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1. For the following reaction, H(aq) +1 -2(aq) + 1/2H2O2(aq) → the following reaction data was...
GIVEN THE FOLLOWING DATA FOR THIS REACTION: NH4+(aq) + NO2-(aq) ---> N2(g) + 2H2O(l) EXPT NH4+ NO2- RATE 1 0.010 M 0.020 M 0.020 M/s 2 0.015 M 0.020 M 0.030 M/s 3 0.010 M 0.010 M 0.005 M/s a. Calculate the order of reaction with respect to NH4+ b. Calculate the order of reaction with respect to NO2- c. Calculate the rate constant k d. Determine the overall order of reaction e. Determine the rate law
the following first order reaction has a half life of 22.5 minutes. 2H2O2(aq) 2H2O(l) + O2(g) a. calculate the rate constant for this reaction. b. if the initial concentraition of H2O2 is 0.30M, calculate the amout of H2O2 that reamains after 45 min.
3. For the reaction, H2O2 (aq) + 3 (aq) + 2 H (aq) → 2 H20 (1) + 1- (aq) Ot The rate law was experimentally determined to be Rate = k[H2O2][T] a. What is the reaction order in terms of H20,? b. What is the reaction order in terms of I? because et is nuoto c. What is the reaction order in terms of HT? O d. What is the overall reaction order of this reaction? 4. If a...
The reaction 2H2O2(aq)→2H2O(l)+O2(g) is first order in H2O2 and under certain conditions has a rate constant of 0.00752 s−1 at 20.0 ∘C. A reaction vessel initially contains 150.0 mL of 30.0% H2O2 by mass solution (the density of the solution is 1.11 g/mL). The gaseous oxygen is collected over water at 20.0 ∘C as it forms. What volume of O2 will form in 73.9 seconds at a barometric pressure of 719.5 mmHg . (The vapor pressure of water at this...
QUESTION 9 Use the following information for the reaction: 2 ClO 2(aq) + 2 OH - (aq) → ClO 3-(aq) + ClO 2-(aq) + H 2O(l) Experiment [ClO2] (mol/L) [OH- ] (mol/L) Initial Rate (mol/L-min) i 0.020 0.030 0.00276 ii 0.060 0.030 0.0248 iii 0.020 0.090 0.00828 By what nearest whole number factor does the initial rate change from experiment i to experiment ii? In the analysis of this data would it be useful to compare data for experiment ii...
Question 5 What is AHºp for the following reaction? 2H2O2(1) - 2H2O(1) + O2(g) AH® (H2O(l) = -285.8 kJ/mol, AHºf(H2O2(0) = -187.6 kJ/mol -98.2 kJ/mol @ -473.4 kJ/mol -196.4 kJ/mol 98.2 kJ/mol -946.8 kJ/mol Previous
The decomposition of hydrogen peroxide (H2O2(aq)) is proposed to follow a reaction mechanism of Step 1: H2O2(aq) + Br(aq)-H2O(l) + BrO (aq) Step 2: Bro (aq) + H2O2(aq),H2O(l) + O2(g) + Br(aq) What is the catalyst, and what is the effect of having a catalyst present? Periodic Table and Datasheet Br is the catalyst, and the reaction follows a faster pathway with Br than without BrO is the catalyst, and the reaction follows a faster pathway with Bro-than without Bro...
The following data were obtained for the reaction given below. 2 C102(aq) + 2 OH "(aq) → CIO3- (aq) + ClO2" (aq) + H20(1) Rate - AC10,1 (CIO). (mol/L) (OH), (mol/L) Initial Rate (mol/L's) 0.0500 0.100 5.75 x 10-2 0.100 0.100 2.30 x 10-1 0.100 0.0500 1.15 x 101 (a) Determine the rate law and the value of the rate constant. (Rate equations take the general form 'rate = k. [A] [B]'.) rate law chemPad Help X.X° El Greek rate...
14) You determined the rate law for the reaction of I' with H2O2 in an acidic solution. The rate law was "zero order" with respect to acid ("[H3O+]"). 21+ + H2O2 + 2H+ + 12 + 2 H20 rate = k[I1'[H202] If the conditions are changed to neutral or basic pH, the form of the rate law remains the same but the reaction changes. 2 H2O2 → 2 H2O + O2 rate = k[I+]'[H202] Which statement is TRUE? a) l'...
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...