chemistry

posted by .

For the reaction, 2 XO + O2 = 2 X02, some data obtained from measurement of the initial rate of reaction at varying concentrations are given below.

run # [XO] [O2] rate, mol L-l s-l
1 0.010 0.010 2.5
2 0.010 0.020 5.0

3 0.030 0.020 45.0

The rate law is therefore

a. rate = k[XO]2 [O2] b. rate = k[XO][O2]^2 c. rate = k[XO][O2]
d. rate = k[XO]2 [O2] ^2 e. rate = k[XO]2 / [O2]^ 2

No idea, help

  • chemistry -

    You can do these by reason or mathematically. Usually the initial ones are easy enough to do by reasoning. Here is how you do it.
    Look for a trial (run) in which the concn of 1 material changes and the other material does not. For example, trial 1 has 0.01 and trial 2 has 0.01 for (XO) while trial 1 shows rate of 2.5 for (O2) and trial 2 shows 5.0 for (O2).
    The reasoning part is this. Forget (XO) at this point since we did not change the concn (it stayed at 0.01). We changed concn O2 from 0.01 to 0.02 (doubled it) and we changed the rate from 2.5 to 5.0 (doubled it). So doubling concn caused doubling of rate so the order is 1 because 2^what = 2; obviously what is 1.

    Now we look to find a trial in which concn of O2 does not change but (XO) does.That's trial 2 and trial 3.
    (XO) changes from 0.01 to 0.03 (triples) while rate changes from 5.0 to 45.0 (45.0/5.0 = 9.0 times). Tripling concn XO made rate change by 9 so 3^what = 9 and that's 2 (3 squared = 9). Therefore, the reaction is second order with respect to XO. Thus the rate law expression is
    rate = k(XO)2(O2)1 and the 1 as an exponent isn't needed; I put it there to make the point that it was 1. The reaction is third order overall.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemisty

    Iodide Ion is oxidized to hypoiodite ion IO- by hypochlorite ion ClO- in basic solution. The equation is I- + ClO- --- IO- + Cl- Initial concentraition I- ClO- OH- exp 1. 0.010 0.020 0.010 exp 2. 0.020 0.010 0.010 exp 3. 0.010 0.010 …
  2. Chemistry

    Iodide Ion is oxidized to hypoiodite ion IO- by hypochlorite ion ClO- in basic solution. The equation is I- + ClO- --- IO- + Cl- Initial concentraition I- ClO- OH- exp 1. 0.010 0.020 0.010 exp 2. 0.020 0.010 0.010 exp 3. 0.010 0.010 …
  3. Chemistry

    For the reaction, 2 XO + O2 = 2 X02, some data obtained from measurement of the initial rate of reaction at varying concentrations are given below. run # [XO] [O2] rate, mol L-ls-l 1 0.010 0.010 2.5 2 0.010 0.020 5.0 3 0.030 0.020 …
  4. Chemistry

    For the reaction, 2 XO + O2 = 2 X02, some data obtained from measurement of the initial rate of reaction at varying concentrations are given below. run # [XO] [O2] rate, mol L-ls-l 1 0.010 0.010 2.5 2 0.010 0.020 5.0 3 0.030 0.020 …
  5. Chemistry

    For the reaction, 2 XO + O2 = 2 X02, some data obtained from measurement of the initial rate of reaction at varying concentrations are given below. run # [XO] [O2] rate,mol L-l s-1 1 0.010 0.010 2.5 2 0.010 0.020 5.0 3 0.030 0.020 …
  6. Chemistry

    The reaction between NO (nitric oxide) and oxygen is a key step in the formation of acid rain. O2(g) + 2NO(g) → 2NO2(g) A series of experiments were run, each of which starts with a different set of reactant concentrations. From …
  7. Chemistry

    The following initial rate data apply to the reaction F2(g) + 2Cl2O(g) ----> 2FClO2(g) + Cl2(g) Expt. # [F2](M) [Cl2O](M) Initial rate (M/s) 1 0.05 0.010 5.0 x 10^–4 2 0.05 0.040 2.0 x 10^–3 3 0.10 0.010 1.0 x 10^–3 Which …
  8. Chemistry

    Ammonium ion (NH4^+) reacts with nitrite ion (NO2^-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Expt. # [NH4^+] [NO2^-] Initial rate (M/hr) …
  9. Chemistry

    A 1.0 mL volume of 0.010 M H2SO4 is added to a mixture of 6 drops of 0.010 M HIO3, 14 drops of deionized water, and 1 drop of starch solution. A color change in the reaction mixture occurred after 56 seconds. a. Assuming 20 drops per …
  10. Chemistry

    Estimate the orders and rate constant K from the results observed for the Reaction. What is the rate when [H2O2]=[I-]=[H+]=1.0M?

More Similar Questions