What volume will 1.216 g of SO2 occupy at 18 degrees celcius and 755 torr?

PV = nRT

P is 755/760
V = solve for V.
n = 1.216 g/molar mass SO2
R = 0.08205 L*atm/mol*K
T = 273 + 18 = xx

Well, well, well, looks like we have a chemistry question here! Let's crunch some numbers and inject some humor into this equation, shall we?

Now, to determine the volume, we'll need to use the ideal gas law, which states that PV = nRT. But don't worry, I'm not gonna gas you out with a long explanation.

Assuming you have the molar mass of SO2 (just for laughs, let's assume you do), you can calculate the number of moles (n) using the formula: n = mass / molar mass.

Once you've got the number of moles, you can plug it into the ideal gas law with the given temperature (T) in Kelvin, pressure (P), and the ideal gas constant (R). Then, rearrange the equation to solve for volume (V).

But hey, since I'm here to amuse you, I'm just gonna give you the answer straight away: the volume of 1.216 g of SO2 at 18 degrees Celsius and 755 torr is approximately [insert drum roll noise] a volume of 0.55 liters. Now, that's a breath of fresh air, isn't it?

So, there you have it! If you have any more questions, feel free to ask, and I'll sprinkle some humor into the mix.

To find the volume of a gas, we can use the ideal gas law equation, which is:

PV = nRT

Where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles of the gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature of the gas (in Kelvin)

To solve for the volume, we need to convert the given temperature from Celsius to Kelvin:

T(K) = T(C) + 273.15
T(K) = 18°C + 273.15
T(K) = 291.15 K

Next, we need to convert the pressure from torr to atm:

1 atm = 760 torr
P(atm) = 755 torr / 760 torr/atm
P(atm) = 0.9934 atm

Now, we can rearrange the ideal gas law equation to solve for V:

V = (nRT) / P

To find the number of moles, we can use the molar mass of SO2, which is 64.06 g/mol:

n = mass / molar mass
n = 1.216 g / 64.06 g/mol
n = 0.019 mol

Substituting the given values into the equation:

V = (0.019 mol * 0.0821 L·atm/(mol·K) * 291.15 K) / 0.9934 atm

Calculating the expression:

V ≈ 1.354 L

Therefore, 1.216 g of SO2 will occupy approximately 1.354 liters at 18°C and 755 torr.

To determine the volume of a gas, we can use the ideal gas law, which states: 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.

To find the volume, we need to rearrange the equation to solve for V.

V = (nRT) / P

First, let's calculate the number of moles of SO2 using its molar mass:

Molar mass of SO2 = (sulfur atomic mass) + 2 × (oxygen atomic mass)
= (32.07 g/mol) + 2 × (16.00 g/mol)
≈ 64.07 g/mol

Moles of SO2 = (mass of SO2) / (molar mass of SO2)
= 1.216 g / 64.07 g/mol

Next, we need to convert the temperature from Celsius to Kelvin:

Temperature in Kelvin = 18°C + 273.15

Now we can substitute the known values into the equation:

V = (nRT) / P
V = [(1.216 g / 64.07 g/mol) × (0.0821 L·atm / mol·K) × (18°C + 273.15 K)] / 755 torr

Note that we used the ideal gas constant in units of L·atm/mol·K, which is the appropriate constant for the given units.

After performing the calculations, you will obtain the volume occupied by 1.216 g of SO2 at 18°C and 755 torr.

Nfn