The reaction 2NO (g)  + O2 (g)  →  2NO2 (g) was studied. and the following data were obtained where Rate = -(Δ[O2])/(Δt) [NO]0(molecules/cm3) [O2]0(molecules/cm3) Initial Rate (molecules/cm3 • s) 1.00 x 1018 1.00 x 1018 2.00 x 1016 3.00 x 1018 1.00 x 1018 1.80 x 1017 2.50 x 1018 2.50 x 1018 3.13 x 1017 What would be the initial rate for an experiment where [NO]0 = 6.21 x 1018 molecules/cm3 and [O2]0 = 7.36 x 1018 molecules/cm3?

Consider this reaction: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) At a certain temperature it obeys this rate law. =(0.0152 s¹)[H₂CO3] rate = Suppose a vessel contains H₂CO3 at a concentration of 0.250M. Calculate the concentration of H₂CO3 in the vessel 56.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X

See image below. Can you please show me how to solve this problem?

Consider the hypothetical reaction A(g)  +  B(g)                  C(g) The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0L. The reaction is second order with respect to A and first order in respect to B. Which of the containers, W,X,Y or Z, would have the greatest reaction rate? Justify your answer.

3. The following mechanism is proposed for the reaction of chlorine with chloroform: Cl, + CHCI, CCI, + HCI Cl, Step 1 fast equilibrium 2Cl CHCI, +CI » HCI +CCI, CCI, +Cl»cCI, Step 2 slow Step 3 fast a) Show that this mechanism gives the correct, overall balanced reaction equation. b) Write the rate law predicted by this mechanism.

3) The reaction 2NO(g) + O2(g) → 2 NO₂(g) was studied, and the following data were obtained where Δ[02] At Rate = [NO]. [0₂]0 (molecules/cm³) (molecules/cm³) 1.00 x 1018 3.00 x 10¹8 2.50 × 1018 1.00 x 1018 1.00 × 10¹8 2.50 × 1018 Submit Answer Initial Rate (molecules/cm³.s) 2.00 × 1016 1.80 x 10¹7 3.13 x 10¹7 What would be the initial rate for an experiment where [NO], = 1.57 x 10¹8 molecules/cm³ and [0₂]0 = 8.82 x 10¹8 molecules/cm³? 3 Rate = molecules/cm³.s Try Another Version [References] 5 item attempts remaining Show Hint

Writing the rate law implied by a simple mechanism with an initial slow... Suppose the formation of nitryl fluoride proceeds by the following mechanism: elementary reaction step 1 NO₂ (g) +F₂ (g) 2 k₁ k₂ 2 F (g) + NO₂(g) → NO₂F (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. NO₂F (g) +F (g) Note: your answer should not contain the concentrations of any intermediates. rate constant rate = k 0+ 00 X Ś

The reaction CH3NC → CH3CN has a rate constant of 0.498 s-1 at a specific temperature. What is the concentration of CH3NC after 41 seconds if its initial concentration is 1.368 M? (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0) esc 3 7 delete Q E Y P A D G K return ock V B N M command option control option command 10 40 an the a greates4

Consider this reaction: 2C1₂0, (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate = (1.31 M¹-8¹)[Chos S Suppose a vessel contains Cl₂O5 at a concentration of 0.690 M. Calculate the concentration of C1₂O5 in the vessel 3.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M ? CU x10 X S