Consider two hypothetical gases, gas A and gas B, which have the following Van der Waals constants: Gas A: a = 0.0 L² bar mol-² b=0.0174 L mol-¹ Gas B: a = 0.0 L² bar mol-2 b=0.0237 L mol-1 In one sample, 10 moles of gas A is placed in a 1.00 L container at 350 K. In the second sample, 10 moles of gas B is placed in a different 1.00 L container at 350 K. Compare the pressures in the two containers with the pressure predicted by the Ideal Gas Law. Which of the following statements is correct? The pressure of Gas B will deviate less than the pressure of Gas A from the pressure predicted by the Ideal Gas law. The pressure of Gas B will be larger than that predicted by the Ideal Gas Law. The pressure of Gas A will deviate less than the pressure of Gas B from the pressure predicted by the Ideal Gas law. The pressure of Gas A will be larger than that predicted by the Ideal Gas Law. The pressure of Gas A will deviate less than the pressure of Gas B from the pressure predicted by the Ideal Gas law. The pressure of Gas A will be smaller than that predicted by the Ideal Gas Law.

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Chapter1: Chemical Foundations
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Consider two hypothetical gases, gas A and gas B, which have the following Van der Waals constants:
Gas A: a = 0.0 L² bar mol-²
b=0.0174
L mol-¹
Gas B: a = 0.0 L² bar mol-2
b=0.0237 L mol-1
In one sample, 10 moles of gas A is placed in a 1.00 L container at 350 K. In the second sample, 10
moles of gas B is placed in a different 1.00 L container at 350 K. Compare the pressures in the two
containers with the pressure predicted by the Ideal Gas Law.
Which of the following statements is correct?
The pressure of Gas B will deviate less than the pressure of Gas A from the pressure predicted by
the Ideal Gas law. The pressure of Gas B will be larger than that predicted by the Ideal Gas Law.
The pressure of Gas A will deviate less than the pressure of Gas B from the pressure predicted by
the Ideal Gas law. The pressure of Gas A will be larger than that predicted by the Ideal Gas Law.
The pressure of Gas A will deviate less than the pressure of Gas B from the pressure predicted by
the Ideal Gas law. The pressure of Gas A will be smaller than that predicted by the Ideal Gas Law.
Transcribed Image Text:Consider two hypothetical gases, gas A and gas B, which have the following Van der Waals constants: Gas A: a = 0.0 L² bar mol-² b=0.0174 L mol-¹ Gas B: a = 0.0 L² bar mol-2 b=0.0237 L mol-1 In one sample, 10 moles of gas A is placed in a 1.00 L container at 350 K. In the second sample, 10 moles of gas B is placed in a different 1.00 L container at 350 K. Compare the pressures in the two containers with the pressure predicted by the Ideal Gas Law. Which of the following statements is correct? The pressure of Gas B will deviate less than the pressure of Gas A from the pressure predicted by the Ideal Gas law. The pressure of Gas B will be larger than that predicted by the Ideal Gas Law. The pressure of Gas A will deviate less than the pressure of Gas B from the pressure predicted by the Ideal Gas law. The pressure of Gas A will be larger than that predicted by the Ideal Gas Law. The pressure of Gas A will deviate less than the pressure of Gas B from the pressure predicted by the Ideal Gas law. The pressure of Gas A will be smaller than that predicted by the Ideal Gas Law.
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