A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg?

• A. 1013 mmHg
• B. 760 mmHg
• C. 1500 mmHg
• D. 1140 mmHg

Answer: (D)

Verified step by step guidance

1. Start by understanding the relationship between different units of pressure. The problem requires converting pressure from atmospheres (atm) to millimeters of mercury (mmHg).
2. Recall that 1 atm is equivalent to 760 mmHg. This conversion factor will be crucial in solving the problem.
3. Set up the conversion using the formula: \( P_{mmHg} = P_{atm} \times \frac{760 \text{ mmHg}}{1 \text{ atm}} \).
4. Substitute the given pressure in atm (1.50 atm) into the formula: \( P_{mmHg} = 1.50 \text{ atm} \times \frac{760 \text{ mmHg}}{1 \text{ atm}} \).
5. Perform the multiplication to find the pressure in mmHg. This will give you the pressure of the helium gas in the tank in mmHg.