Homework Answers
![rej = 50 LX 1000 1.0x10 mol/L = 5x105M {Agt ] = 5o LX 1.0x100 mol/L = 5x107m Ksp = 1.8x10lo Q = [Ag+ 3 [4] = = 5x105 x 5 x107](http://img.homeworklib.com/questions/81658400-bcb0-11eb-abf5-191e3efaf858.png?x-oss-process=image/resize,w_560)
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R R=8.314 JK Imola 0%=273.15k (vi) Determine whether a precipitate of AgCl(s) will form on mixing...
From the data table determine the rate law for reactions 1-4 and calculate the value of...
From the data table determine the rate law for reactions 1-4
and calculate the value of k for each. Thanks
I-IV
BACKGROUND
INFORMATION
Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2
Concentration= 0.44 M
•Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M
•Calculation of I^- after mixing for parts I,II, IV= 0.10
M
•Calculation of Initial (mol/L-s)
Filled in Table
Now the solutions for Rate Order and Rate Constant are
needed
Reactants 8 ml 30% HO, 2...
the extra credit problem Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol...
the extra credit problem
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate...
extra credit Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated...
extra credit
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law 1....
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws...
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law 1. You study...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH +...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH + pOH = 14 = pK+pKb [OH (H:0= 10-14 = K, * Ks (in water at 25°C) pH =pK, + log([base)/(acid]) pOH =pKy + log (acid]/[base]) Molar Solubility = (*+ m for a salt that dissociates into ions with coefficients of n and m - b b -4ac where 0 = ax + bx+c VA= A/ X=- 1)...
The first three ionization energies of an element X are 590,1145, and 4912 kJ.mol 1. What...
The first three ionization energies of an element X are 590,1145, and 4912 kJ.mol 1. What is the most likely formula for the stable ion of X? Ох* Ох Ox+ Question 24 (8 points) What is the process to determine the theoretical yield of solid produced when 25.00 mL of 1.00 M silver nitrate and 25.00 mL of 0.100 M calcium chloride are combined? The molar mass of silver chloride is 143.32 g.mol-1 2AgNO3(aq) +CaCl2(aq) -- 2AgCl(s) + Ca(NO3)2(aq) 1.00...
Please I need help on this. I'm so lost 1. Acetic acid (H)CO2H) has k, =...
Please I need help on this. I'm so lost
1. Acetic acid (H)CO2H) has k, = 1.8 x 10- and acetate (H:C:01") has ks = 5.6 x 10-10. (a) Write balanced chemical equilibrium equations (with physical states) for acid dissociation of acetic acid and base hydrolysis of acetate ion. (b) Write K, and equilibrium constant expressions for the above reactions. (c) Use your expressions from part b to show that Kx. = 1.0 x 10-* = [H,O'][OH). 2. For each...
1. Which of the followi ch of the following reactions is not readily explained by the...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids a...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
Please help with solving Question 1 (A-C) Thank you! Unless otherwise specified in the problem, you...
Please help with solving Question 1 (A-C) Thank you!
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. Carbonic acid: Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857...
From the data table determine the rate law for reactions 1-4
and calculate the value of k for each. Thanks
I-IV
BACKGROUND
INFORMATION
Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2
Concentration= 0.44 M
•Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M
•Calculation of I^- after mixing for parts I,II, IV= 0.10
M
•Calculation of Initial (mol/L-s)
Filled in Table
Now the solutions for Rate Order and Rate Constant are
needed
Reactants 8 ml 30% HO, 2...
the extra credit problem
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate...
extra credit
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law 1....
Helpful Stuff Gas Arrhenius Equation: k = Ae-Ea/RT Constant: R= 8.314 J/mol K Integrated Rate Laws and Half-Lives: Zero order: [A] = -kt + [A]. t1/2 =[A]/2k • First order: In[A] = -kt + In[A]. t1/2 = 0.693/k • Second order: 1/[A] = kt + 1/[A] t1/2 = 1/k[A] • Pseudo first order: Use first order integrated rate law for the pseudo-first order reactant; other reactant concentrations remain constant, but are still present in overall rate law 1. You study...
R-0.08206 (atm - L)(mol - K)= 8.314 J/(mol-K) pH = -log[H30) pOH = -log(OH) pX=-logX [HO'] = 10 Ph. K, EK.(RT) pH + pOH = 14 = pK+pKb [OH (H:0= 10-14 = K, * Ks (in water at 25°C) pH =pK, + log([base)/(acid]) pOH =pKy + log (acid]/[base]) Molar Solubility = (*+ m for a salt that dissociates into ions with coefficients of n and m - b b -4ac where 0 = ax + bx+c VA= A/ X=- 1)...
The first three ionization energies of an element X are 590,1145, and 4912 kJ.mol 1. What is the most likely formula for the stable ion of X? Ох* Ох Ox+ Question 24 (8 points) What is the process to determine the theoretical yield of solid produced when 25.00 mL of 1.00 M silver nitrate and 25.00 mL of 0.100 M calcium chloride are combined? The molar mass of silver chloride is 143.32 g.mol-1 2AgNO3(aq) +CaCl2(aq) -- 2AgCl(s) + Ca(NO3)2(aq) 1.00...
Please I need help on this. I'm so lost
1. Acetic acid (H)CO2H) has k, = 1.8 x 10- and acetate (H:C:01") has ks = 5.6 x 10-10. (a) Write balanced chemical equilibrium equations (with physical states) for acid dissociation of acetic acid and base hydrolysis of acetate ion. (b) Write K, and equilibrium constant expressions for the above reactions. (c) Use your expressions from part b to show that Kx. = 1.0 x 10-* = [H,O'][OH). 2. For each...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
Please help with solving Question 1 (A-C) Thank you!
Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. Carbonic acid: Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857...
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