Oxygen combines with nitrogen monoxide to form nitrogen dioxide, described as 2 NO • 02w-2 NO2 . This reaction is caried out in a 45-liter reaction vessel, and over a given perlod, the rate of axygen consumption is 1.82 Mis. What is the rate of change in the nitrogen diaxide concentration over the same period? O364 Mis O091 Ms O182 Mis 0121 M. 0273 M

Consider the given reaction : 2HgC2(ag) + C204²(ag) – 2CH(ag) + 2CO2(g) + Hg2Cl2(s) Experiment [HgCl2] [C2O42] Initial rate 1 0.0836 M 0.202 M 5.2 x10-5 0.0836 M 0.404 M 2.08 x10-4 0.0418 M 0.404 M 1.04 x104 4 0.0627 M 0.606 M ? Calculate the initial rate for experiment 4. 3.50 x 10-4 M min-1 8.75 x 103 M min-1 1.20 x 10-4 M min-1 O 6.00 x 104 M min 1

Units of M s-1 please

Reaction of nitrogen monoxide and hydrogen A student collects the data below for the reaction:   2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)   Trial [NO]i [H2]i Initial Rate (M/s) 1 0.050 M 0.050 M 0.0917 2 0.10 M 0.050 M 0.367 3 0.10 M 0.10 M 0.734 Write 2-3 sentences to describe how you determined the rate law for the reaction.

2NOCl(g) → 2NO(g) + Cl2(g)      Rate = k[NOCl]2If this gaseous system has an initial rate of decomposition of NOCl of 0.0010 M s-1, and the volume of the system is reduced to one fifth of its original value, what is the new initial rate of decomposition of NOCl? Assume the temperature remains the same. 5.0×10-3 M s-1 2.5×10-2 M s-1 2.0×10-4 M s-1 4.0×10-5 M s-1 1.0×10-1 M s-1

Consider the reaction 4NO2(g)+ O2(g)→ 2N2O5(g)At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0019 M/s.  What rate is the molecular oxygen being consumed?

Consider the reaction 4NO2(g)+ O2(g)→ 2N2O5(g)At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0022 M/s.  What rate is the molecular oxygen being consumed?

Consider the reaction 4NO2(g)+ O2(g)→ 2N2O5(g)At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0019 M/s.  What rate is the molecular oxygen being consumed?

Consider the balanced chemical equation. H₂O₂ (aq) +31 (aq) + 2H+(aq) → I3¯¯(aq) + 2H₂O(1) In the first 11.0 s of the reaction, the concentration of I drops from 1.000 M to 0.752 M. Part A Predict the rate of change in the concentration of H₂O2 (A[H₂O2]/At). Express the rate to three significant figures and include the appropriate units. A[H₂O₂]/At = Submit Request Answer Part B Value μÀ HÅ Δ[13]/Δt = Value Predict the rate of change in the concentration of I3 (A[13¯]/At). Express the rate to three significant figures and include the appropriate units. Submit Request Answer Units Units ? www. ?

Need the following questions answered The reaction of interest:                                       O2 (g) +          2 NO (g)         →        2 NO2 (g)   Expt. [O2] (M) [NO] (M) Initial Rate (M/s) 1 0.0110 0.0130 0.00321 2 0.0220 0.0130 0.00640 3 0.0110 0.0260 0.01280 4 0.0330 0.0130 0.00960 5 0.0110 0.0390 0.02880   What is the reaction order for oxygen?         What is the reaction order for nitrogen monooxide?       What is the overall reaction order?     What is the rate law for this reaction?         What is the specific rate constant (k) for this reaction?         Write the rate law for this reaction that includes the numerical value of the specific rate constant: