calculate the pressure,in atmospheres, of 2.00 mol helium gas in a 10.0-L container at 27 celcius? Please i don't understand any of this? help please?
Use the ideal gas law
PV=nRT
temps have to be in kelvins. Use the correct R (mol, liters, k, atm)
Sure! I'd be happy to walk you through the process of calculating the pressure of a gas using the ideal gas law. First, let's break down the steps involved:
Step 1: Identify the given information:
- Number of moles of helium gas: 2.00 mol
- Volume of the container: 10.0 L
- Temperature: 27°C (which needs to be converted to Kelvin)
Step 2: Convert the temperature to Kelvin:
The temperature needs to be in Kelvin for the ideal gas law equation, which uses absolute temperature. To convert from Celsius to Kelvin, you simply add 273.15 to the Celsius value:
27°C + 273.15 = 300.15 K
Step 3: Use the ideal gas law equation:
The ideal gas law equation is given as: PV = nRT
- P = pressure (what we're trying to calculate)
- V = volume (given as 10.0 L)
- n = number of moles (given as 2.00 mol)
- R = gas constant (its value depends on the units used, but typically 0.0821 L·atm/K·mol)
- T = temperature (converted to Kelvin as 300.15 K)
Rearranging the equation to solve for pressure (P), we have:
P = (nRT) / V
Step 4: Plug in the values:
Substituting the given values into the equation, we have:
P = (2.00 mol * 0.0821 L·atm/K·mol * 300.15 K) / 10.0 L
Step 5: Calculate the pressure:
After performing the calculations, you will find the answer to be the pressure in atmospheres (atm).