# CHM135H1 Study Guide - Midterm Guide: Phosgene, Iron Oxide, Reaction Rate

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17 Mar 2014
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TT2 2011
1. Consider the reaction H2(g) + I2(g) => 2 HI(g). The relationship between the rate of
disappearance of I2 and the rate of formation of HI is:
a) -Δ[I2]/Δt = +Δ[HI]/Δt
b) -Δ[I2]/Δt = +2Δ[HI]/Δt
c) -2Δ[I2]/Δt = -Δ[HI]/Δt
d) -2Δ[I2]/Δt = +Δ[HI]/Δt
e) -Δ[I2]/Δt = -Δ[HI]/Δt
2. Consider the following statements about a chemical reaction:
i) The forward reaction rate increases as the reaction gets going
ii) The forward reaction rate always equals the reverse reaction rate
iii) Since a catalyst affects forward and reverse rates differently, the yield of product is
increased
a) Only statement i) is true
b) Only statement ii) is true
c) Only statement iii) is true
d) Only statements ii) and iii) are true
e) None of the statements are true
3. The following rate data was obtained by students for the reaction between hydrogen
peroxide and iodide under acidic conditions:
Run [H2O2] (M) [I-] (M) Initial rate (M/s)
1 0.0080 0.015 1.16 x 10-6
2 0.020 0.015 2.91 x 10-6
3 0.020 0.0060 1.16 x 10-6
The correct empirical rate law and value of the rate constant for this reaction are:
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a) Rate = k[H2O2][I-], k = 9.7 x 10-3 M-1 s-1
b) Rate = k[H2O2]2[I-], k = 1.0 x 10-1 M-2 s-1
c) Rate = k[H2O2][I-]0, k = 1.4 x 10-4 s-1
d) Rate = k[H2O2]0[I-]1, k = 7.7 x 10-5 s-1
e) Rate = k[H2O2]2[I-]2, k = 8.0 x 101 M-3 s-1
4. Phosgene is formed by the reaction CO(g) + Cl2(g) => COCl2(g), for which the activation
energy is 135 kJ/mol. At what temperature will the reaction be 1000 times faster than it is
at 125 °C for the same initial amounts of CO and Cl2?
a) 153 °C
b) 180 °C
c) 206 °C
d) 233 °C
e) 259 °C
5. Iron oxide ores are reduced to iron metal by exothermic reaction with carbon monoxide
FeO(s) + CO(g)  Fe(s) + CO2(g)
Which of the following changes in condition will cause the equilibrium to shift to the
right?
b) remove CO
d) halve the volume
e) reduce the temperature
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