![SECTION B (Open ended) 1. Given the following data for this reaction: NH (B) + NO2 aa = N2 + 2H2O) EXPT INHE] [NO:) RATE 0](http://img.homeworklib.com/questions/7376ca80-142a-11ea-aaa5-571a9b00af30.png?x-oss-process=image/resize,w_560)
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SECTION B (Open ended) 1. Given the following data for this reaction: NH" (B) + NO2 aa = N2 + 2H2O) EXPT INHE...
GIVEN THE FOLLOWING DATA FOR THIS REACTION: NH4+(aq) + NO2-(aq) ---> N2(g) + 2H2O(l) EXPT NH4+...
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
13.13 The rate law for the reaction NH+ (aq) + NO3(aq) = N2(g) + 2H2O(1) is given by rate = k [NH 1 [NO2). At 25°C,...
13.13 The rate law for the reaction NH+ (aq) + NO3(aq) = N2(g) + 2H2O(1) is given by rate = k [NH 1 [NO2). At 25°C, the rate constant is 3.0 x 10 */M. s. Calculate the rate of the reaction at this temperature if [NH] = 0.26 M and [NO2] = 0.080 M.
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-)
please help me all question in this picture Q. 6. Given the following data for the...
please help me all question in this picture
Q. 6. Given the following data for the NH+NO,N2+2H,0 reaction: Trial [NH4+] [NOS] Rate 0.010 M 0.020 M 0.020 M/s 2 0.015 0.020 0.030 3 0.010 0.010 0.005 The rate law for the reaction is: b) rate k[NH NOT d) rate k[NH NO1 a) rate kINH4 TINO21 c) rate kNH4TNO:1 Q. 7. When a catalyst is used in a reaction, a) the forward reaction is increased while the reverse reaction is retarded....
The rate law for the reaction NH4+(aq) + NO2−(aq) → N2(g) + 2H2O(l) is given by...
The rate law for the reaction NH4+(aq) + NO2−(aq) → N2(g) + 2H2O(l) is given by rate = k[NH4+][NO2−]. At a certain temperature, the rate constant is 3.80 × 10−4 /M·s. Calculate the rate of the reaction at that temperature if [NH4+] = 0.261 M and [NO2−] = 0.160 M. × 10 M/s Enter your answer in scientific notation.
QUESTION 6 From the following data, the reaction order for Ais___and the reaction order for Bis...
QUESTION 6 From the following data, the reaction order for Ais___and the reaction order for Bis A Second order for A: first order for B B. zero order for Azero order for B C. zero order for Afirst order for B D. first order for As first order for B E. None of the answers are correct. QUESTION 7 You are trying to determine the reaction rate for a reaction with several intermediate steps. The rate for the overall reaction...
Consider the reaction of ammonium ions (NH and nitrite ions (NO2), shown in Equation 1. NH...
Consider the reaction of ammonium ions (NH and nitrite ions (NO2), shown in Equation 1. NH (aq) +NO2 (aq)N2 (g +2H O 0) Solutions of NH4 and NO2 were mixed in various quantities and the following rate data were obtained at a constant temperature: Experiment Initial [NH4 Initial [NO2] Initial rate for formation of N2 moVL s 3.04 x 10 6.08 x 10 1.22 x 10 0.1507.50 x 10 0.1501.50 102 0.300 1.50x 10 1. Find the order of the...
1. For the following reaction, H(aq) +1 -2(aq) + 1/2H2O2(aq) → the following reaction data was...
1. For the following reaction, H(aq) +1 -2(aq) + 1/2H2O2(aq) → the following reaction data was obtained: 42 12 (aq) + H20 1-1 (mol/L) H2O2(mol/L) Rate(mol/L*min) Expt. #1 0.015 0.030 0.0022 Expt. #2 0.035 0.030 0.0052 Expt. #3 0.055 0.030 0.0082 Expt. #4 0.035 0.050 0.0087 A. Determine the order of the two reactants(1'1 and H202) and the over all order. His a catalyst and is not included in the rate expression. B. Write the rate expression for the reaction...
Consider the reaction: 2 NO(g) + O2 (g)--> 2 NO2 (g) The following data were obtained...
Consider the reaction: 2 NO(g) + O2 (g)--> 2 NO2 (g)
The following data were obtained from three experiments using
the method of initial rates:
3. Consider the reaction: 2 NO(g) + O2(g) → 2 NO2(g) The following data were obtained from three experiments using the method of initial rates: Initial [NO] Initial rate NO Initial [02] mol mol L-1 mol L-1 L-15-1 0.010 0.010 Experiment 1 Experiment 2 Experiment 3 0.020 0.010 2.5 x 10-5 1.0 x 10-4 5.0...
1a. The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g)...
1a. The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second order with respect to NO(g) and first order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.6 x 102 M–2 s–1. When the initial concentrations of NO and O2 are 0.02 M and 0.015 M, respectively, the rate of the reaction is ___ M/s. 1b. The rate constant of a first-order decomposition reaction is 0.014...
13.13 The rate law for the reaction NH+ (aq) + NO3(aq) = N2(g) + 2H2O(1) is given by rate = k [NH 1 [NO2). At 25°C, the rate constant is 3.0 x 10 */M. s. Calculate the rate of the reaction at this temperature if [NH] = 0.26 M and [NO2] = 0.080 M.
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-)
please help me all question in this picture
Q. 6. Given the following data for the NH+NO,N2+2H,0 reaction: Trial [NH4+] [NOS] Rate 0.010 M 0.020 M 0.020 M/s 2 0.015 0.020 0.030 3 0.010 0.010 0.005 The rate law for the reaction is: b) rate k[NH NOT d) rate k[NH NO1 a) rate kINH4 TINO21 c) rate kNH4TNO:1 Q. 7. When a catalyst is used in a reaction, a) the forward reaction is increased while the reverse reaction is retarded....
QUESTION 6 From the following data, the reaction order for Ais___and the reaction order for Bis A Second order for A: first order for B B. zero order for Azero order for B C. zero order for Afirst order for B D. first order for As first order for B E. None of the answers are correct. QUESTION 7 You are trying to determine the reaction rate for a reaction with several intermediate steps. The rate for the overall reaction...
Consider the reaction of ammonium ions (NH and nitrite ions (NO2), shown in Equation 1. NH (aq) +NO2 (aq)N2 (g +2H O 0) Solutions of NH4 and NO2 were mixed in various quantities and the following rate data were obtained at a constant temperature: Experiment Initial [NH4 Initial [NO2] Initial rate for formation of N2 moVL s 3.04 x 10 6.08 x 10 1.22 x 10 0.1507.50 x 10 0.1501.50 102 0.300 1.50x 10 1. Find the order of the...
1. For the following reaction, H(aq) +1 -2(aq) + 1/2H2O2(aq) → the following reaction data was obtained: 42 12 (aq) + H20 1-1 (mol/L) H2O2(mol/L) Rate(mol/L*min) Expt. #1 0.015 0.030 0.0022 Expt. #2 0.035 0.030 0.0052 Expt. #3 0.055 0.030 0.0082 Expt. #4 0.035 0.050 0.0087 A. Determine the order of the two reactants(1'1 and H202) and the over all order. His a catalyst and is not included in the rate expression. B. Write the rate expression for the reaction...
Consider the reaction: 2 NO(g) + O2 (g)--> 2 NO2 (g)
The following data were obtained from three experiments using
the method of initial rates:
3. Consider the reaction: 2 NO(g) + O2(g) → 2 NO2(g) The following data were obtained from three experiments using the method of initial rates: Initial [NO] Initial rate NO Initial [02] mol mol L-1 mol L-1 L-15-1 0.010 0.010 Experiment 1 Experiment 2 Experiment 3 0.020 0.010 2.5 x 10-5 1.0 x 10-4 5.0...
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