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13 Dec 2019

Show that at high temperatures, qv = kT/hcv

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Calculate the following for N2O gas at 298 K: a) The characteristic rotational temperature, qR. b) The characteristic vibrational temperature, qV, for each if the four vibrational modes c) The molecular partition function, q. Clearly show the values and calculations for the translational, rotational, and vibrational contributions (qT, qR, and qV for each vibrational mode). d) The constant-volume molar heat capacity, CV,m. Clearly show the values and calculations for the translational, rotational, and vibrational contributions. e) The constant-pressure molar heat capacity, Cp,m (use the relationship between CV,m and Cp,m for a perfect gas) . Compare your value with that found in Table 2C.5. f) The standard molar entropy, (the molar entropy at standard pressure, ). Clearly show the values and calculations for the translational, rotational, and vibrational contributions. Compare your value with that found in Table 2C.5. Molecular properties of N2O that you will need for the calculations. = 0.4190 cm-1 = 2224 cm-1 = 1285 cm-1 = 589 cm-1 (doubly degenerate

(4) Rate Law from Concentration versus Time Data

NO2(g) + CO(g) --> NO(g) + CO2(g)

The rate of the above reaction depends only on the concentration of nitrogen dioxide at temperatures below 225Â°C. At a temperature below 225Â°C the following data were obtained:

Time (s)

0 1.45Ã10^3

3.62Ã10^3

5.44Ã10^3

1.09Ã10^4

2.18Ã10^4

[NO2] (mol/L)

0.580

0.554

0.519

0.493

0.428

0.340

(a) Which of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data. (say yes or no to each)

1/[NO2] - 1/[NO2]0 = kt

[NO2] = [NO2]0 - kt

ln[NO2] - ln[NO2]0 = -kt

-d[NO2]/dt = k[NO2]^2

k[NO2]^2 = d[CO2]/dt

(b) Calculate the rate constant (k). Enter the numerical value and corresponding units.

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Show that at high temperatures, qv = kT/hcv

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