The reaction of NO and O2 produces NO2.
2 NO(g) + O2(g) „_ 2 NO2(g)
The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.7 x 10^2 M^¡V2s^¡V1. What is the rate of reaction when the initial concentrations of NO and O2 are 0.025 M and 0.015 M, respectively?

Show your work: I thought it was
1/0.025-1/0.015=4.7 x 10^2 M^¡V2s^¡V1

but that is not right b/c the answer is 4.4 x 10^-3 M/s

  1. 👍 0
  2. 👎 0
  3. 👁 2,125
  1. You're trying to solve the problem wrong. Since one is first order and the other is second order, that equation won't work; besides, you have only one concn. What you want to use is the rate equation of
    rate = k(NO)^2(O2)
    Plug in k, NO, and O2 and calculate rate. 4.4E-3 is the right answer.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2 (g)+ H2O (l) --> 2HNO3 (l) + NO (g) Suppose that 5 mol NO2 and 1 mol H2O combine and react completely. How many moles of

  2. chem

    For the elementary reaction NO 3 + CO → NO2 + CO 2 the molecularity of the reaction is __________, and the rate law is rate = __________. A) 2, k[NO 2][CO 2] B) 2, k[NO 3][CO]/[NO2 ][CO 2] C) 4, k[NO 3][CO][NO 2][CO 2] D) 4,

  3. CHEM

    Consider the reaction, 3 NO2(g) + H2O(l) ® 2 HNO3(aq) + NO(g), where DH = – 137 kJ. How many kilojoules are released when 92.3 g of NO2 reacts?

  4. Chemistry

    Nitrogen dioxide decomposes at 300°C via a second-order process to produce nitrogen 14) monoxide and oxygen according to the following chemical equation. 2 NO2(g) → 2 NO(g) + O2(g). A sample of NO2(g) is initially placed in a

  1. Chemistry

    The reaction between nitric oxide (NO) and oxygen to form nitrogen dioxide (NO2) is a key step in photochemical smog formation. 2 NO(g) + O2(g) 2 NO2(g) (a) How many moles of NO2 are formed by the complete reaction of 0.404 mole

  2. chem

    For the reaction 3NO2 + H2O  2HNO3 + NO, how many grams of HNO3 can form when 1.00 g of NO2 and 2.25 g of H2O are allowed to react? This is a limiting reagent problem. 1. Write the equation. You have done that and it is balanced.

  3. chemistry

    Balance the following redox reaction occurring in acidic solution Cu(s) + NO3-(aq)--> Cu2+(aq) +NO2(g) This is what I have done so far Cu-->Cu2+ + 2e- 2H + NO-3 --> NO2 + H2O Need help please

  4. Chemistry

    The gram-formula mass of NO2 is defined as the mass of one mole of a. one mole of NO2 b. one molecule of NO2 c. two moles of NO d. two molecules of NO Explain why.

  1. Chemistry due soon

    If the following reaction: NO(g) + 1/2O2(g) NO2(g) has the following enthalpy change: H° = -56 kJ/mol What is the enthalpy of the decomposition reaction of 2 moles of NO2? A. 112 kJ B. 56 kJ C. -56 kJ D. -112 kJ i think the

  2. Inorganic chemistry

    Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide. NO2(g) + CO(g) ==>NO(g) + CO2(g) A proposed mechanism for this reaction is 2No2(g) = NO3(g) + NO(g) (fast,equilibrium) NO2(g) + CO(g)

  3. Chemistry

    What mass of NO2 is formed by the complete reaction of 2 mol O3 with excess NO in the reaction? O3 + NO --> O2 + NO2 I know the molar mass of O3 is 48 g/mol and NO2 46 g/mol a) 23.0 g b) 46.0 g c) 92.0 g d) 96.0 g

  4. PChem

    For the gas phase reaction 2NO2 + F2 ¨ 2NO2F, the rate constant is k= 38 dm3/mol-s at 27 oC. The reaction is first-order in NO2 and first-order in F2. A) Calculate the number of moles of NO2, F2, and NO2F after 10.0 s if 2.00

You can view more similar questions or ask a new question.