How many moles of gas will occupy 6.75 m3 at 65.0°C and 3.28 x 105 Pa?

A. 7.98 x 104 mol
B. 4.10 x 103 mol
C. 7.88 x 102 mol
D. 4.15 x 105 mol

The answer is c sorry

How u get 7.88 x 10^2 help

How many moles of gas will occupy 6.75 m^3 at 65.0°C and 3.28 x 10^5 Pa?

A. 7.98 x 10^4 mol
B. 4.10 x 10^3 mol
C. 7.88 x 10^2 mol
D. 4.15 x 10^5 mol

right

I'm no expert, but I do know that gas loves to occupy space and make themselves at home. It's like they're the "moles" of the party! So, let's calculate how many moles of gas are in this scenario.

We can use the ideal gas law equation to help us out: PV = nRT. It's like the gas equivalent of making a deal. It stands for Pressure times Volume equals the number of moles, R is the ideal gas constant, and T is the temperature.

Now, let's plug in the given values. We have a volume of 6.75 m3, a temperature of 65.0°C (which we'll have to convert to Kelvin by adding 273.15), and a pressure of 3.28 x 105 Pa.

PV = nRT

(3.28 x 105 Pa) * (6.75 m3) = n * R * (65.0°C + 273.15 K)

And after some calculations, we find that n (the number of moles) is approximately 4.10 x 103 mol.

So, the answer is option B: 4.10 x 103 mol.

To find the number of moles of gas that will occupy a given volume, temperature, and pressure, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in Pascals)
V = volume (in cubic meters)
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature (in Kelvin)

First, let's convert the given temperature from Celsius to Kelvin.

T(K) = T(°C) + 273.15
T(K) = 65.0 + 273.15
T(K) = 338.15 K

Now, we can rearrange the equation to solve for the number of moles (n):

n = PV / RT

Substituting the given values:

n = (3.28 x 10^5 Pa) * (6.75 m^3) / ((8.314 J/(mol·K)) * (338.15 K))

n ≈ 7.88 x 10^2 mol

Therefore, the correct answer is option C. 7.88 x 10^2 mol.