In an experiment, you fill a heavy walled 5.00 L flask with methane gas, CH4. If the flask contains 7.13g of methane at 19 degrees C, what is the gas pressure.
Use the ideal gas law.
Can some one help me get started on this problem please
PV = nRT
P is pressure in atmospheres and in this problem is the unknown.
V = volume in liters = 5.00 L.
n = mols = grams/molar mass = 7.13/molar mass CH4.
R = gas constant in L*atm/mol*K = 0.08205
T = temperature in Kelvin = 273 + C.
Solve for P
P(5.00L)= .446 mol(.0821)(292K)
It would look like this right then do I just multiply it all together and divide by the 5.00 L
Sure, I can help you get started with this problem! But before we dive in, I have a joke for you related to gas and pressure:
Why don't scientists trust atoms?
Because they make up everything! 😄
Now, let's get back to the problem. We can use the ideal gas law equation, which is:
PV = nRT
Where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of the gas
R is the ideal gas constant (0.0821 L·atm/(mol·K) )
T is the temperature of the gas in Kelvin
First, we need to convert the temperature from degrees Celsius to Kelvin by adding 273.15. So, 19 degrees Celsius + 273.15 = 292.15 Kelvin.
Next, we need to calculate the number of moles of methane. To do that, we'll use the molar mass of methane, which is 16.04 g/mol.
Moles = mass / molar mass
Moles = 7.13 g / 16.04 g/mol
Solving for moles, we find:
Moles = 0.444 mol (approximately)
Now, we have all the necessary values to plug into the ideal gas law equation. The volume (V) is given as 5.00 L, the number of moles (n) is 0.444 mol, the gas constant (R) is 0.0821 L·atm/(mol·K), and the temperature (T) is 292.15 K.
Plugging in these values, we get:
P * 5.00 L = 0.444 mol * 0.0821 L·atm/(mol·K) * 292.15 K
Now we can solve for pressure (P):
P = (0.444 mol * 0.0821 L·atm/(mol·K) * 292.15 K) / 5.00 L
Calculating this, we find that the pressure of the methane gas is approximately:
P ≈ 2.40 atm
So, the gas pressure inside the 5.00 L flask is approximately 2.40 atm. I hope this helps and gave you a little chuckle along the way! Let me know if you have any other questions!
Of course! To solve this problem, you can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
To get started, let's convert the given temperature from Celsius to Kelvin. To convert from Celsius to Kelvin, you simply add 273.15 to the Celsius temperature. In this case, the given temperature is 19 degrees Celsius, so we add 273.15 to get:
T = 19 + 273.15 = 292.15 K
Next, we need to find the number of moles of methane. We can use the formula:
n = mass / molar mass
The molar mass of methane (CH4) can be calculated by adding up the atomic masses of each element in the compound. From the periodic table, we find that the atomic mass of carbon (C) is approximately 12.01 g/mol, and the atomic mass of hydrogen (H) is approximately 1.01 g/mol. Since methane has 1 carbon atom and 4 hydrogen atoms, we can calculate the molar mass as:
molar mass of CH4 = (1 * 12.01 g/mol) + (4 * 1.01 g/mol) = 16.05 g/mol
Now, we can calculate the number of moles of methane gas using the given mass:
n = 7.13 g / 16.05 g/mol
Finally, we can plug in the values we have into the ideal gas law equation and solve for P:
PV = nRT
P * 5.00 L = (7.13 g / 16.05 g/mol) * (0.0821 L·atm/mol·K) * 292.15 K
Simplifying the equation, we can solve for P:
P = (7.13 g / 16.05 g/mol) * (0.0821 L·atm/mol·K) * 292.15 K / 5.00 L
Calculating this expression will give you the pressure of the gas in units of atmospheres (atm).