Question

Exactly one mole of an ideal gas is contained in a 2.00-liter container at 1,000 k. what is the pressure exerted by this gas? given: r = 0.08205 l � atm/k � mol a. 164 atm b. 82 atm c. 64 atm d. 41 atm

Answer 1

d. 41 atm

Step-by-step explanation:

To find the pressure exerted by the gas, we need to use the ideal gas law. The ideal gas law is an equation in thermodynamics that describes the behavior of a hypothetical ideal gas and relates the pressure, volume, and temperature of the gas. It is expressed by the equation PV = nRT, where P is the pressure in atm, V is the volume in liters, n is the number of moles, R is the universal gas constant in L·atm / (K·mol), and T is the temperature in Kelvin.

We can rearrange the equation to solve for pressure.

• PV = nRT
• 
  `P = (nRT)/(V)`

Now, plug in the values with the appropriate units.

• 
  `P =((1 mol)(0.08205 (L*atm)/(K*mol))(1000 K) )/(2.00 L)`
• P = 41.025 atm

The pressure exerted by one mole of an ideal gas contained in a 2.00 L container at 1000 K is d. 41 atm.