In a gas mixture, the partial pressures are argon 393 mm Hg, neon 73 mm Hg, and nitrogen 119 mm Hg. What is the total pressure (atm) exerted by the gas mixture?
To find the total pressure exerted by the gas mixture, you need to sum up the partial pressures of all the gases. Here's how you can calculate it:
Step 1: Convert the given partial pressures to atmospheres (atm). Since 1 atm is equal to 760 mm Hg, divide each of the partial pressures by 760 to convert them to atm.
Partial pressure of argon (in atm) = 393 mm Hg / 760 mm Hg/atm
Partial pressure of neon (in atm) = 73 mm Hg / 760 mm Hg/atm
Partial pressure of nitrogen (in atm) = 119 mm Hg / 760 mm Hg/atm
Step 2: Add up all the partial pressures.
Total pressure (in atm) = Partial pressure of argon + Partial pressure of neon + Partial pressure of nitrogen
Step 3: Calculate the total pressure.
Total pressure (in atm) = (Partial pressure of argon / 760) + (Partial pressure of neon / 760) + (Partial pressure of nitrogen / 760)
Now, let's calculate it:
Total pressure (in atm) = (393 mm Hg / 760 mm Hg/atm) + (73 mm Hg / 760 mm Hg/atm) + (119 mm Hg / 760 mm Hg/atm)
Total pressure (in atm) = 0.516 + 0.096 + 0.157
Total pressure (in atm) = 0.769 atm
Therefore, the total pressure exerted by the gas mixture is approximately 0.769 atm.