Kinetics and Equilibrium
... What can we conclude from each chart? How are the two charts defining what it means for a reaction to be in equilibrium? ...
... What can we conclude from each chart? How are the two charts defining what it means for a reaction to be in equilibrium? ...
Cl -1
... metals, active nonmetal elements can replace less active nonmetals. Use the Activity series (snoopy sheet) to determine whether or not the reaction will occur. Driving force is the transfer of electrons. ...
... metals, active nonmetal elements can replace less active nonmetals. Use the Activity series (snoopy sheet) to determine whether or not the reaction will occur. Driving force is the transfer of electrons. ...
5H2O → CuSO4 + 5H2O(g)
... Example: NaCl (aq) + AgNO3 (aq) ? Draw these compounds in two separate aqueous environments. What are the possible products when they are combined? ...
... Example: NaCl (aq) + AgNO3 (aq) ? Draw these compounds in two separate aqueous environments. What are the possible products when they are combined? ...
FINAL EXAM REVIEW PROBLEMS
... residue. Calculate the mass percent of solute present in the original seawater. ...
... residue. Calculate the mass percent of solute present in the original seawater. ...
Balancing Chemical Reactions
... 1.) The formulas of the reactants and products cannot be changed, do not alter subscripts or charges. 2.) The only numbers that can be changed are the numbers indicating how many molecules or atoms, which are called coefficients. 3.) A coefficient is assumed to be one if there is not a number in fro ...
... 1.) The formulas of the reactants and products cannot be changed, do not alter subscripts or charges. 2.) The only numbers that can be changed are the numbers indicating how many molecules or atoms, which are called coefficients. 3.) A coefficient is assumed to be one if there is not a number in fro ...
Introduction
... ◦ Acid-base neutralization: acid and base react to form water and a salt (ionic compound) ◦ Oxidation-Reduction: electrons are transferred between atoms in reaction Combination Decomposition Single-replacement (metal or hydrogen) ...
... ◦ Acid-base neutralization: acid and base react to form water and a salt (ionic compound) ◦ Oxidation-Reduction: electrons are transferred between atoms in reaction Combination Decomposition Single-replacement (metal or hydrogen) ...
Prerequisite Knowledge for Chemistry
... The periodic table is ordered from left to right and down by increasing atomic number. ...
... The periodic table is ordered from left to right and down by increasing atomic number. ...
Chapter 4 4.1 Defining the Atom • Early Models of the Atom atom
... 1) All elements are composed of tiny indivisible particles called atoms 2) Atoms of the same element are identical. Atoms of any one element are different from those of any other element 3) Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratio ...
... 1) All elements are composed of tiny indivisible particles called atoms 2) Atoms of the same element are identical. Atoms of any one element are different from those of any other element 3) Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratio ...
name chemistry final review
... a. 200.0 g C3H6 and 200.0 g of O2 2 C3H6 + 9 O2 → 6 H2O + 6 CO2 O2 is the LR, C3H6 is in excess. There is 141.5g of C3H6 left over and 75.08g H2O and 183.4g CO2 produced. b. 45.9 g CuSO4 and 67.3 g of Fe(C2H3O2)3 3 CuSO4 + 2 Fe(C2H3O2)3 → 3 Cu(C2H3O2)2 + Fe2(SO4)3 CuSO4 is the LR, Fe(C2H3O2)3 is in ...
... a. 200.0 g C3H6 and 200.0 g of O2 2 C3H6 + 9 O2 → 6 H2O + 6 CO2 O2 is the LR, C3H6 is in excess. There is 141.5g of C3H6 left over and 75.08g H2O and 183.4g CO2 produced. b. 45.9 g CuSO4 and 67.3 g of Fe(C2H3O2)3 3 CuSO4 + 2 Fe(C2H3O2)3 → 3 Cu(C2H3O2)2 + Fe2(SO4)3 CuSO4 is the LR, Fe(C2H3O2)3 is in ...
Types of Chemical Reactions
... Convert the grams of each element into the moles of each element with their molar mass. Divide the smallest number of moles of an element into the moles of each element present. Convert the fractional ratios for each element into whole numbers by multiplying all the ratios by the same ...
... Convert the grams of each element into the moles of each element with their molar mass. Divide the smallest number of moles of an element into the moles of each element present. Convert the fractional ratios for each element into whole numbers by multiplying all the ratios by the same ...
File
... credit awarded for correct formulas) Equations must be balanced using the smallest possible whole number coefficients. ( 12 pts, 3,2,3,2,2) a) Magnesium + silver nitrate magnesium nitrate + silver ...
... credit awarded for correct formulas) Equations must be balanced using the smallest possible whole number coefficients. ( 12 pts, 3,2,3,2,2) a) Magnesium + silver nitrate magnesium nitrate + silver ...
CHM 50 Exam 1 Review Name Due Tuesday 9/29/09 Exam 1 will
... b. Potassium chlorate when heated yields potassium chlorate plus oxygen gas. c. An aqueous phosphoric acid solution plus an aqueous calcium hydroxide solution yields water and solid calcium phosphate. 5. A cartain alloy of copper has a density of 3.75g/ml and is 65.0% by mass copper. How many atoms ...
... b. Potassium chlorate when heated yields potassium chlorate plus oxygen gas. c. An aqueous phosphoric acid solution plus an aqueous calcium hydroxide solution yields water and solid calcium phosphate. 5. A cartain alloy of copper has a density of 3.75g/ml and is 65.0% by mass copper. How many atoms ...
PRACTICE – Naming and Writing Ionic Compounds
... Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) 2NaHSO4(aq) + 8HCl(aq) a. How many moles of Na2S2O3 are needed to react with 0.12mol of Cl2? ...
... Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) 2NaHSO4(aq) + 8HCl(aq) a. How many moles of Na2S2O3 are needed to react with 0.12mol of Cl2? ...
CH 5-7 Chapter 5-7 review wkey
... 21. If you need 1.00 L of 0.125 M H2SO4, how would you prepare this solution? a) Add 950. mL of water to 50.0 mL of 3.00 M H2SO4. b) Add 500. mL of water to 500. mL of 0.500 M H2SO4. c) Add 750 mL of water to 250 mL of 0.375 M H2SO4. d) Dilute 36.0 mL of 1.25 M H2SO4 to a volume of 1.00 L. e) Dilute ...
... 21. If you need 1.00 L of 0.125 M H2SO4, how would you prepare this solution? a) Add 950. mL of water to 50.0 mL of 3.00 M H2SO4. b) Add 500. mL of water to 500. mL of 0.500 M H2SO4. c) Add 750 mL of water to 250 mL of 0.375 M H2SO4. d) Dilute 36.0 mL of 1.25 M H2SO4 to a volume of 1.00 L. e) Dilute ...
Section A oxide in molten cryolite?
... Q1 In the extraction of aluminium by electrolysis, why is it necessary to dissolve aluminium oxide in molten cryolite? A to reduce the very high melting point of the electrolyte B cryolite provides the ions needed to carry the current C cryolite reacts with the aluminium oxide to form ions D molten ...
... Q1 In the extraction of aluminium by electrolysis, why is it necessary to dissolve aluminium oxide in molten cryolite? A to reduce the very high melting point of the electrolyte B cryolite provides the ions needed to carry the current C cryolite reacts with the aluminium oxide to form ions D molten ...
the nakuru district sec. schools trial examinations - 2015
... 14 Red-hot iron reacts with steam to give tri-iron tetroxide and hydrogen gas. The reaction is reversible 3Fe(s) + 4H2O(s) Fe304(s) + 4H2(g) (a) Define dynamic equilibrium (1 mark) Although the reaction appears to have stopped by attaining a state of balance, both forward and backward reactions ar ...
... 14 Red-hot iron reacts with steam to give tri-iron tetroxide and hydrogen gas. The reaction is reversible 3Fe(s) + 4H2O(s) Fe304(s) + 4H2(g) (a) Define dynamic equilibrium (1 mark) Although the reaction appears to have stopped by attaining a state of balance, both forward and backward reactions ar ...
Thermodynamics
... We can determine G for any phase by measuring H and S for the reaction creating the phase from the elements We can then determine G at any T and P mathematically Most accurate if know how V and S vary with P and T • dV/dP is the coefficient of isothermal compressibility • dS/dT is the heat capacit ...
... We can determine G for any phase by measuring H and S for the reaction creating the phase from the elements We can then determine G at any T and P mathematically Most accurate if know how V and S vary with P and T • dV/dP is the coefficient of isothermal compressibility • dS/dT is the heat capacit ...
AP Chemistry
... A(g) + B(g) C(g) + D(g) For the gas-phase reaction represented above, the following experimental data were obtained. Exp. Initial [A] Initial [B] ...
... A(g) + B(g) C(g) + D(g) For the gas-phase reaction represented above, the following experimental data were obtained. Exp. Initial [A] Initial [B] ...
Chapter1 - WilsonChemWiki
... CH4 + 2 O2 CO2 + 2 H2O The underlined numbers are used to balance the number of atoms in both sides of the equation. Types of Reactions: (See Reference Table) 1) Synthesis reaction: two or more elements or simple compounds bond together to form product, example: N2 + 2O2 2NO2 2) Decomposition re ...
... CH4 + 2 O2 CO2 + 2 H2O The underlined numbers are used to balance the number of atoms in both sides of the equation. Types of Reactions: (See Reference Table) 1) Synthesis reaction: two or more elements or simple compounds bond together to form product, example: N2 + 2O2 2NO2 2) Decomposition re ...
Review Chapters 4-6 problems Chem 105 Final Sp07
... and multiplying this ratio by 100%. 33. A French scientist named __________ introduced the law of conservation of matter. 34. In the reaction below, how many grams of PF5 can be produced from the reaction of 1.00 g P4 with 1.00 g F2? P4(s) + 10 F2(g) 4 PF5(g) 35. The pH of 1.0 10-5 M HNO3 is ___ ...
... and multiplying this ratio by 100%. 33. A French scientist named __________ introduced the law of conservation of matter. 34. In the reaction below, how many grams of PF5 can be produced from the reaction of 1.00 g P4 with 1.00 g F2? P4(s) + 10 F2(g) 4 PF5(g) 35. The pH of 1.0 10-5 M HNO3 is ___ ...
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.