Hydrogen gas reduces NO to N2 in the following reaction: 2H2(g) + 2NO(g) + 2H20(g) +N_(8)...
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...
Hydrogen gas reduces NO to N2 in the following reaction: 2H,(8) + 2NO(g) – 2H,0 (8) #N, (g) The initial reaction rates of four mixtures of H2 and NO were measured Experiment [H2) (M) [NO]. (M) Initial Rate (M/s) 0.212 0.136 0.0315 0.212 0.272 0.0633 0.424 0.544 0.499 0.848 0.544 2.00 1st attempt Part 2 (0.5 point) Feedback Determine the rate constant for the reaction at 1500°C. * .85 M *-1 14' >
what is the correct rate law for the reaction at 1500 C
determine the rate constant for the reaction at 1500C
Hydrogen gas reduces NO to N2 in the following reaction: 2H2 (g) +2NO(&2H20(g)N2() The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C with the following results: Experiment [H2lo (M) [NOlo (M) Initial Rate (M/s) 2 3 4 0.212 0.212 0.424 0.848 0.136 0.272 0.544 0.544 0.0265 0.0533 0.419 1.68
I need help with part b which is
Determine the rate constant for the reaction at 1500°C.
The answer should be ___________ M^-x S^-1
This is a Mixe worth 1 point / You have 2 of 6 attempts remaining / There is a 396 attempt penalty 12 Question (1 point) See page 569 Hydrogen gas reduces NO to N2 in the following reaction: 2I12(g) +2NO(g211,0g)+N2g The initial reaction rates of four mixtures of H2 and NO were measured at 1500°C...
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)
4. Suppose the following data is obtained for the reaction: 2NO(g)+2H2(g) → N2(g)+2H20(g) [NO] [Hz] Rate (mol L 54) 0.1 0.1 1.4 x 10-4 0.2 0.1 5.6 x 10-4 0.1 0.2 2.8 x 10-4 Determine the rate law for the reaction
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
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
For the reaction, 2NO(g)+2H2(g)→N2(g)+2H2O(g), what direction will the reaction proceed if [NO]=7.9x10-3M, [H2]=0.25 M, [N2]=0.15 M, & [H2O]=0.13 M. (K=650) forward reverse the reaction has stopped the reaction is at equilibrium
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