number of molecules can react as long as they are in the correct ratio – Since 6.02 X 1023 molecules is the number of particles in a mole, the coefficients therefore represent the number of moles involved in a chemical reaction. ...
Review Station Ideas
... Station 10 – HYDRATES A student is assigned the task of determining the number of moles of water in one mole of MgCl2 · n H2O. The student collects the data shown in the following table. Mass of empty container Initial mass of sample and container Mass of sample and container after first heating Mas ...
... Station 10 – HYDRATES A student is assigned the task of determining the number of moles of water in one mole of MgCl2 · n H2O. The student collects the data shown in the following table. Mass of empty container Initial mass of sample and container Mass of sample and container after first heating Mas ...
Chapter 4 Quantities of Reactants and Products 4.1 Chemical
... Stoichiometry is the relationship that describes the relation between the masses of reactants and products. 4.2 Patterns of Chemical Reactions (p. 126) In a combination reaction, two substances combine to form a third substance. {A + B ----> AB} ...
... Stoichiometry is the relationship that describes the relation between the masses of reactants and products. 4.2 Patterns of Chemical Reactions (p. 126) In a combination reaction, two substances combine to form a third substance. {A + B ----> AB} ...
name - cloudfront.net
... 19. Which of the following will occur when solutions of CuSO4(aq) and BaCl2(aq) are mixed? A. A precipitate of CuCl2 will form; Ba2+ and SO42– are spectator ions. B. A precipitate of CuSO4 will form; Ba2+ and Cl– are spectator ions. C. A precipitate of BaSO4 will form; Cu2+ and Cl– are spectator ion ...
... 19. Which of the following will occur when solutions of CuSO4(aq) and BaCl2(aq) are mixed? A. A precipitate of CuCl2 will form; Ba2+ and SO42– are spectator ions. B. A precipitate of CuSO4 will form; Ba2+ and Cl– are spectator ions. C. A precipitate of BaSO4 will form; Cu2+ and Cl– are spectator ion ...
Calculations with Chemical Formulas and Equations
... – C is determined from the mass of CO2 produced – H is determined from the mass of H2O produced – O is determined by difference after the C and H have been ...
... – C is determined from the mass of CO2 produced – H is determined from the mass of H2O produced – O is determined by difference after the C and H have been ...
Unit 8 Homework Packet
... Calculate the mass of chlorine gas required to produce 5.00 × 10-3 g of chlorine monofluoride given an excess of fluorine gas. ...
... Calculate the mass of chlorine gas required to produce 5.00 × 10-3 g of chlorine monofluoride given an excess of fluorine gas. ...
Are You suprised ?
... CaCO3 + HCl CaCl2 + H2O + CO2 How many moles of CaCO3 can be dissolved in .0250 mol HCl? ...
... CaCO3 + HCl CaCl2 + H2O + CO2 How many moles of CaCO3 can be dissolved in .0250 mol HCl? ...
U-6 Stoichiometry Notes
... • mole = the number of atoms of an element that would be found in, say, 12.01 grams of carbon-12 or 14.01 grams of nitrogen-14 (the molar mass) • mole = ______________________ atoms (this number is called “________________ number”) • mole = __________ L of any gas at STP (standard temperature and pr ...
... • mole = the number of atoms of an element that would be found in, say, 12.01 grams of carbon-12 or 14.01 grams of nitrogen-14 (the molar mass) • mole = ______________________ atoms (this number is called “________________ number”) • mole = __________ L of any gas at STP (standard temperature and pr ...
Dr Davids Essential Chemistry Definitions Bk1
... element) more positive or less negative. Polymerisation: A reaction in which many small molecules (monomers) join up in a long chain to form a macromolecule. eg, ethene polymerises to give polyethene. Catalyst: A positive catalyst speeds up a chemical reaction by providing an alternative reaction pa ...
... element) more positive or less negative. Polymerisation: A reaction in which many small molecules (monomers) join up in a long chain to form a macromolecule. eg, ethene polymerises to give polyethene. Catalyst: A positive catalyst speeds up a chemical reaction by providing an alternative reaction pa ...
Block 1 - cloudfront.net
... Fe2 + 2H20 2FeOH2 a. Write the six mole ratios that can be derived from this equation. b. How many moles of Iron are needed to form 2.5 mol of FeOH2? ...
... Fe2 + 2H20 2FeOH2 a. Write the six mole ratios that can be derived from this equation. b. How many moles of Iron are needed to form 2.5 mol of FeOH2? ...
Chemical Reactions Practice Test
... a) twice as many atoms b) the same number of atoms c) half the number of atoms _____2. What unit allows chemists to compare one chemical to another? a) amu b) kilograms c) atomic weights d) moles ______3. The coefficients from the balanced equation represent a) mole ratios b) masses c) molar masses ...
... a) twice as many atoms b) the same number of atoms c) half the number of atoms _____2. What unit allows chemists to compare one chemical to another? a) amu b) kilograms c) atomic weights d) moles ______3. The coefficients from the balanced equation represent a) mole ratios b) masses c) molar masses ...
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.