Chapter 3 Powerpoint
... Sample Exercise 3.20 • Adipic acid, H2C6H8O4, is used to produce nylon. Adipic acid is made by the following reaction: 2C6H12(l) + 5O2(g) 2H2C6H8O4(l) + 2H2O(g) a. Assume that you carry out this reaction starting with 25.0g of cyclohexane and that cyclohexane is the limiting reagent. What is the ...
... Sample Exercise 3.20 • Adipic acid, H2C6H8O4, is used to produce nylon. Adipic acid is made by the following reaction: 2C6H12(l) + 5O2(g) 2H2C6H8O4(l) + 2H2O(g) a. Assume that you carry out this reaction starting with 25.0g of cyclohexane and that cyclohexane is the limiting reagent. What is the ...
Final Review 2006
... d. change in total mass of substances ____ 31. A solid produced by a chemical reaction in solution that separates from the solution is called a. a precipitate. c. a molecule. b. a reactant. d. the mass of the product. ____ 32. After the correct formula for a reactant in an equation has been written, ...
... d. change in total mass of substances ____ 31. A solid produced by a chemical reaction in solution that separates from the solution is called a. a precipitate. c. a molecule. b. a reactant. d. the mass of the product. ____ 32. After the correct formula for a reactant in an equation has been written, ...
Safety - Wando High School
... 2. By balancing an equation what are you making equal on each side? 3. Write out the steps to balancing an equation. 4. Balance the following: KOH + Co3(PO4)2 K3PO4 + Co(OH)2 6 Types of Reactions 1. What are the 6 types of chemical reactions studied? 2. Give a brief explanation as to what happens ...
... 2. By balancing an equation what are you making equal on each side? 3. Write out the steps to balancing an equation. 4. Balance the following: KOH + Co3(PO4)2 K3PO4 + Co(OH)2 6 Types of Reactions 1. What are the 6 types of chemical reactions studied? 2. Give a brief explanation as to what happens ...
NYOS Charter School
... 14. Which of the following is true of equilibria reactions in chemistry? a. reactions with a large, positive Keq proceed very quickly b. all particle movement stops when equilibrium is reached c. particles are continuously moving back and forth between reactants and products d. the state of equilibr ...
... 14. Which of the following is true of equilibria reactions in chemistry? a. reactions with a large, positive Keq proceed very quickly b. all particle movement stops when equilibrium is reached c. particles are continuously moving back and forth between reactants and products d. the state of equilibr ...
Conservation of Mass Lab
... the left side and only one on the right side, so place a coefficient of 3 in front of calcium sulfate. Now deal with the aluminum. You have three on the left and one on the right, so place a coefficient of 2 in front of aluminum chloride. Last, you must place a coefficient of 3 in front of calcium c ...
... the left side and only one on the right side, so place a coefficient of 3 in front of calcium sulfate. Now deal with the aluminum. You have three on the left and one on the right, so place a coefficient of 2 in front of aluminum chloride. Last, you must place a coefficient of 3 in front of calcium c ...
Chapter 5 CHEM 121
... BALANCED CHEMICAL EQUATIONS • A balanced chemical equation is one in which the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products. • A reaction can be balanced by applying the law of conservation of matter. • Coefficients (in red be ...
... BALANCED CHEMICAL EQUATIONS • A balanced chemical equation is one in which the number of atoms of each element in the reactants is equal to the number of atoms of that same element in the products. • A reaction can be balanced by applying the law of conservation of matter. • Coefficients (in red be ...
Bonding 1. Which one of the following is most likely to be an ionic
... 7. Consider the following gas-phase equilibrium: H2(g) + I2(g) ↔ 2HI(g) At a certain temperature, the equilibrium constant Kc is 4.0. Starting with equimolar quantities of H2 and I2 and no HI, when equilibrium was established, 0.20 moles of HI was present. How much H2 was used to start the reaction ...
... 7. Consider the following gas-phase equilibrium: H2(g) + I2(g) ↔ 2HI(g) At a certain temperature, the equilibrium constant Kc is 4.0. Starting with equimolar quantities of H2 and I2 and no HI, when equilibrium was established, 0.20 moles of HI was present. How much H2 was used to start the reaction ...
rp oc4
... 10. Suppose a g is collected in 145 mL flask whef-tfle temperature of the gas is 23°C and the pressure of the gas is 785 mm Hg. Calculate the volume of the gas at STP. .1.38432.m.L ...
... 10. Suppose a g is collected in 145 mL flask whef-tfle temperature of the gas is 23°C and the pressure of the gas is 785 mm Hg. Calculate the volume of the gas at STP. .1.38432.m.L ...
quarter 4 final exam guide - District 196 e
... (3.78 L) of 18.0 M H2SO4. How would you make 1.5 liters of 6.0 M H2SO4 from the 18.0 M H2SO4? ...
... (3.78 L) of 18.0 M H2SO4. How would you make 1.5 liters of 6.0 M H2SO4 from the 18.0 M H2SO4? ...
Chemical Reactions PPT
... type of atom on the reactants side of the chemical equation MUST be equal to the number of each type of atom on the products side of the equation. • Coefficient-represent the number of units of each substance taking part in the reaction ...
... type of atom on the reactants side of the chemical equation MUST be equal to the number of each type of atom on the products side of the equation. • Coefficient-represent the number of units of each substance taking part in the reaction ...
balancing eqns teacher
... All chemical equations have reactants and products. We express a chemical equation as follows: ...
... All chemical equations have reactants and products. We express a chemical equation as follows: ...
Practice Exam #2
... A) The system loses heat and has work done on it by the surroundings. B) The system loses heat and does work on the surroundings. C) The system gains heat and does work on the surroundings. D) The system gains heat and has work done on it by the surroundings. E) None of the above is correct. ...
... A) The system loses heat and has work done on it by the surroundings. B) The system loses heat and does work on the surroundings. C) The system gains heat and does work on the surroundings. D) The system gains heat and has work done on it by the surroundings. E) None of the above is correct. ...
PHT-224 Lectures 6
... Special Case Apparent zero order of reaction In aqueous suspensions of drugs, as the dissolved drug decomposes more drug dissolve to maintain drugconcentration i.e. drug concentration kept constant, once all undissolved drug is dissolved, rate becomes first order. ...
... Special Case Apparent zero order of reaction In aqueous suspensions of drugs, as the dissolved drug decomposes more drug dissolve to maintain drugconcentration i.e. drug concentration kept constant, once all undissolved drug is dissolved, rate becomes first order. ...
Advanced Placement Chemistry Test
... equal to, or less than the initial concentration of HI(g). Justify your answer. {3 marks} ...
... equal to, or less than the initial concentration of HI(g). Justify your answer. {3 marks} ...
Section 2 Types of Chemical Reactions Chapter 8
... known as the reactants and the resulting substances are known as the products. • According to the law of conservation of mass, the total mass of reactants must equal the total mass of products for any given chemical reaction. ...
... known as the reactants and the resulting substances are known as the products. • According to the law of conservation of mass, the total mass of reactants must equal the total mass of products for any given chemical reaction. ...
chemical reactions
... 1. A balanced chemical reaction- both sides of equation have the same number of atoms of each element ...
... 1. A balanced chemical reaction- both sides of equation have the same number of atoms of each element ...
Exam practice answers
... The total enthalpy change is (+425 + 470 + 416 + 335) = +1646 kJ mol−1, which is the enthalpy change when four C−H bonds are broken in methane and, therefore, the enthalpy change when one C−H bond is broken is +1646/4 = 411.5 kJ mol−1. (c) ...
... The total enthalpy change is (+425 + 470 + 416 + 335) = +1646 kJ mol−1, which is the enthalpy change when four C−H bonds are broken in methane and, therefore, the enthalpy change when one C−H bond is broken is +1646/4 = 411.5 kJ mol−1. (c) ...
