confused about how to determine the value of x 5. For 2 NO + O2 +...
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...
2. (13 pts) Determine the rate constant and reaction orders for the following reaction using the data provided: 2 NO (g) + 02 (g) > 2 NO2 (g) Rate (M/s 0.028 0.057 0.114 0.227 Experiment NO 0.020 0.020 0.020 0.040 0.010 0.010 0.020 0.040 0.020 0.020 3 4 a.) For the rate law, determine all reaction orders Rate -k [NO]m[O2]' Reaction order m (CIRCLE ONE) 1½ Reaction order n (CIRCLE ONE) 1½
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+ 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
Part A Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O2(g) + 2NO2(9) [NO]; (M) [Ogl (M) Initial Rate (M4 st) 0.030 0.0055 8.55 x 103 0.030 0.0110 1.71 x 10-2 0.0055 3.42 x 10-2 0.060 Rate = 3.1 x 105 M-3 s[NO]2[0212 Rate = 57 M' s'[NO][O21 Rate = 9.4 x 103 M25 *[NO][0212 Rate = 3.8 M-1/2 s [NO](O2) 1/2 Rate = 1.7 x 103 M2 s?[NO]2[02]
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
Show work please. So I know how to apporach problems like these in the future. (2 points) Determine the complete rate law for the following reaction using the data provided. 7. 2 NO(g) +O2(g)2 NO2(g) [NO]i (M) [O2]i (M) Initial Rate (M-Is-I) 0.030 0.030 0.060 0.00558.55 x 10-3 0.01101.71 x 10-2 0.0055 3.42×10-2 What is the initial rate if the concentration of both species is 0.050 M? (1 points) Consider the following reaction: A reaction mixture initially contains 2.24 atm...
1. Consider the reaction 2H2 + O2 + 2H2O What is the ratio of the initial rate of the appearance of water to the initial rate of disappearance of oxygen? a) 1:1 b) 2:1 c) 1:2 d) 2:2 e) 3:2 Garance of water to the initial rate of disappearance of oxyge 2. Consider the reaction X Y Z Which of the following is a possible rate law? a) Rate = k[X] Rate = k[Y] Rate = k[Y][Z] Rate = k[X][Y]...
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...
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...