13. Only the O=O, but not the N=N, in the air reacts with the H2S. Which of the following is the best explanation for this behavior? A. The kinetic energy of oxygen molecules is greater than the kinetic energy of nitrogen molecules. B. N2 molecules are lighter than O2 so they collide with the H2S with less momentum. C. The activation energy for the reaction with N2 is too big because of the very strong triple bond. D. The concentration of N2 in the atmosphere is less than the concentration of O2.

If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N2? N₂(g)+ 3H₂(g) →2NH₂(g) O a. 245 M/s O b.0.345 M/s O c.0.518 M/s O d.0.173 M/s O e. 0.690 M/s

Which of these reactions is correct? * A. 3Na,S + 2AIN → 2NAN, + 3AI,S, B. 3Na,S + 2AIN → 2Na,Al, + 3NS, C. 3Na,S + 2AIPO, → 2Na,PO, + Al,S, D. No reaction O A B O D

The overall reaction of ozone reacting to form oxygen has been proposed to occur in a reaction mechanism of:           Step 1:  O3(g)    O2(g) + O(g)           Step 2:  O3(g) + O(g)    2O2(g) What is the role of O(g) and what is the overall balanced equation?   a. O(g) is a catalyst; 2O3(g)      3O2(g)                  b. O(g) is a catalyst; 2O3(g)  +  O(g)      3O 2(g) + O(g)   c. O(g) is an intermediate; 2O3(g)      3O2(g)   d. O(g) is an intermediate; 2O3(g) + O(g)     3O2(g) + O(g)

8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time

What is the rate of consumption of oxygen in a combustion reaction carried out in a 23.40-L flask if 4.05 mmol of O₂ is consumed in 39.9 ms? 4.0 M/S

If the rate of formation of chlorine trifluoride is 0.260 M/s, what is the rate of disappearance of F2? Cl2(g) + 3 F2(g) -----> 2 ClF3(g) a. -1.56 M/s b. -0.780 M/s c. -0.390 M/s d.-0.173 M/s   e. -0.0433 M/s

Nitrogen monoxide reacts with hydrogen at 500 °C as in the equation below. 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) A series of experiments was carried out to investigate the kinetics of this reaction. The results are shown in the table below. experiment 1 2 3 [NO] /mol dm-3 0.10 0.10 0.30 [H₂] /mol dm-3 k= 0.20 0.50 0.50 In this question, om- grammar. (i) For each reacta, deduce the order of reaction. Show your reasoning. (ii) Deduce the rate equation for this reaction. initial rate /mol dm-³ s-1 2.6 6.5 58.5 available for the quality of spelling, punctuation and (iii) Calculate the rate constant, k, for this reaction. State the units for k. units

The answer is C, please show steps, thanks.

Step 1: (slow) Step 2: C0 (fast) = CI The particle models shown above represent a proposed two-step mechanism for the destruction of ozone (03) in the upper atmosphere. Based on the models, which of the following represents a species that acts as a catalyst for the reaction? 88.8