Write the rate law for the following elementary reaction: NO3(g) + CO(g) → NO₂(g) + CO2(g) Use k₁ to stand for the rate constant. rate 0/0 X 3 010 8 ?

The isomerization of cyclopropane, C3H6, is believed to occur by the mechanism shown in the equations above. Here  C3H6* is an excited cyclopropane molecule. At low pressure, Step 1 is much slower than Step 2. Derive the rate law for this mechanism at low pressure?

Initial rate: 1.6 •10^-7mol/L•s K=6.4 •10^-9L/mol•s Rate law: k[HI]^2 Can you please show me the steps.

Consider the hypothetical reaction: A + B + 2C → 2D + E where the rate law is Rate = -ALA) = k[A][B]2 An experiment is carried out where [Alo = 7.200 x 102 M, [B]. = 2.500 M and [Cla = 2.500 M. The reaction is started, and after 11.60 seconds, the concentration of A is 2.200 x 10° M. Calculate the value of k for this reaction in units of M2s1. Answer:

Click in the answer box to activate the palette. Enter the general form of the rate law for the following process. Represent the order as  n, n', and so forth.  Complete the equation using brackets, [], to represent concentration.  2Cu(g) + O2(g) → 2CuO(g)

Consider this reaction: 2HI (g) → H, (g) +I, (g) At a certain temperature it obeys this rate law. rate =(0,465 s)[HI Suppose a vessel contains HI at a concentration of 0.540M. Calculate the concentration of HI in the vessel 2.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

0/5 Writing the rate law of an elementary reaction Write the rate law for the following elementary reaction: 2 NO(g) + Br,(g) + 2 NOBR(g) Use k, to stand for the rate constant. rate

Nitrogen monoxide, NO, reacts with hydrogen to give nitrous oxide, N20, and water. 2NO(g) + H2 (g) → N½O(g) + H20(g) In a series of experiments, the following initial rates of disappearance of NO were obtained: Initial Concentration of NO Initial Concentration of H2 Initial Rate of Reaction of NO Exp. 1 8.6 x 10-3 M 4.1 x 10-3 M 8.7 x 10-5 M/s 3 Exp. 2 1.7 x 10-2 M 4.1 x 10- M 3.5 x 10-4 M/s Exp. 3 8.6 x 10-3 M 8.2 x 10-3 M -4 1.7 x 10 M/s

Consider this reaction: 2SO3 (g) →2SO₂ (g) + 0₂ (8) At a certain temperature it obeys this rate law. rate= (0.00626 s¹)[03] Suppose a vessel contains SO3 at a concentration of 0.250M. Calculate the concentration of SO3 in the vessel 99.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś

Write the rate law for the following elementary reaction: 2 N,05(9) → 2 N2O4(9) + O2(g) Use k, to stand for the rate constant. rate