If 37.5 mol of an ideal gas occupies 38.5 Lat 85.00°C, what is the pressure of the gas?

Question

Mateo Aguilar · Accepted Answer

#P~=29*atm# #P=(nRT)/V# #=# #(37.5*cancel(mol)xx0.0821*cancelL*atm*cancel(K^-1)*cancel(mol^-1)xx358.15*cancelK)/(38.5*cancelL)# Note that the equation is consistent dimensionally. We wanted an answer in #"atmospheres"# and we got one. When we do equations like this, the gas constant #R# can have many different values, each with different units. For chemists, probably the most useful one is #R=0.0821*L*atm*K^-1*mol^-1#. These need not be learned, because they will appear as supplementary material on the exam paper. They do have to be used correctly.

Olivia Anton · Answer

undefined To find the pressure of the gas, 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 Kelvin. First, we need to convert the temperature from Celsius to Kelvin by adding 273.15. Then, we can rearrange the equation to solve for pressure, $P$, using the given values of $n$, $V$, and $T$, and the ideal gas constant $R$. Let's calculate.

Jeremiah Adams · Answer

undefined To find the pressure of the gas, we can use the ideal gas law equation: PV = nRT. Where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin using the formula: Kelvin = Celsius + 273.15. So, 85.00°C + 273.15 = 358.15 K.

Next, we plug in the given values into the ideal gas law equation:
P * 38.5 L = (37.5 mol) * (0.0821 L*atm/mol*K) * 358.15 K

Solving for P:
P = (37.5 * 0.0821 * 358.15) / 38.5

P ≈ 28.98 atm

So, the pressure of the gas is approximately 28.98 atm.