king fahd university of petroleum and minerals chemistry
... 11. A 20.0 mL sample of 0.150 M ethylamine (CH3CH2NH2) is titrated with 0.0981 M HCl. What is the pH after the addition of 5.0 mL of HCl? For ethylamine, pKb = 3.25. A) B) C) D) ...
... 11. A 20.0 mL sample of 0.150 M ethylamine (CH3CH2NH2) is titrated with 0.0981 M HCl. What is the pH after the addition of 5.0 mL of HCl? For ethylamine, pKb = 3.25. A) B) C) D) ...
Chapter 11 Chemical Reactions
... Symbols used in equations (aq) after the formula = dissolved in water, an aqueous solution: NaCl(aq) is a salt water solution used after a product indicates a gas has been produced: H2↑ used after a product indicates a solid has been produced: PbI2↓ ...
... Symbols used in equations (aq) after the formula = dissolved in water, an aqueous solution: NaCl(aq) is a salt water solution used after a product indicates a gas has been produced: H2↑ used after a product indicates a solid has been produced: PbI2↓ ...
CHEM WKST: EQUILIBRIUM / LE CHATELIER`S PRINCIPLE
... 8) For the reaction: N2(g) + 6HCl(g) ⇄ 2NH3(g) + 3Cl2(g); ΔH = +461 kJ Indicate what happens to [HCl] if the following changes occur. a) More N2 is added. [HCl] ↓ b) Some NH3 is removed. [HCl] ↓ c) The temperature is increased. [HCl] ↓ d) The pressure is lowered. [HCl] ↑ e) The volume of the contain ...
... 8) For the reaction: N2(g) + 6HCl(g) ⇄ 2NH3(g) + 3Cl2(g); ΔH = +461 kJ Indicate what happens to [HCl] if the following changes occur. a) More N2 is added. [HCl] ↓ b) Some NH3 is removed. [HCl] ↓ c) The temperature is increased. [HCl] ↓ d) The pressure is lowered. [HCl] ↑ e) The volume of the contain ...
03. The Theoretic bases of bioenergetics
... It’s denoted by symbol G and is given by ▲G = ▲H - T ▲S where ▲G is the change of Gibbs energy (free energy) This equation is called Gibbs equation and is very useful in predicting the spontaneity of a process. N.B. Gibbs equation exists at constant temperature and pressure ...
... It’s denoted by symbol G and is given by ▲G = ▲H - T ▲S where ▲G is the change of Gibbs energy (free energy) This equation is called Gibbs equation and is very useful in predicting the spontaneity of a process. N.B. Gibbs equation exists at constant temperature and pressure ...
Review for SNC 2P Chemistry Unit(SPRING 2014)
... example: Elements and solutions are pure substances. (a) An atom with more electrons than protons will be a positive ion. (b) A molecular compound is held together with ionic bonds. (c) The chloride ion is an example of a polyatomic ion. (d) The chemical test for hydrogen gas of to use a glowing spl ...
... example: Elements and solutions are pure substances. (a) An atom with more electrons than protons will be a positive ion. (b) A molecular compound is held together with ionic bonds. (c) The chloride ion is an example of a polyatomic ion. (d) The chemical test for hydrogen gas of to use a glowing spl ...
In Class Problems and Notes AP Chemistry General Equilibrium
... pressure P. State whether the partial pressure of NH3(g) will have increased, decreased, or remained the same when equilibrium is reestablished after each of the following disturbances of the original system. Some solid NH4Cl remains in the flask at all times. Justify each answer with a one-or-two s ...
... pressure P. State whether the partial pressure of NH3(g) will have increased, decreased, or remained the same when equilibrium is reestablished after each of the following disturbances of the original system. Some solid NH4Cl remains in the flask at all times. Justify each answer with a one-or-two s ...
Solution
... E) 6 13.) Which of the following statements are true? A) pH of 0.01 M HCl > pH of 0.01 M KOH B) pH of 0.01 M HF > pH of 0.01 M KBr C) pH of 0.01 M NH4Cl > pH of 0.01 M NH3 D) pH of 0.01 M NaCN > pH of 0.01 M CaCl2 14.) A blue advertising signs emits light with a wavelength of 400 nm. Which relations ...
... E) 6 13.) Which of the following statements are true? A) pH of 0.01 M HCl > pH of 0.01 M KOH B) pH of 0.01 M HF > pH of 0.01 M KBr C) pH of 0.01 M NH4Cl > pH of 0.01 M NH3 D) pH of 0.01 M NaCN > pH of 0.01 M CaCl2 14.) A blue advertising signs emits light with a wavelength of 400 nm. Which relations ...
Double Replacement Reactions
... First, if the equation is not complete, write out the correct formulas… 1. Use charges 2. Know the 7 Diatomic Elements: Make sure you know which elements are diatomic so you can write the correct equation. ...
... First, if the equation is not complete, write out the correct formulas… 1. Use charges 2. Know the 7 Diatomic Elements: Make sure you know which elements are diatomic so you can write the correct equation. ...
Nuclear Astrophysics (1)
... a reaction involving particles 1 through 4 (with the C's being integer numbers) is in equilibrium, i.e. the forward and backward reactions occur on timescales shorter than the observing time. Then the following relation holds between the chemical potentials. ...
... a reaction involving particles 1 through 4 (with the C's being integer numbers) is in equilibrium, i.e. the forward and backward reactions occur on timescales shorter than the observing time. Then the following relation holds between the chemical potentials. ...
Electrochemistry primer
... electromotive force. A voltmeter can measure the electromotive force produced by the reaction. Electromotive force (measured in voltage) is a measure of the maximum work that could be released per unit of charge passed through the cell. A volt is a joule (energy) per coulomb (charge). The voltage ge ...
... electromotive force. A voltmeter can measure the electromotive force produced by the reaction. Electromotive force (measured in voltage) is a measure of the maximum work that could be released per unit of charge passed through the cell. A volt is a joule (energy) per coulomb (charge). The voltage ge ...
Chemical Equilibrium - Chemistry with Mrs. Caruso Let the Bonding
... Ex. Suppose there is an equilibrium position described by the concentrations: N2+ 3H2 ⇌ 2NH3 [N2]= .399M; [H2]= 1.197M; [NH3]= .202M What will happen if 1.000 M of N2 is added to the system at constant volume? Will shift to the right. 2. Change in Pressure or Volume: Only for Gases!!!! If _____incre ...
... Ex. Suppose there is an equilibrium position described by the concentrations: N2+ 3H2 ⇌ 2NH3 [N2]= .399M; [H2]= 1.197M; [NH3]= .202M What will happen if 1.000 M of N2 is added to the system at constant volume? Will shift to the right. 2. Change in Pressure or Volume: Only for Gases!!!! If _____incre ...
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 ...
August 30, 2016 Lecture 1: Thermodynamics vs. Statistical Mechanics
... Entropy increases in all spontaneous (irreversible) processes until the maximum is reached for the equilibrium state while the energies (or potentials) are striving for minima. In addition to internal energy, there are other energy forms which can be related to internal energy by Legendre transforma ...
... Entropy increases in all spontaneous (irreversible) processes until the maximum is reached for the equilibrium state while the energies (or potentials) are striving for minima. In addition to internal energy, there are other energy forms which can be related to internal energy by Legendre transforma ...
Exam 1 Key
... K = PCO PH23 / PCH4 PH2O K = (0.18)(0.01)3 / (1)(1) = 1.8 × 10 -‐7 (b) What is ΔG° for this reaction at 600 K? (3 pts) ΔG° = -RT ln K = -(8.314 J mol-1 K-1)(600 K) ln 1.8 × 10-7 = 77.5 kJ mol-1 (c) Is the reaction endothermic or exothermic? Explain how you know. (3 pts) ΔG = ΔH - T ΔS where ΔG a ...
... K = PCO PH23 / PCH4 PH2O K = (0.18)(0.01)3 / (1)(1) = 1.8 × 10 -‐7 (b) What is ΔG° for this reaction at 600 K? (3 pts) ΔG° = -RT ln K = -(8.314 J mol-1 K-1)(600 K) ln 1.8 × 10-7 = 77.5 kJ mol-1 (c) Is the reaction endothermic or exothermic? Explain how you know. (3 pts) ΔG = ΔH - T ΔS where ΔG a ...
Chemical equilibrium
In a chemical reaction, chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. Usually, this state results when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and backward reactions are generally not zero, but equal. Thus, there are no net changes in the concentrations of the reactant(s) and product(s). Such a state is known as dynamic equilibrium.