Ch 8 Lecture Notes
... Determine the oxidation numbers for the reactants and compare to the products. Write the oxidation and reduction half-reactions without electrons (yet) Balance everything but oxygen and hydrogen Balance oxygen by adding water Balance hydrogen by adding (a) H+ in acidic solutions, (b) in basic soluti ...
... Determine the oxidation numbers for the reactants and compare to the products. Write the oxidation and reduction half-reactions without electrons (yet) Balance everything but oxygen and hydrogen Balance oxygen by adding water Balance hydrogen by adding (a) H+ in acidic solutions, (b) in basic soluti ...
CHAPTER 4 | Solution Chemistry and the Hydrosphere
... Think about It It is important in the net ionic equation to specify the precipitate as (s). If (aq) is used after the formula for a salt, it implies that the salt is soluble. 4.74. Collect and Organize Silver chloride is an insoluble salt so we can assume that 100% of it precipitates from mixing 10 ...
... Think about It It is important in the net ionic equation to specify the precipitate as (s). If (aq) is used after the formula for a salt, it implies that the salt is soluble. 4.74. Collect and Organize Silver chloride is an insoluble salt so we can assume that 100% of it precipitates from mixing 10 ...
workbook Chem (WP)
... 1. metals that can form more than one value of ionic charge 2. named using the Stock system or the Classical system a. describe each naming system 3. Write the formula for the following: a. copper (I) oxide b. nickel (III) sulfide c. manganese (IV) oxide d. yttrium (III) chloride e. titanium (III) n ...
... 1. metals that can form more than one value of ionic charge 2. named using the Stock system or the Classical system a. describe each naming system 3. Write the formula for the following: a. copper (I) oxide b. nickel (III) sulfide c. manganese (IV) oxide d. yttrium (III) chloride e. titanium (III) n ...
Mr Alasdair Ross at Southpointe Academy
... The Vapour Pressure of a liquid is the partial pressure exerted by its vapor in dynamic equilibrium with liquid at a constant temperature. The Vapour Pressure of a liquid increases with temperature. At a higher temperature more molecules have enough kinetic energy to escape from the liquid state. At ...
... The Vapour Pressure of a liquid is the partial pressure exerted by its vapor in dynamic equilibrium with liquid at a constant temperature. The Vapour Pressure of a liquid increases with temperature. At a higher temperature more molecules have enough kinetic energy to escape from the liquid state. At ...
Answers to Homework Problem Sheet 8
... The temperature change, ΔT = (31.1 °C – 24.6 °C) = 6.7 K. The heat capacity of water is 4.184 J K-1 g-1. The heat change is therefore: q = c × m × ΔT = (4.184 J K-1 g-1) × (199 g) × (6.7 K) = 5600 J or 5.6 kJ (heat released) The number of moles of H+ and OH- present are both the same: number of mole ...
... The temperature change, ΔT = (31.1 °C – 24.6 °C) = 6.7 K. The heat capacity of water is 4.184 J K-1 g-1. The heat change is therefore: q = c × m × ΔT = (4.184 J K-1 g-1) × (199 g) × (6.7 K) = 5600 J or 5.6 kJ (heat released) The number of moles of H+ and OH- present are both the same: number of mole ...
Problem 1 from 2007 form B AP exam
... 3. In a hydrogen-oxygen fuel cell, energy is produced by the overall reaction represented above. (a) When the fuel cell operates at 25qC and 1.00 atm for 78.0 minutes, 0.0746 mol of O2(g) is consumed. Calculate the volume of H2(g) consumed during the same time period. Express your answer in liters m ...
... 3. In a hydrogen-oxygen fuel cell, energy is produced by the overall reaction represented above. (a) When the fuel cell operates at 25qC and 1.00 atm for 78.0 minutes, 0.0746 mol of O2(g) is consumed. Calculate the volume of H2(g) consumed during the same time period. Express your answer in liters m ...
May/Jun 16 Paper 3 - Theory (Core) QP S2
... Which one of the following values is the pH of a strongly alkaline solution? Put a ring around the correct answer. A ...
... Which one of the following values is the pH of a strongly alkaline solution? Put a ring around the correct answer. A ...
AP Chapter 5 Powerpoint
... calorimeter, the temperature of the resultant solution increases from 21.0 oC to 27.5 oC. Calculate the enthalpy change for the reaction in kJ/mol HCl, assuming that the calorimeter loses only a negligible quantity of heat, that the total volume of the solution is 100 mL, that its density is 1.0 g/m ...
... calorimeter, the temperature of the resultant solution increases from 21.0 oC to 27.5 oC. Calculate the enthalpy change for the reaction in kJ/mol HCl, assuming that the calorimeter loses only a negligible quantity of heat, that the total volume of the solution is 100 mL, that its density is 1.0 g/m ...
Critical Micelar Concentration and Thermodynamic Parameters of
... As can be see from Figure 2, the Gibbs free energy appears favorable in all micellization processes that are entropy driven. The SDS shows a favorable enthalpy, which can be attributed to ionic contacts of the polar head-groups. ...
... As can be see from Figure 2, the Gibbs free energy appears favorable in all micellization processes that are entropy driven. The SDS shows a favorable enthalpy, which can be attributed to ionic contacts of the polar head-groups. ...
Chem152
... 49. What is the molecular formula for lactic acid if the percent composition is 40.00% C, 6.71% H, 53.29% O, and the approximate molar mass is 90 g/mol? A) CHO B) CH2O C) CHO2 D) C3H6O3 E) C6HO8 50. How many atoms of nickel equal a mass of 58.69 g? A) 1 B) 27 C) 58.69 D) 59 E) 6.02 × 1023 51. How ma ...
... 49. What is the molecular formula for lactic acid if the percent composition is 40.00% C, 6.71% H, 53.29% O, and the approximate molar mass is 90 g/mol? A) CHO B) CH2O C) CHO2 D) C3H6O3 E) C6HO8 50. How many atoms of nickel equal a mass of 58.69 g? A) 1 B) 27 C) 58.69 D) 59 E) 6.02 × 1023 51. How ma ...
CHEM*130 (F 01) REVIEW QUESTIONS FOR MIDTERM I PAGE
... equations and chemical reaction, sequential reactions, limiting reactants, net ionic equations, gravimetric analysis and volumetric analysis) and (2) thermochemistry (thermochemical equations, standard enthalpy of formation and Hess’s law). These questions are intended to provide you with practice a ...
... equations and chemical reaction, sequential reactions, limiting reactants, net ionic equations, gravimetric analysis and volumetric analysis) and (2) thermochemistry (thermochemical equations, standard enthalpy of formation and Hess’s law). These questions are intended to provide you with practice a ...
Household Acids and Bases Lab
... A visual indicator is a chemical substance that reflects the nature of the chemical system in which it is placed by changing color. Most visual indicators are complex organic molecules that exist in multiple colored forms, one of which could be colorless, depending on the chemical environment. Many ...
... A visual indicator is a chemical substance that reflects the nature of the chemical system in which it is placed by changing color. Most visual indicators are complex organic molecules that exist in multiple colored forms, one of which could be colorless, depending on the chemical environment. Many ...
16. Quantitative volumetric analysis with conductometric detection of
... Conductometry is an electroanalytical method involving the measurement of electrolytic conductivity which value changes with the change of the concentration of ions in solution. Electrolytic conductivity of the solution is due to an electric charge transfer by cations (positive ions) and anions (neg ...
... Conductometry is an electroanalytical method involving the measurement of electrolytic conductivity which value changes with the change of the concentration of ions in solution. Electrolytic conductivity of the solution is due to an electric charge transfer by cations (positive ions) and anions (neg ...
Chapter 2
... • Table salt (sodium chloride or NaCl) is a compound with equal numbers of chlorine and sodium atoms. • While pure sodium is a metal and chlorine is a gas, their combination forms an edible compound, an emergent property. ...
... • Table salt (sodium chloride or NaCl) is a compound with equal numbers of chlorine and sodium atoms. • While pure sodium is a metal and chlorine is a gas, their combination forms an edible compound, an emergent property. ...
Packet #7- Chemical Reactions
... the total mass of products after the reaction is the same as the total mass of the reactants at the start. This fact allows you to work out the mass of one substance in a reaction if the masses of the other substances are known. For example: Carbon reacts with oxygen to form carbon dioxide: C + O2 → ...
... the total mass of products after the reaction is the same as the total mass of the reactants at the start. This fact allows you to work out the mass of one substance in a reaction if the masses of the other substances are known. For example: Carbon reacts with oxygen to form carbon dioxide: C + O2 → ...
p-Block Elements, Part 1
... • It has a valence of 4 (highest in 2nd period) • It can make stable bonds with itself • It can make multiple bonds to C, N, O • The C-H bond is nonpolar, but bonds to other elements (N, O, halogens) are polar This is why life is based on the chemistry of carbon ...
... • It has a valence of 4 (highest in 2nd period) • It can make stable bonds with itself • It can make multiple bonds to C, N, O • The C-H bond is nonpolar, but bonds to other elements (N, O, halogens) are polar This is why life is based on the chemistry of carbon ...
Electrochemistry - Northwest ISD Moodle
... are balanced. There are 3 C, 3 N, 2 H, 9 O, 2 Mn, and a charge of 5− on both sides of the equation. Comment It is important to remember that this procedure does not imply that H + ions are involved in the chemical reaction. Recall that in aqueous solutions at 20 °C, Kw = [H+][OH–] = 1.0 × 10–14. Thu ...
... are balanced. There are 3 C, 3 N, 2 H, 9 O, 2 Mn, and a charge of 5− on both sides of the equation. Comment It is important to remember that this procedure does not imply that H + ions are involved in the chemical reaction. Recall that in aqueous solutions at 20 °C, Kw = [H+][OH–] = 1.0 × 10–14. Thu ...
Chemical Reactions (Part One)
... form copper oxide and carbon dioxide. What is the word equation for this reaction? Why did the mass decrease? The mass decreased because the carbon dioxide gas escaped out into the air. Can you calculate the mass of carbon dioxide that was produced in the reaction? 35 of 40 ...
... form copper oxide and carbon dioxide. What is the word equation for this reaction? Why did the mass decrease? The mass decreased because the carbon dioxide gas escaped out into the air. Can you calculate the mass of carbon dioxide that was produced in the reaction? 35 of 40 ...
Chemical Equations PowerPoint
... of the following, predict the products and write a word equation. Next, write a formula equation and a balanced chemical equation. Finally, write the type of reaction represented by each chemical equation. ...
... of the following, predict the products and write a word equation. Next, write a formula equation and a balanced chemical equation. Finally, write the type of reaction represented by each chemical equation. ...
Standard Half Cell Potentials
... The standard state is defined as a temperature of 298 K and a pressure of 1 bar. Pure substances (solids, liquids and gases) should be in their normal state at this temperature and pressure. Solutions should have an activity* equal to one, which we will approximate here as a concentration equal to 1 ...
... The standard state is defined as a temperature of 298 K and a pressure of 1 bar. Pure substances (solids, liquids and gases) should be in their normal state at this temperature and pressure. Solutions should have an activity* equal to one, which we will approximate here as a concentration equal to 1 ...
Classification of Matter
... Example: Pure water always has the exact same chemical and physical properties under the same conditions. If water ever tastes different then it isn’t pure water; it fits into our next ...
... Example: Pure water always has the exact same chemical and physical properties under the same conditions. If water ever tastes different then it isn’t pure water; it fits into our next ...
Electrolysis of water
Electrolysis of water is the decomposition of water (H2O) into oxygen (O2) and hydrogen gas (H2) due to an electric current being passed through the water.This technique can be used to make hydrogen fuel (hydrogen gas) and breathable oxygen; though currently most industrial methods make hydrogen fuel from natural gas instead.