Use the van der Waals equation and the data in Table 2.1 of Chang to calculate:

Question

Use the van der Waals equation and the data in Table 2.1 of Chang to calculate:
a) the pressure of 10.0 g of ammonia in a container of volume 500.0 mL at 25 °C
b) the pressure of 10.0 g of hydrogen in a vessel of volume 250.0 mL at 100.0 °C
c) repeat parts (a) and (b) using the ideal gas law
d) the percentage error assuming that ammonia and hydrogen behave as ideal gases under the same conditions as in (a) and (b)

Table 2.1 van der Waals Constants and Boiling Points of Some Substances Substance a/atm L2 mol-2 b/L mol Boiling Point/K He Ne Ar H2 N2 02 CO CO2 CH4 H2o NH3 0.0341 0.214 1.34 0.240 1.35 1.34 1.45 3.60 2.26 5.47 0.0237 0.0174 0.0322 0.0264 0.0386 0.0312 0.0395 0.0427 0.0430 0.0305 0.0379 4.2 27.2 87.3 20.3 77.4 90.2 83.2 195.2 109.2 373.15 239.8 4.25

Explanation / Answer

http://www.webqc.org/van_der_waals_gas_law.html

you can use the above link for identifying the Pressure of

NH3 (no of moles) = 0.5883

H2(no of moles) = 5

a,b accordingly from the table

this link can also be used

http://calistry.org/calculate/vanDerWaalsCalculator

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