At STP a sample of neon gas occupies 502
cm3. How many moles of neon gas does this represent? answer in mols
To determine the number of moles of neon gas, 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)
However, the given volume is in cubic centimeters (cm^3), so we need to convert it to cubic meters (m^3) before proceeding.
Given:
Volume (V) = 502 cm^3
To convert cm^3 to m^3, we divide by 1,000,000 (since there are 1,000,000 cm^3 in 1 m^3).
Volume (V) = 502 cm^3 ÷ 1,000,000 = 0.000502 m^3
Now, we substitute the values into the ideal gas law equation:
PV = nRT
Since the question states that the sample is at STP (Standard Temperature and Pressure), we can assume that the temperature is 273.15 K and the pressure is 1 atmosphere (or 101325 Pascals).
P = 101325 Pa
V = 0.000502 m^3
R = 8.314 J/(mol·K)
T = 273.15 K
Substituting the values into the equation:
(101325 Pa) * (0.000502 m^3) = n * (8.314 J/(mol·K)) * (273.15 K)
Simplifying the equation:
51.00315 = n * 2274.2261
Rearranging the equation to solve for n:
n = 51.00315 / 2274.2261
Using a calculator to divide the values:
n ≈ 0.0224 mol
Therefore, the number of moles of neon gas in the given sample at STP is approximately 0.0224 mol.
To calculate the number of moles, we can use the ideal gas equation: PV = nRT.
At STP (Standard Temperature and Pressure), the temperature (T) is 273.15 K, and the pressure (P) is 1 atmosphere (atm). The volume (V) given is 502 cm3, which needs to be converted to liters (L) by dividing by 1000.
So, V = 502 cm3 = 502/1000 L = 0.502 L.
Substituting these values into the ideal gas equation:
(1 atm) * (0.502 L) = n * (0.0821 L•atm/(mol•K)) * (273.15 K).
Simplifying the equation:
0.502 = n * 22.414.
Solving for n (the number of moles):
n = 0.502 / 22.414 ≈ 0.0224 mol.
Therefore, the sample of neon gas represents approximately 0.0224 moles.