What pressure (in atmospheres) will be exerted by 1.3 moles of gas in a 13 litre flask at 22 degrees Celcius? (Gas constant (R) = 0.0821 L atm K^-1 mol^-1)

Use ideal gas law:

PV=nRT (T in °K)

=>

P=nRT/V
=1.3 mol *0.0821 L atm °K-1 mol-1 *(22+273.16)°K/13 L
=2.423 atm
=2.4 atm (approx.)

Well, let's put on our funny hats and break out the math humor! Ready? Here we go:

First, we need to use the ideal gas law, which is like the comedian of gas laws. It goes: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

Now, let's solve it step by step. First, we need to convert the temperature from Celsius to Kelvin. So, to Kelvin we goooo! Adding 273 to 22 gives us 295 Kelvin.

Next, we plug the values into the equation. We know that n is 1.3 moles, R is 0.0821 L atm K^-1 mol^-1, V is 13 liters, and T is 295 Kelvin.

PV = nRT becomes P * 13 = 1.3 * 0.0821 * 295

Now let's solve for P. Dividing both sides of the equation by 13 gives us:

P = (1.3 * 0.0821 * 295) / 13

Calculating this funny business gets us a pressure of approximately 2.234 atmospheres.

So, to answer your question (and hopefully make you laugh), 1.3 moles of gas in a 13-liter flask at 22 degrees Celsius will exert a pressure of about 2.234 atmospheres.

To find the pressure exerted by the gas, we can use the Ideal Gas Law equation:

PV = nRT

where:
P = pressure
V = volume
n = number of moles
R = gas constant
T = temperature

Given:
n = 1.3 moles
V = 13 liters
R = 0.0821 L atm K^-1 mol^-1
T = 22 degrees Celsius = 22 + 273 = 295 Kelvin

Substituting these values into the equation, we have:

P * 13 = 1.3 * 0.0821 * 295

Now, solve for P:

P = (1.3 * 0.0821 * 295) / 13
P ≈ 2.9322 atm

Therefore, the pressure exerted by 1.3 moles of gas in a 13-liter flask at 22 degrees Celsius is approximately 2.9322 atmospheres.

To find the pressure exerted by the gas, we can use the ideal gas law equation:

PV = nRT

where:
P is the pressure in atmospheres (atm)
V is the volume of the gas in liters (L)
n is the number of moles of the gas (mol)
R is the ideal gas constant (0.0821 L atm K^-1 mol^-1)
T is the temperature in Kelvin (K)

First, we need to convert the given temperature from Celsius to Kelvin by adding 273.15 to it:
22°C + 273.15 = 295.15 K

Next, we can substitute the given values into the ideal gas law equation and solve for pressure (P):

P * 13 L = 1.3 mol * 0.0821 L atm K^-1 mol^-1 * 295.15 K

P * 13 L = 32.3776 L atm

P = 32.3776 L atm / 13 L

P ≈ 2.49 atm

Therefore, the pressure exerted by 1.3 moles of gas in a 13 liter flask at 22 degrees Celsius is approximately 2.49 atmospheres.