N2+2H2O <--> 2NO =2H2. which way would the equilibrium shift if you remove H2?
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N2+2H2O <--> 2NO =2H2. which way would the equilibrium shift if you remove H2?
N2+2H2O ,--> 2NO+2H2. which way would the equilibrium shift if you increased the volume?
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
9. Which of the following will have no shift in equilibrium if the volume is decreased? 2H2O(g) + N2(g) + 2H2(g) + 2NO(g) SiO2(g) + 4HF(g) SiF4(g) + 2H2O(g) CO(g) + H2(g) C(g) + H2O(g) C6H1206(s) + 602 6CO2(g) + 6H2O(g) 10. Which of the following will shift this endothermic reaction to the REACTANT side? 302(g) 203(g) Increase the pressure Decrease the O2 gas Increase the temperature Remove the ozone, O3
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
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...
QUESTION 19 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? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2
QUESTION 9 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? k[N2O][H2] k[NO]2[H2] k[NO]2[H2]2 k[NO]1/2[H2] k[NO]2
the following reaction 2NO(0) + 2H2 (g) № (g) + 2 HaO (g) H2/0000 M quilbrium constant, Ke, for the reaction. Initially, a mixture of 0.300 M NO, 0.100 M NOwas found to beg,062-м. D.ig2 the value of the brium (init h N2)t eubrhum the conentreton dr H20 was allowed to reach equilibrium ( 0-200 8) Consider the following reaction. HSO.. (aq) + H2O (I) → HO. (aq) + SO2-(aq) The initial concentrations are [HSO門-0.3000 M, [HO+]s 0.050 M. [SO...
The gas NO reacts with H2, forming N2 and H2O: 2NO(g)+2H2(g) 2H2O(g)+N2(g) If Δ[NO]/ Δt = –24.0 M/s under a given set of conditions, what are the rates of change of [N2] and [H2O]?