For the reaction: CH3OH (aq) + H3O+ (aq) + Cl-(aq) --> CH3Cl + 2 H2O (l)...
For the reaction:
CH3OH (aq) + H3O+ (aq) + Cl-(aq) --> CH3Cl + 2 H2O (l)
The concentration of acid decreases from 2.23 M to 1.89 M in 64.0 s.
- Calculate the average rate of disappearance of acid
- Calculate the average rate of appearance of CH3Cl
- Calculate the average rate of appearance of H2O
Homework Answers
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For the reaction:
CH3OH (aq) + H3O+ (aq) +
Cl-(aq) --> CH3Cl + 2 H2O (l)...
For the reaction below, the concentration of iodide ion decreases from 1.000 M to 0.868 M...
For the reaction below, the concentration of iodide ion decreases from 1.000 M to 0.868 M in the first 10.0 s. H2O2 (aq) + 3I-1 (aq)+ 2H+ (aq) --> I3-1 (aq) + 2 H2O (l) Calculate the average rate for the disappearance of I-1 Calculate the average rate of appearance for I3-1 Calculate the average rate of disappearance of H+
For the reaction CH3OH(aq) + Cl-(aq) <--> CH3Cl(aq) + OH-(aq) , K = 3.4 x 10-15...
For the reaction CH3OH(aq) + Cl-(aq) <--> CH3Cl(aq) + OH-(aq) , K = 3.4 x 10-15 at a particular temperature. What can be said about the relative energies of products and reactants? Group of answer choices products must be more stable products and reactants must be of nearly equal stabilities no way to determine without more information reactants must be more stable
For the reaction [H](M) 2.36 CH, OH(aq) + H+ (aq) + C- (aq) CH, Cl(aq) +...
For the reaction [H](M) 2.36 CH, OH(aq) + H+ (aq) + C- (aq) CH, Cl(aq) + H2O(1) the value of [H*] was measured over a period of time. Given the data in the table, find the average rate of disappearance of H+ (aq) for the time interval between each measurement. Interval: Os to 34.0 1 (s) 0 34.0 57.0 2.14 2.02 120.0 1.85 reaction rate: M/S Interval: 34.0 sto 57,0 s reaction rate: M/s Interval: 57.0 s to 120.0 s...
For the following reaction: CH_3 OH(aq) + H^+ (aq) + Cl^- (aq) rightarrow CH_3Cl(aq) + H_2O(l)...
For the following reaction: CH_3 OH(aq) + H^+ (aq) + Cl^- (aq) rightarrow CH_3Cl(aq) + H_2O(l) the value of [H^+] was measured over a period of time. Given the data, find the average rate of disappearance of H^+(aq) for the time interval between each measurement. What is the average rate of appearance of CH_3 CI(aq) for the same time intervals?
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O...
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O (l) A 1.0 L buffer solution is 0.280 M in HC2H302 (acetic acid) and 0.320 M in NaC2H302 (sodium acetate). Calculate the pH of the budder and he Ka for HC2H3O2 IS 1.8 X 10-5 Calculate the pH of te solution above after the addition of 0.0400 moles of solid NaOH. Assume no volume change upon the addition of base.
3. Consider the following general reaction, at room temperature: HClO2 (aq) + H2O (l) ⇌ H3O+(aq)...
3. Consider the following general reaction, at room temperature: HClO2 (aq) + H2O (l) ⇌ H3O+(aq) + ClO2–(aq) Ka = 1.2 x 10-2 Initially, a reaction contained 0.100 M HClO2 then it reached equilibrium. Set up an ICE table to calculate the [H3O+(aq)]. Using the “x is small approximation”, which of the following best describes the calculated percentage change in the initial amount of acid? A) 3.46% B) 34.6% C) 12.0% D) 28.9%
Write the following as a net ionic equation: HCl(aq) + H2O(l) → H3O+(aq) + Cl −(aq)
Write the following as a net ionic equation: HCl(aq) + H2O(l) → H3O+(aq) + Cl −(aq)
HBrO (aq) + H2O (l) ⇋ H3O+ (aq) + BrO- (aq) If the value of Kc...
HBrO (aq) + H2O (l) ⇋ H3O+ (aq) + BrO- (aq) If the value of Kc for this process is 5.2 x 10-5, there is no H3O+ or BrO- initially present, and the initial [HBrO] = 0.354 M, what will be the concentration of BrO- at equilibrium?
Consider the following reaction: HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq) Kc=1.8×10−5 at 25∘C If a solution initially contains 0.180 M HC2H3O2,...
Consider the following reaction: HC2H3O2(aq)+H2O(l)⇌H3O+(aq)+C2H3O−2(aq) Kc=1.8×10−5 at 25∘C If a solution initially contains 0.180 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25∘C? Express your answer using two significant figures.
1. Butyl chloride, C.H.CI, reacts with water to form butyl alcohol, C.H.OH. CH,Cl (aq) + H2O...
1. Butyl chloride, C.H.CI, reacts with water to form butyl alcohol, C.H.OH. CH,Cl (aq) + H2O (1) - C.H.OH(aq) + HCl(aq) If the initial concentration of butyl chloride is 0.1000 M and the concentration after 50 s of reaction is 0.0905 M, calculate the average rate of reaction (at the start of the reaction, i.e., the initial rate).
For the reaction [H](M) 2.36 CH, OH(aq) + H+ (aq) + C- (aq) CH, Cl(aq) + H2O(1) the value of [H*] was measured over a period of time. Given the data in the table, find the average rate of disappearance of H+ (aq) for the time interval between each measurement. Interval: Os to 34.0 1 (s) 0 34.0 57.0 2.14 2.02 120.0 1.85 reaction rate: M/S Interval: 34.0 sto 57,0 s reaction rate: M/s Interval: 57.0 s to 120.0 s...
For the following reaction: CH_3 OH(aq) + H^+ (aq) + Cl^- (aq) rightarrow CH_3Cl(aq) + H_2O(l) the value of [H^+] was measured over a period of time. Given the data, find the average rate of disappearance of H^+(aq) for the time interval between each measurement. What is the average rate of appearance of CH_3 CI(aq) for the same time intervals?
1. Butyl chloride, C.H.CI, reacts with water to form butyl alcohol, C.H.OH. CH,Cl (aq) + H2O (1) - C.H.OH(aq) + HCl(aq) If the initial concentration of butyl chloride is 0.1000 M and the concentration after 50 s of reaction is 0.0905 M, calculate the average rate of reaction (at the start of the reaction, i.e., the initial rate).
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