For this reaction general expression of rate law ::
Rate = k [NO]x [H2]y
==
form 1 and 2nd data set :
rate 2 / rate 1 = 4 = k [0.2]x [0.1]y /k [0.1]x [0.1]y
2x = 4 ===> x = 2
and
form 1 and 3 data set :
rate 3 / rate 1 = 2 = k [0.1]x [0.2]y /k [0.1]x [0.1]y
2y = 2 ===> y = 1
thus,
Rate = k [NO]2 [H2]
4. Suppose the following data is obtained for the reaction: 2NO(g)+2H2(g) → N2(g)+2H20(g) [NO] [Hz] Rate...
The following initial rate information was collected at 25°c for the following reaction: 2H2(g)+2NO(g) N2(g) +2H20(g) H2lo (M) INOlo (M) Initial Rate (M/min) 0.0010 0.0020 1.2 x 10-4 0.0010 0.0030 1.8 x 104 0.0020 0.0020 4.8 x 104 Determine the overall order of the reaction and present you answer in numeric torm (le. 0, 1,2 eto)
Hydrogen gas reduces NO to N2 in the following reaction: 2H2(g) + 2NO(g) + 2H20(g) +N_(8) The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2lo (M) [NO] (M) Initial Rate (M/s) 1 0.212 0.136 0.0275 2 0.212 0.272 0.0553 3 0.424 0.544 0.435 0.848 0.544 1.75 4 Determine the rate constant for the reaction at 1500°C. M-xs-1
A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) → N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? O k[no]/2[Hz] O k[N20][H2] O k[NO]2 O k[NO]2[Hz] O k[NO]2[H212
3. The reaction rate of the gas-phase reaction 2NO+2H2 → N2 + 2H2O was measured for several different initial pressures of the reactants. Determine the rate equation and thence the rate constant. [Hz] /mM [NO] /mM 26 20 26 d[N2]/dt /Ms? 6.17 x 10-S 1.57 x 10-5 7.59 x 10-5 1.14 104 10.1 26 26 19 28.5
The rate law for the reaction 2H2(g) + 2NO(g) ----> N2(g) + 2H2O(g) is rate=k[H2][NO]2. What is the rate constant at 800 degrees C when [NO] = 0.050 M and [H2] = 0.010 M and the rate of the reaction is 1.5 M/s
What is the overall order of the following reaction 2NO+Hz >N2 + 2H20 Ratér k po]Cz]
Need help with part 2 Hydrogen gas reduces NO to N2 in the following reaction: 2H2(g) +2NO(g) + 2H20(g) +N2(g) The initial reaction rates of four mixtures of Hy and NO were measured at 1500°C with the following results: Experiment (H2lo (M) [NO], (M) Initial Rate (M/s) 1 0.212 0.136 0 .0225 0.212 0.272 0.0453 0.424 0.544 0.355 0.848 10.544 1.43 V 3rd attempt Part 1 (1 point) W See Periodic Table Choose the correct rate law for the reaction...
N2 (g) + O2 (g) --> 2NO (g) The following data was recorded: Exper [N2] [O2] Rate 1 0.04 0.02 707 mol/Lsec 2 0.04 0.01 500 mol/Lsec 3 0.01 0.01 125 mol/Lsec Determine the rate law.
1) 2) 3) A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) N20(g) + H20(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) +H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO2 Ok[NO]2[H212 O k[NO]2[H2] Ok[N20][H2] k[NO]1/2[H2] 2NO(g) +Cl2 (g) → NOCI (8) Experiment concentration of NO (M) 0.09 0.045 0.045 concentration of Cl2(M) Rate (M/s) 0.01 3.40 x 10-4 8.50 x...
2. Good question. The reaction 2NO(g) + O2(g) → 2NO.(g) was studied by a CHEM 154 student and the following data were obtained for the rate of consumption of oxygen. Write the rate law for this reaction. What would be the initial rate for an experiment where [NO), = 1.03 x 10-mol/L and [O),= 1.22 x 102 mol/L? Expt. [NO], (M) (01. (M) Initial rate (M/s) 1 1.66 x 10-3 1.66 x 10-3 3.32 x 10-5 2 4.98 x 10-...