Question

a sample of hydrogen gas exerts a pressure of 456 torr in a container. what is this pressure in atmospheres?
a) 0.217 atm
b) 0.496 atm
c) 0.613 atm
d) 1.53 atm
e) 4.60 atm

Explanation:

Step1: Recall the conversion factor

We know that \( 1 \text{ atm} = 760 \text{ torr} \). So to convert torr to atm, we use the conversion factor \( \frac{1 \text{ atm}}{760 \text{ torr}} \).

Step2: Set up the conversion

We have a pressure of 466 torr. To convert this to atm, we multiply the given pressure in torr by the conversion factor:
\( 466 \text{ torr} \times \frac{1 \text{ atm}}{760 \text{ torr}} \)

Step3: Calculate the result

First, cancel out the torr units: \( \frac{466}{760} \text{ atm} \). Then, perform the division: \( \frac{466}{760} \approx 0.613 \text{ atm} \).

Answer:

C) 0.613 atm