Consider the reaction: A + B --> products.  From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant:   [A] (M)                       [B] (M)                       Rate (M/s)   1.50                             1.50                             3.15 X 10-1 1.50                             2.50                             2.98 X 10 –1 3.00

Consider this reaction: →H2CO3aq+H2OaqCO2aq At a certain temperature it obeys this rate law.rate =·0.0579M−1s−1H2CO32 Suppose a vessel contains H2CO3 at a concentration of 0.820M. Calculate the concentration of H2CO3 in the vessel 280.seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M

Some measurements of the initial rate of a certain reaction are given in the table below. [N:] N2| |H2| initial rate of reaction 0.768 M 2.48M 0.0363 M/s 0.768 M 0.466M 0.00128M/s 0.209M 2.48M 0.00988 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k ||| x10 k =

For the given equation at 800 °C: CO(g) + Ch(g) > COCh(g), the following data were collecica Experiment (COL(M) 0.96 1.92 0.96 (CH] (M) 1.60 1.60 3.20 Rate of appearance COCh (M/s) 0.121 0.242 0.484 Determine the Rate Law for the reaction From your Rate Law determined in question #1 above, determine the value of the rate constant WITH THE APPROPRIATE UNITS. ONLY If you could not answer #1 above, use this "mock" data to solve for k: Rate = K[ARB]?, with [A] = 1.00 M and B]o = 1.50 M, with a rate of 2.50 x 10-2 M/s.

Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) → SO₂(g) + Cl₂ (g) - [SO₂Cl₂], (M) k = 0.100 0.200 0.300 Initial rate (M/s) 2.30 x 10-6 4.60 x 10-6 6.90 x 10-6 Determine the value and units of the rate constant. MacBook Pro units: Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemi

: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9

Given the information based on time and concentration, determine the order of the reaction and the rate constant k when graphing the following data: A--> C+D Time (s) (A] M 10 0.1000 50 0.0856 100 0.0749 200 0.0598 350 0.0460 500 0.0373 800 0,0271

Some measurements of the initial rate of a certain reaction are given in the table below. |H2|| ||2| | initial rate of reaction 1.50M| 2.25М 0.540 M/s 1.50M 6.45 М 1.55 M/s 5.57 М 2.25М 2.01 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k x10 k =

Given below is the data for the reaction. Calculate the value of the rate constant "k" with proper units. A + B → C Set [A] (M) [B] (M) Init, rate M-sec 1 0.050 0.200 5.0 x 10-5 2. 0.100 0.200 5.0 x 10-5 0.050 0.600 4.5 x 10-4 Determine the order in "A" Determine the order in "B" Substitute the order for A and B in the rate law equation below. Rate = k [A]' [B]

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCII → OI¯ + Cl¯ This rapid reaction gives the following rate data: |[OCI¯] (M) [I¯] (M) Initial Rate (M/s) 1.36 × 10-4 1.5 × 10- -3 3.0 × 10-³ 1.5 x 10- -3 1.5 x 10 -3 1.5 × 10-³ 3.0 × 10-³ 2.72 × 10-4 2.72 × 10-4 Calculate the rate constant with proper units. Express the rate constant to two significant figures. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash (e.g. ft * lb or ft-lb). k Submit Part C HÅ Value Request Answer Units ? Calculate the rate when [OC] = 2.3 × 10-³ and [I¯] = 6.0 × 10-4 Express the rate in molarity per second to two significant figures.