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Ammonium ion reacts slowly with nitrite ion: NH4+ (aq) + NO2(aq) → N2(g) + 2H20(1) Rate...
Ammonium ion reacts slowly with nitrite ion: NH4+ (aq) + NO2(aq) + N2(g) + 2H20(1) Rate...
Ammonium ion reacts slowly with nitrite ion: NH4+ (aq) + NO2(aq) + N2(g) + 2H20(1) Rate data for this reaction, measured at a certain temperature, are as follows: Expt. (NH4+] (M) [NO] (M) Rate (MSP) 1 10.1200 .300 5.20 x 106 2 0.480 0.300 2.08 x 105 3 0.480 0.150 1.04 x 105 (a) Determine the rate law for the reaction. Enter your result in the equation below, by putting the appropriate exponent next to each species. (Enter of the...
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-)
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
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.
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2(g) + H20 (1) Experiment (NH4+) (N...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2(g) + H20 (1) Experiment (NH4+) (NO2). Initial rate (m/s) AWN + 0.24 0.10 0.12 0.10 0.120.15 0.12 0.12 7.2 x 10-4 3.6 x 104 5.4 x 10-4 4.3 x 10-4 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate [NH4+) at 114 seconds after the start of the reaction. In this experiment, both...
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial ra...
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial rate (M/s) 0.10 0.24 7.2 x 104 1 0.10 0.12 3.6 x 104 0.12 0.15 5.4 x 104 0.12 0.12 4.3 x 104 4 First determine the rate law and rate constant Under the same initial conditions as in Experiment 4, calculate [NH4 ] at 368 seconds after the start of the reaction. In this experiment, both reactants are present at the...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq)...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) → N2 (g) + H20 (1) AWNA Experiment (NH4+1: [NO2). Initial rate (M/s) 0.24 0.10 17.2 x 10-4 0.12 0.10 13.6 x 10-4 0.15 15.4 x 10-4 0.12 0.12 4.3 x 10-4 0.12 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate (NH4+] at 103 seconds after the start of the reaction. In this experiment,...
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...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2- (aq)...
Initial rate data are listed in the table for the
reaction:
NH4+ (aq) + NO2- (aq) →
N2 (g) + H2O (l)
First determine the rate law and rate constant.
Under the same initial conditions as in Experiment
4, calculate [NH4+] at 184 seconds after
the start of the reaction. In this experiment, both reactants are
present at the same initial concentration.
The units should be M, and should be calculated to
three significant figures.
1:26 Bb Bb # ....
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.
Ammonium ion reacts slowly with nitrite ion: NH4+ (aq) + NO2(aq) + N2(g) + 2H20(1) Rate data for this reaction, measured at a certain temperature, are as follows: Expt. (NH4+] (M) [NO] (M) Rate (MSP) 1 10.1200 .300 5.20 x 106 2 0.480 0.300 2.08 x 105 3 0.480 0.150 1.04 x 105 (a) Determine the rate law for the reaction. Enter your result in the equation below, by putting the appropriate exponent next to each species. (Enter of the...
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-)
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) + N2(g) + H20 (1) Experiment (NH4+) (NO2). Initial rate (m/s) AWN + 0.24 0.10 0.12 0.10 0.120.15 0.12 0.12 7.2 x 10-4 3.6 x 104 5.4 x 10-4 4.3 x 10-4 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate [NH4+) at 114 seconds after the start of the reaction. In this experiment, both...
Initial rate data are listed in the table for the reaction NH4t (aq)NO2 (aq)N2 (g)H20 () Experiment [NH4+[NO2Initial rate (M/s) 0.10 0.24 7.2 x 104 1 0.10 0.12 3.6 x 104 0.12 0.15 5.4 x 104 0.12 0.12 4.3 x 104 4 First determine the rate law and rate constant Under the same initial conditions as in Experiment 4, calculate [NH4 ] at 368 seconds after the start of the reaction. In this experiment, both reactants are present at the...
Initial rate data are listed in the table for the reaction: NH4+ (aq) + NO2 (aq) → N2 (g) + H20 (1) AWNA Experiment (NH4+1: [NO2). Initial rate (M/s) 0.24 0.10 17.2 x 10-4 0.12 0.10 13.6 x 10-4 0.15 15.4 x 10-4 0.12 0.12 4.3 x 10-4 0.12 First determine the rate law and rate constant. Under the same initial conditions as in Experiment 4, calculate (NH4+] at 103 seconds after the start of the reaction. In this experiment,...
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...
Initial rate data are listed in the table for the
reaction:
NH4+ (aq) + NO2- (aq) →
N2 (g) + H2O (l)
First determine the rate law and rate constant.
Under the same initial conditions as in Experiment
4, calculate [NH4+] at 184 seconds after
the start of the reaction. In this experiment, both reactants are
present at the same initial concentration.
The units should be M, and should be calculated to
three significant figures.
1:26 Bb Bb # ....
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.
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