Question

1. If 0.00100 moles of hydrogen gas at 155°C exert a pressure of 323 atm, what is the volume?

A) 0.00092 L
B) 1.0 L
C) 10.0 L
D) 0.92 L

2. It is desired to obtain a volume of 1.00 dm³ of nitrogen at 100°C and 640 kPa. How many moles of nitrogen would be required?
A) 1.00 moles
B) 0.01 moles
C) 0.156 moles
D) 6.40 moles

3. Some oxygen is collected in a 0.250 dm³ container at 25.0°C and 720. kPa. How many moles of oxygen is this?
A) 0.0098 moles
B) 2.50 moles
C) 0.25 moles
D) 1.00 moles

Answer 1

The volume of 0.00100 moles of hydrogen gas at 155°C and 323 atm can be calculated using the Ideal Gas Law, but the exact volume is not given in the question's options. The provided options incorrectly state moles instead of volume, suggesting a typo in the question.

Step-by-step explanation:

To calculate the volume of 0.00100 moles of hydrogen gas at 155°C exerting a pressure of 323 atm, the Ideal Gas Law is used, which is PV=nRT, where P is pressure, V is volume, n is moles, R is the ideal gas constant, and T is temperature in Kelvin. First, convert the temperature from Celsius to Kelvin by adding 273.15 to 155°C, resulting in T = 428.15 K. The ideal gas constant R is typically 0.08206 L atm mol⁻¹ K⁻¹ in these units. Using the Ideal Gas Law and solving for V:

V = ⅓nRT / P

Substituting the values gives:

V = (0.00100 moles)(0.08206 L atm mol⁻¹ K⁻¹)(428.15 K) / (323 atm)

Carrying out the multiplication and division provides the volume of the gas. However, the exact answer is not listed among the provided options since they seem to indicate moles rather than volume. There may be a typo in the question.