If 10.00 mol of an ideal gas were confined to 22.41 L at 0.0 °C, it would exert a pressure of 10.00 atm. Use the van der Waalsequation and Table 10.3 to estimate the pressure exerted by 1.000 mol of Cl2(g ) in 22.41 L at 0.0 °C. TABLE 10.3 Van der Waals Constants for Gas MoleculesSubstancea (L²-atm/mol?)b (L/mol)Не0.03410.02370Ne0.2110.0171Ar1.340.0322Kr2.320.0398Xe4.190.0510На0.2440.0266N21.390.0391O21.360.0318F21.060.0290Cl,6.490.0562Н-о5.460.0305NH34.170.0371CH42.250.0428CO23.590.0427CCI420.40.1383

The van der waals equation is as shown below. Since for Cl2 we have a = 6.49 and b = 0.0562 Given…

Answered: TABLE 10.3 Van der Waals Constants for…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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If 10.00 mol of an ideal gas were confined to 22.41 L at 0.0 °C, it would exert a pressure of 10.00 atm. Use the van der Waals
equation and Table 10.3 to estimate the pressure exerted by 1.000 mol of Cl₂(g ) in 22.41 L at 0.0 °C.

TABLE 10.3 Van der Waals Constants for Gas Molecules
Substance
a (L²-atm/mol?)
b (L/mol)
Не
0.0341
0.02370
Ne
0.211
0.0171
Ar
1.34
0.0322
Kr
2.32
0.0398
Xe
4.19
0.0510
На
0.244
0.0266
N2
1.39
0.0391
O2
1.36
0.0318
F2
1.06
0.0290
Cl,
6.49
0.0562
Н-о
5.46
0.0305
NH3
4.17
0.0371
CH4
2.25
0.0428
CO2
3.59
0.0427
CCI4
20.4
0.1383

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