The iodide ion reacts with ingredient in chlorine bl aws (Section 14.3) the foll

Question

The iodide ion reacts with ingredient in chlorine bl aws (Section 14.3) the following rate data n M/s, for the (b) Calculate e time of the is greatet, the ,000 s, or be- ph [CH NC s rates in Mis Areact, (a) If [A] is doubled, how will the rate will the rate constant change? (b) What are the s the following rate law Rate hgers for A and B? What is the overall reaction reacc) What are the units of the rate constant? tion a hypothetical reaction between A, B, and C t is first order in A, zero order in B, and second order 1.5×10-3 3.0 1.5 × 10-3 1.5) 3.0 14.28 Consi (a) Write the rate law for tate constant with prop when (a-,-2.0 × 10 14.34 The reaction 2C1O-(ag) C. (a) Write the rate law for the reaction. (b) How does in e when [A] is doubled and the other reac entrations are held constant? (c) How does the sured for th the rate c tant Cne when [B] is tripled and the other reactant ons are held constant? (d) How does the rate when [CI is tripled and the other reactant con- are held constant? (e) By what factor does the rate change when the concentrations of all three reac tants are tripled? (f) By what factor does the rate change when the concentrations of all three reactants are cut in aq) + H2OU) change Experiment [C0](M half? 0.020 129 The decomposition reaction of N2Os in carbon tetrachlo- ride is 2 N2Os4NO2 + 02. The rate law is first order a) Determine the rate L the rate constant with g when [C1 0.100 k 14.35 The following data w in N20s. At 64 °C the rate constant is 4.82 x 10-3 (a) Write the rate law for the reaction. (b) What is the rate of reaction when [N20s] 0.0240 M? (c) what happens to the rate when the concentration of N,Os is doubled to 0.0480 M? (d) What happens to the rate when the con- centration of N2Os is halved to 0.0120 M? in M/s, for the t. (b) Calculate me for the data hich is greater, 215.0 min, or Graph [HCI Experiment (BF] (M) 0.250 0.250 14.30 Consider the following reaction: d) 2N0(g) + 2H2(g)- N2(g) + 2H2O(g) rates in neous 0.175 (a) The rate law for this reaction is first order in H2 and second order in NO. Write the rate law. (b) If the rate what is the reaction rate when [NO]-0.035 M and the concentration of H, is 0.010 M (d) What is the tions, indicate actant is related (a) What is the rate the overall order of t constant with prope [BFs] = 0.100M and constant for this reaction at 1000 K is 6.0 x 10)M b] = 0.015 M? (c) what is the reaction rate at 1000 K 0.10 M 14.36 The following d rate of disappeas when the concentration of NO is increased to on rate at 1000 K if INO] is decreased to 0.010 M and H2] is increased to 0.030 M Consider the following reaction: 4.31 0012 CH,Br(ag)+OH(agCH,OH(ag) + Br (al) rate law for this reaction is first order in CH Br 0.025 ce of each prod- The rst order in OH-. When [CHBr) is 5.0 x 1 OH is0 0.0432 M/s unitsfeue of the rate constant? (b) What are constant? (c) What would happen 0.050 M, the reaction rate at 298 K is e units of the rate

Explanation / Answer

14.27

   rate = k[B]^2

a) if [A] is doubled, no change in rate of reaction.

b) from rate law : order of B = 2

                   order of A = 0

   over all reaction order = 2+0 = 2

c) rate constant(k) = M-1.s-1

14.31
a) rate = k[CH3Br][OH-]

   0.0432 = k*0.005*0.05

k = 172.8 M-1.s-1

b) units of k = M-1.s-1

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