A reaction has two reactants Q and P. What is the order with respect to each reactant and the overall order of the reaction described by the following rate expressions?
(a)
(c)
(d)
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Chapter 11 Solutions
Owlv2, 4 Terms (24 Months) Printed Access Card For Masterton/hurley's Chemistry: Principles And Reactions, 8th
- One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?arrow_forwardA reaction has two reactants X and Y. What is the order with respect to each reactant and the overall order of the reaction described by the following rate expressions? (a) rate=k1[ X ][ Y ]2 (b) rate=k2[ X ]2 (c) rate=k3[ X ][ Y ] (d) rate=k4arrow_forwardExpress the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]arrow_forward
- Sucrose, a sugar, decomposes in acid solution to give glucose and fructose. The reaction is first-order in sucrose, and the rate constant at 25 C is k = 0.21 h1. If the initial concentration of sucrose is 0.010 mol/L, what is its concentration after 5.0 h?arrow_forwardThe hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?arrow_forwardRegular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?arrow_forward
- Nitryl fluoride is an explosive compound that can be made by oxidizing nitrogen dioxide with fluorine: 2 NO2(g) + F2(g) → 2 NO2F(g) Several kinetics experiments, all done at the same temperature and involving formation of nitryl fluoride, are summarized in this table: Write the rate law for the reaction. Determine what the order of the reaction is with respect to each reactant and each product. Calculate the rate constant k and express it in appropriate units.arrow_forwardAt 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.arrow_forwardThe isomerization of cyclopropane, C3H6, is believed to occur by the mechanism shown in the following equations: C3H6+C3H5k1C3H6+C3H6(Step1)C3H6k2C2=CHCH3(Step2) 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. Explain.arrow_forward
- Chlorine dioxide, ClO2, is a reddish-yellow gas that is soluble in water. In basic solution it gives ClO3 and ClO2 ions. 2ClO2(aq)+2OH(aq)ClO3(aq)+ClO2(aq)+H2O To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Obtain the rate law and the value of the rate constant.arrow_forwardThe initial rate ( [NO]/ t] of the reaction of nitrogen monoxide and oxygen NO(g) + 2O2(g) NO2(g) was measured for various initial concentrations of NO and O2 at 25 C. Determine the rate equation from these data. What is the value of the rate constant, k, and what are its units?arrow_forwardHydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is [HI]/t = k[HI]2. At 443C, k = 30. L/mol min. If the initial HI(g) concentration is 1.5 102 mol/L, what concentration of HI(g) will remain after 10. minutes?arrow_forward
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