Question

1. a container holds three gases: oxygen, carbon dioxide, and helium. the partial pressures of the three gases are 1520.00 torr, 3.00 atm, and 204.00 kpa, respectively. what is the total pressure inside the container?

Explanation:

Step1: Convert all pressures to kPa

First, convert 1520.00 torr to kPa:
$1520.00 \text{ torr} \times \frac{101.325 \text{ kPa}}{760 \text{ torr}} = 202.65 \text{ kPa}$
Next, convert 3.00 atm to kPa:
$3.00 \text{ atm} \times 101.325 \text{ kPa/atm} = 303.975 \text{ kPa}$
The pressure of helium is already 204.00 kPa.

Step2: Sum the partial pressures

Add the converted pressures together:
$P_{total} = 202.65 \text{ kPa} + 303.975 \text{ kPa} + 204.00 \text{ kPa}$

Answer:

$710.625 \text{ kPa}$ (or can be rounded to 711 kPa; if converted to other units: ~5.33 atm, ~5330 torr)