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The initial rates of reaction between an organic bromide, Y, and hydroxide ion, were measured as...
Please show work. 3. Ammonium ion (NH4*) reacts with nitrite ion (NO2) to yield nitrogen gas...
Please show work.
3. Ammonium ion (NH4*) reacts with nitrite ion (NO2) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Expt. # (NH4+1 [NO2] Initial rate (M/h) 1 0.010 0.020 0.020 2 0.015 0,020 0.030 0.015 0.010 0.0075 Which of the following is the rate law (rate equation) for this reaction? rate - KINH4+ INO214 ratek (NH4+ ][NO2-)-2 rate-k (NH4+ [NO2-) rate - (NH4+ 1*2 [NO2-)
PW 5) Consider the following reaction and the data of initial rates measured using different concentrations...
PW 5) Consider the following reaction and the data of initial rates measured using different concentrations of reactants. [10 pt) 2 NO(g) + O2(g) → 2 NO2(g) [NO]i (M) 0.030 0.030 0.060 [O2li (M) 0.0055 0.0110 0.0055 Initial Rate (Mºs-1) 8.55 x 10-3 1.71 x 10-2 3.42 x 10-2 a) Determine the reaction order of the chemical reaction. [5 pt] b) Calculate the rate constant (k) including the unit and write the rate law of the reaction. TS 1
A student studies the reaction: A - Products. Using the table of initial concentrations and rates...
A student studies the reaction: A - Products. Using the table of initial concentrations and rates below, find the order of the reaction with respect to reactant A. [Alinitial Rate Experiment 1 0.749 M 0.238 M.S! Experiment 2 2.34 M 0.826 M's
28 its Data representing initial concentrations and initial rates for the following reaction are given below....
28 its Data representing initial concentrations and initial rates for the following reaction are given below. Choose the correct rate expression. 20102(aq) + 2OH"(aq) + CIO, (aq) + CO2 (aq) + H2O(1) Exp. No. 1 [CIO2lo (M) 0.060 0.020 0.020 [OH-]o (M) 0.030 0.030 0.090 2 3 Initial Rate (Ms) 0.0248 0.00276 0.00828 rate = k (CIO) (OH)2 ratek (CIO) (OH) rate = k (CIO) [OH-] rate = k [CIO] (OH) ratek (CIO) [OH- Previous ОО Near
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between A and B, aA+bB⇌cC+dD The dependence of the...
57. In a kinetic study of the reaction shown below, the following data were obtained for...
57. In a kinetic study of the reaction shown below, the following data were obtained for the initial rates of Initial Rate of Reaction Initial Concentrations 3.2 x 103 M's 2.9% 104 MS 14x 10 M's 4.8 x 10 M's (a) Determine the order with respect to HgClh algebraically (show your work to receive full credit) Exp. 1 0.164 M Exp. 2 0.164 M Exp. 3 0.082 M Exp. 4 0.246 M 0.15 M 0.45 M 0.45 M 0.15 M...
The reaction between phenolphthalein and hydroxide ion is first order with respect to the phenolphthalein and...
The reaction between phenolphthalein and hydroxide ion is first order with respect to the phenolphthalein and zero order with respect to the hydroxide. Calculate the rate constant for this reaction when the instantaneous rate of reaction is 2.5 x 10-5moles per liter per second for a concentration of 0.00250 M for the phenolphthalein. Group of answer choices a. 0.010 M-1 s-1 b. 2.5 x 10-5M/s c. 0.010 s-1 d. 0.010 M-2 s-1 e. cannot be determined from the given information
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....
For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial [A] (M) [B] (M) [C] (M) Initial rate (M/s) 1 0.40 0.40 0.40 1.2×10−4 2 0.40 0.40 1.20 3.6×10−4 3 0.80 0.40 0.40 4.8×10−4 4 0.80 0.80 0.40 4.8×10−4 Rate law equation The rate of a chemical reaction depends on the concentrations of the reactants. For the general reaction between Aand B, aA+bB⇌cC+dD The dependence of the reaction...
Question 23 3 pts Reaction rates at various initial concentrations of reactants were measured at 900°C...
Question 23 3 pts Reaction rates at various initial concentrations of reactants were measured at 900°C for the following reaction 2NO(g) + 2H2(N) + 2 H2O() Use the data in the table to determine the rate law for the reaction. Initial Rate (M/S) Initial [NO] 0.300 0.150 0.250 Initial [H.] 0.100 0.100 0.200 5.69 x 10-2 1.42 x 10- 7.90 x 10- o Rate - k[NO] Hal o Rate - KINOJH2] o Rate -KINO Hal o Rate =kINO] [Hala Question...
Homework 8-3_1 Reaction Rate Orders, Temp Effects Reaction Rates and Rate Orders The following initial rate...
Homework 8-3_1 Reaction Rate Orders, Temp Effects Reaction Rates and Rate Orders The following initial rate data was collected for the reaction: HI(g) + CHşl(g) à CH.(g) +1-(9) Experiment (HI) (CHI) Initial Rate 0.015 M0.900 M 4.01 x 10M's 0.030 M0.900 M 8.04 x 10'Ms 0.030 M0.450 M 3.99 x 10 m/s 1. What is the rate law for this reaction? a. Rate =k [HI] [CHI] b. Rate = k [HI] [C,H,I] c. Rate = k [HI] (C,H,I] d. Rate...
Please show work.
3. Ammonium ion (NH4*) reacts with nitrite ion (NO2) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Expt. # (NH4+1 [NO2] Initial rate (M/h) 1 0.010 0.020 0.020 2 0.015 0,020 0.030 0.015 0.010 0.0075 Which of the following is the rate law (rate equation) for this reaction? rate - KINH4+ INO214 ratek (NH4+ ][NO2-)-2 rate-k (NH4+ [NO2-) rate - (NH4+ 1*2 [NO2-)
PW 5) Consider the following reaction and the data of initial rates measured using different concentrations of reactants. [10 pt) 2 NO(g) + O2(g) → 2 NO2(g) [NO]i (M) 0.030 0.030 0.060 [O2li (M) 0.0055 0.0110 0.0055 Initial Rate (Mºs-1) 8.55 x 10-3 1.71 x 10-2 3.42 x 10-2 a) Determine the reaction order of the chemical reaction. [5 pt] b) Calculate the rate constant (k) including the unit and write the rate law of the reaction. TS 1
A student studies the reaction: A - Products. Using the table of initial concentrations and rates below, find the order of the reaction with respect to reactant A. [Alinitial Rate Experiment 1 0.749 M 0.238 M.S! Experiment 2 2.34 M 0.826 M's
28 its Data representing initial concentrations and initial rates for the following reaction are given below. Choose the correct rate expression. 20102(aq) + 2OH"(aq) + CIO, (aq) + CO2 (aq) + H2O(1) Exp. No. 1 [CIO2lo (M) 0.060 0.020 0.020 [OH-]o (M) 0.030 0.030 0.090 2 3 Initial Rate (Ms) 0.0248 0.00276 0.00828 rate = k (CIO) (OH)2 ratek (CIO) (OH) rate = k (CIO) [OH-] rate = k [CIO] (OH) ratek (CIO) [OH- Previous ОО Near
57. In a kinetic study of the reaction shown below, the following data were obtained for the initial rates of Initial Rate of Reaction Initial Concentrations 3.2 x 103 M's 2.9% 104 MS 14x 10 M's 4.8 x 10 M's (a) Determine the order with respect to HgClh algebraically (show your work to receive full credit) Exp. 1 0.164 M Exp. 2 0.164 M Exp. 3 0.082 M Exp. 4 0.246 M 0.15 M 0.45 M 0.45 M 0.15 M...
Question 23 3 pts Reaction rates at various initial concentrations of reactants were measured at 900°C for the following reaction 2NO(g) + 2H2(N) + 2 H2O() Use the data in the table to determine the rate law for the reaction. Initial Rate (M/S) Initial [NO] 0.300 0.150 0.250 Initial [H.] 0.100 0.100 0.200 5.69 x 10-2 1.42 x 10- 7.90 x 10- o Rate - k[NO] Hal o Rate - KINOJH2] o Rate -KINO Hal o Rate =kINO] [Hala Question...
Homework 8-3_1 Reaction Rate Orders, Temp Effects Reaction Rates and Rate Orders The following initial rate data was collected for the reaction: HI(g) + CHşl(g) à CH.(g) +1-(9) Experiment (HI) (CHI) Initial Rate 0.015 M0.900 M 4.01 x 10M's 0.030 M0.900 M 8.04 x 10'Ms 0.030 M0.450 M 3.99 x 10 m/s 1. What is the rate law for this reaction? a. Rate =k [HI] [CHI] b. Rate = k [HI] [C,H,I] c. Rate = k [HI] (C,H,I] d. Rate...
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