Answer all assigned questions and problems, and show all work.
2NO(g) + O2(g) → 2NO2(g)
Suppose that at a particular moment during the reaction nitric oxide (NO) is reacting at the rate of 0.066 M/s.
NH4+(aq) + NO2–(aq) → N2(g) + 2H2O(l)
is given by rate = k[NH4+][NO2–]. At 25ºC, the rate constant is 3.0 × 10–4/ M · s. Calculate the rate of the reaction at this temperature if [NH4+] = 0.26 M and [NO2–] = 0.080 M. (5 points)
A + B → products
From the following data obtained at a certain temperature, determine the order of the reaction and calculate the rate constant. (5 points)
|[A] (M)||[B] (M)||Rate (M/s)|
|1.50||1.50||3.20 × 10-1|
|1.50||2.50||3.20 × 10-1|
|3.00||1.50||6.40 × 10-1|
4PH3(g) → P4(g) + 6H2(g)
The half-life of the reaction is 35.0 s at 680°C. Calculate (a) the first-order rate constant for the reaction and (b) the time required for 95 percent of the phosphine to decompose. (10 points)
2NOBr(g) → 2NO(g) + Br2(g)
is 0.80/M · s at 10ºC.
CO(g) + Cl2(g) → COCl2(g)
at 250°C is 1.50 × 103 times as fast as the same reaction at 150°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant. (Hint: use equation 13.14.) (10 points)
CH3COCH3 + Br2 → CH3COCH2Br + H+ + Br–
The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and H+ ions at a certain temperature:
|[CH3COCH3]||[Br2]||[H+]||Rate of Disappearance of Br2 (M/s)|
|(1)||0.30||0.050||0.050||5.7 × 10–5|
|(2)||0.30||0.10||0.050||5.7 × 10–5|
|(3)||0.30||0.050||0.10||1.2 × 10–4|
|(4)||0.40||0.050||0.20||3.1 × 10–4|
|(5)||0.40||0.050||0.050||7.6 × 10–5|
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