Practice Test Material - Directorate of Education
... Write the balanced ionic equation for the reaction of potassium dichromate with sodium sulphite to give Cr(III) and sulphate ions. ...
... Write the balanced ionic equation for the reaction of potassium dichromate with sodium sulphite to give Cr(III) and sulphate ions. ...
52.
... Benson,24 the difference in the heats of aquation of HO- and HOO- is 21.5 kcal/mol. Although the existence of such a large solvation effect is not surprising,13 the possibility that this factor alone may be responsible for the alpha-effect seems generally to have been discounted, despite the recogni ...
... Benson,24 the difference in the heats of aquation of HO- and HOO- is 21.5 kcal/mol. Although the existence of such a large solvation effect is not surprising,13 the possibility that this factor alone may be responsible for the alpha-effect seems generally to have been discounted, despite the recogni ...
Topic 9 Oxidation and Reduction Answers - slider-dpchemistry-11
... 9. Why are group 1 and 2 metals such good reducing agents? Group 1 and 2 metals are highly electropositive and readily lose electrons to become positively charged ions (cations) to achieve a full outer shell. Oxidation is a loss of electrons (remember OIL RIG), and if the species is oxidised it must ...
... 9. Why are group 1 and 2 metals such good reducing agents? Group 1 and 2 metals are highly electropositive and readily lose electrons to become positively charged ions (cations) to achieve a full outer shell. Oxidation is a loss of electrons (remember OIL RIG), and if the species is oxidised it must ...
CHM 1033 Chemistry for Health Sciences
... 5. Indicate the number of electronic energy levels (shells). 6. If it is “Representative”, indicate the number of valence electrons (number of electrons located in the outermost energy level). 7. Identify one alkaline metal, one halogen and one noble gas. 8. What’s the tendency of each of these elem ...
... 5. Indicate the number of electronic energy levels (shells). 6. If it is “Representative”, indicate the number of valence electrons (number of electrons located in the outermost energy level). 7. Identify one alkaline metal, one halogen and one noble gas. 8. What’s the tendency of each of these elem ...
File
... 10. Which of the following is true concerning the impact of increasing temperature on reaction rates? a. The number of collisions between reactant atoms is increased. b. The energy of each reactant atom is increased. c. The percentage of collisions with sufficient energy to cross the activation ener ...
... 10. Which of the following is true concerning the impact of increasing temperature on reaction rates? a. The number of collisions between reactant atoms is increased. b. The energy of each reactant atom is increased. c. The percentage of collisions with sufficient energy to cross the activation ener ...
Chapter 11
... • The standard enthalpy of formation (Hfo) is also called the standard heat of formation and is the enthalpy change of the a formation reaction. • A formation reaction is the process of forming 1 mole of a substance in its standard state from its component elements in their standard states. • H2(g) ...
... • The standard enthalpy of formation (Hfo) is also called the standard heat of formation and is the enthalpy change of the a formation reaction. • A formation reaction is the process of forming 1 mole of a substance in its standard state from its component elements in their standard states. • H2(g) ...
Thermodynamics
... -If G<0, the reaction is spontaneous (forward dir.) -If G>0, the reaction is not spontaneous (forward dir.) -If G=0,the reaction is at equilibrium -A reaction is spontaneous in the forward direction only if ΔG is negative. -Spontaneity is controlled by enthalpy and entropy. If ΔH (-) & ΔS (+),the ...
... -If G<0, the reaction is spontaneous (forward dir.) -If G>0, the reaction is not spontaneous (forward dir.) -If G=0,the reaction is at equilibrium -A reaction is spontaneous in the forward direction only if ΔG is negative. -Spontaneity is controlled by enthalpy and entropy. If ΔH (-) & ΔS (+),the ...
05 Halogen deriv. of hydrocarbons. Alcohols,ethers, esters
... ASSAY of thymol (stabilizer) by means of colorimetry, on the basis of reaction with the titan (IV) oxide TiO2, comparing intensity of colouring with a standard solution. Storage. The list of strong substances. In dense corkin bottles (on 50 and 250 ml) from dark glass, in the dry, cool place protec ...
... ASSAY of thymol (stabilizer) by means of colorimetry, on the basis of reaction with the titan (IV) oxide TiO2, comparing intensity of colouring with a standard solution. Storage. The list of strong substances. In dense corkin bottles (on 50 and 250 ml) from dark glass, in the dry, cool place protec ...
O 2 (g) - Valdosta State University
... process, it is _______________. • If only matter is dispersed, then quantitative information is needed to decide whether the process is spontaneous. • If energy is not dispersed after a process occurs, then that process will ____________ _____________________. ...
... process, it is _______________. • If only matter is dispersed, then quantitative information is needed to decide whether the process is spontaneous. • If energy is not dispersed after a process occurs, then that process will ____________ _____________________. ...
x - A Level Tuition
... compared to 1.0 mol dm-3 nitric acid for the same number of moles of water formed. This is because some of the energy evolved from the neutralisation process is used to further dissociate the ethanoic acid completely. ...
... compared to 1.0 mol dm-3 nitric acid for the same number of moles of water formed. This is because some of the energy evolved from the neutralisation process is used to further dissociate the ethanoic acid completely. ...
Unit 6 Interactive Reading Packet File - District 196 e
... water evaporating water freezing 16. Under what conditions does ∆H = q? 17. Which of the following is/are true concerning enthalpy? a) ∆H for a reaction depends upon the states of the reactants and products. b) ∆H (forward reaction) = -∆H (reverse reaction) c) The enthalpy of a system is independent ...
... water evaporating water freezing 16. Under what conditions does ∆H = q? 17. Which of the following is/are true concerning enthalpy? a) ∆H for a reaction depends upon the states of the reactants and products. b) ∆H (forward reaction) = -∆H (reverse reaction) c) The enthalpy of a system is independent ...
Chemistry (B) Final Exam Study Guide 3
... a. They are restricted to metals. c. Two reactants produce two products. b. They involve a single product. d. Any metal replaces any other metal. ____ 70. In the activity series of metals, which metal(s) will displace hydrogen from an acid? a. only metals above hydrogen c. any metal b. only metals b ...
... a. They are restricted to metals. c. Two reactants produce two products. b. They involve a single product. d. Any metal replaces any other metal. ____ 70. In the activity series of metals, which metal(s) will displace hydrogen from an acid? a. only metals above hydrogen c. any metal b. only metals b ...
Chapter 4 Nomenclature and Chemical Equations
... Depending on the type of bonds present in a compound, different rules are applied to its naming. ...
... Depending on the type of bonds present in a compound, different rules are applied to its naming. ...
Rxn Types
... Decomposition of a binary compound When the right energy is applied to a binary compound it will break apart into its respective elements. ...
... Decomposition of a binary compound When the right energy is applied to a binary compound it will break apart into its respective elements. ...
Investigating the kinetic mechanisms of the oxygen
... exists. The formation of Li2O is kinetically limited, and the major discharge product is Li2O2, even at standard potentials more negative than 2.91 V. In theoretical and experimental studies using density functional theory (DFT) and spectroscopic measurements, respectively, Li2O2 production was repo ...
... exists. The formation of Li2O is kinetically limited, and the major discharge product is Li2O2, even at standard potentials more negative than 2.91 V. In theoretical and experimental studies using density functional theory (DFT) and spectroscopic measurements, respectively, Li2O2 production was repo ...
Chap. 6 - Thermodynamics
... 1. How much heat is needed to warm 250 g of water from 22 C to 98 C? What is the molar heat capacity of water? The specific heat of water is 4.18 J/g K. 2. Large beds of rocks are used in some solar-heated homes to store heat. Calculate the quantity of heat absorbed by 50.0 kg of rocks if their te ...
... 1. How much heat is needed to warm 250 g of water from 22 C to 98 C? What is the molar heat capacity of water? The specific heat of water is 4.18 J/g K. 2. Large beds of rocks are used in some solar-heated homes to store heat. Calculate the quantity of heat absorbed by 50.0 kg of rocks if their te ...
Stoichiometry/Mass/Mole Relationships
... 10. ___ C6H12 + ___ O2 → ___ CO2 + ___ H2O 42 grams of cyclohexane burns in excess air to from carbon dioxide and water. How many grams of carbon dioxide and of water vapor are produced? ...
... 10. ___ C6H12 + ___ O2 → ___ CO2 + ___ H2O 42 grams of cyclohexane burns in excess air to from carbon dioxide and water. How many grams of carbon dioxide and of water vapor are produced? ...
Document
... specific heat of the rocks is 0.82 J/g0C. Calculate the quantity of heat absorbed by 50.0kg of rocks if their temperature increases by 12.00C. ...
... specific heat of the rocks is 0.82 J/g0C. Calculate the quantity of heat absorbed by 50.0kg of rocks if their temperature increases by 12.00C. ...
Stoichiometry Regents Unit Review
... Air bags are an important safety feature in modern automobiles. An air bag is inflated in milliseconds by the explosive decomposition of NaN3(s). The decomposition reaction produces N2(g), as well as Na(s), according to the unbalanced equation below. NaN3(s) → Na(s) + N2(g) 20. Balance the equation ...
... Air bags are an important safety feature in modern automobiles. An air bag is inflated in milliseconds by the explosive decomposition of NaN3(s). The decomposition reaction produces N2(g), as well as Na(s), according to the unbalanced equation below. NaN3(s) → Na(s) + N2(g) 20. Balance the equation ...
Chapter 8 and 9 homework
... added to aqueous sodium sulfide to produce solid iron(III) sulfide and aqueous sodium sulfate. 15. What mass of Li3PO4 is needed to prepare 500.0 mL of a solution having a lithium ion concentration of 0.175 M? 16. 17.5 mL of a 0.1050 M Na2CO3 solution is added to 46.0 mL of 0.1250 M NaCl. What is th ...
... added to aqueous sodium sulfide to produce solid iron(III) sulfide and aqueous sodium sulfate. 15. What mass of Li3PO4 is needed to prepare 500.0 mL of a solution having a lithium ion concentration of 0.175 M? 16. 17.5 mL of a 0.1050 M Na2CO3 solution is added to 46.0 mL of 0.1250 M NaCl. What is th ...
Unit D: Quantitative Relationships in Chemical Change
... For each of the following questions, write a balanced chemical equation and then use the mole ratio to answer the question. 1. A student mixes together a solution of silver nitrate with a solution of sodium chromate and a precipitate forms. What amount of precipitate will form if the student has rea ...
... For each of the following questions, write a balanced chemical equation and then use the mole ratio to answer the question. 1. A student mixes together a solution of silver nitrate with a solution of sodium chromate and a precipitate forms. What amount of precipitate will form if the student has rea ...
L22 - Supplementary Student Notes Package
... For each of the following questions, write a balanced chemical equation and then use the mole ratio to answer the question. 1. A student mixes together a solution of silver nitrate with a solution of sodium chromate and a precipitate forms. What amount of precipitate will form if the student has rea ...
... For each of the following questions, write a balanced chemical equation and then use the mole ratio to answer the question. 1. A student mixes together a solution of silver nitrate with a solution of sodium chromate and a precipitate forms. What amount of precipitate will form if the student has rea ...
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.