What is the pressure in a 2.00 L container which holds 0.100 mol of methane and and 0.200 mol of carbon dioxide at standard temperature?
To find the pressure in the container, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
In this case, we have the volume (V = 2.00 L) and the number of moles for each gas (n(CH4) = 0.100 mol and n(CO2) = 0.200 mol). Additionally, since the question mentions "standard temperature," we can assume that the temperature is 273.15 K (0°C or 32°F).
Now, we need to find the total number of moles in the container. Since we are given the individual number of moles for methane and carbon dioxide, we can simply add those together to get the total number of moles (n(total)). In this case, n(total) = n(CH4) + n(CO2) = 0.100 mol + 0.200 mol = 0.300 mol.
Next, we can substitute the known values into the ideal gas law equation: PV = nRT. Rearranging the equation to solve for pressure (P), we get P = (nRT) / V.
Plugging in the values, we have P = (0.300 mol * 0.0821 L·atm/(mol·K) * 273.15 K) / 2.00 L.
Calculating this expression, we find that the pressure in the container is approximately 11.21 atm.