A diver exhales a bubble with a volume of 25 mL at a pressure of 2.4 atm and a temperature of 15 degrees C. how many gas particles are in this bubble?
I would use PV = nRT and solve for n = number of moles gas. One mole contains 6.022E23 molecules.
We did that and somehow got the wrong answer. can you please give me a step by step?
Thank you...
n= PV/RT
n={(2.4)x(25)}/{(.082)x(288)
-> n x 6.022x10^23 = answer
niki has posted but the 25 mL must be inserted as 0.025 L
Thank you,
we were doing,
n=VRT
P
To determine the number of gas particles in the bubble, we can use the ideal gas law equation, which states:
PV = nRT
where:
P = pressure
V = volume
n = number of gas particles (in moles)
R = ideal gas constant
T = temperature
First, we need to convert the given values to appropriate SI units. The pressure should be in pascals (Pa), volume in cubic meters (m³), and temperature in Kelvin (K).
Given:
Volume (V) = 25 mL = 25 × 10^(-6) m³ (converted to m³)
Pressure (P) = 2.4 atm = 2.4 × 101,325 Pa (converted to Pa)
Temperature (T) = 15 °C = 15 + 273.15 K (converted to K)
Now we can rearrange the ideal gas law equation to solve for n:
n = (PV) / (RT)
Using the given values and the ideal gas constant R (8.314 J/(mol⋅K)), we can calculate the number of gas particles:
n = ((2.4 × 101,325) × (25 × 10^(-6))) / (8.314 × 288.15)
Simplifying the equation, we get:
n ≈ 0.0243 moles
To convert from moles to the number of gas particles, we can use Avogadro's number, which is approximately 6.022 × 10^23 particles/mol.
Number of gas particles = 0.0243 moles × 6.022 × 10^23 particles/mol
Thus, the number of gas particles in the bubble is approximately 1.464 × 10^22 particles.