at a deep-sea station 200m below the surface of the Pacific Ocean, workers live in a highly pressurized environment. How many lites of gas at STP must be compressed on the surface to fill the underwater environmen with 2.00 x 10^7 of gas at 20.0 atm?
What gas law do you use to find this?
at a deep-sea station 200m below the surface of the Pacific Ocean, workers live in a highly pressurized environment. How many lites of gas at STP must be compressed on the surface to fill the underwater environmen with 2.00 x 10^7 WHAT of gas at 20.0 atm?
at a deep-sea station 200m below the surface of the Pacific Ocean, workers live in a highly pressurized environment. How many lites of gas at STP must be compressed on the surface to fill the underwater environment with 2.00 x 10^7 L of gas at 20.0 atm?
P1V1 = P2V2
1 atm *V1 = 20 atm*2.00 x 10^7 L
Solve for V1. This assumes the T in the underwater compartment is standard although it probably isn't.
To find the amount of gas at STP (Standard Temperature and Pressure) needed to fill the underwater environment, you can use the ideal gas law equation: PV = nRT. In this equation, P represents the pressure, V represents the volume, n represents the number of moles of gas, R is the ideal gas constant, and T represents the temperature.
In this scenario, the pressure is given as 20.0 atm, and the volume is unknown, representing the volume of the underwater environment at a depth of 200m below the surface. The goal is to calculate the number of moles of gas (n) needed to fill this volume at STP.
To use the ideal gas law, you need to convert the given pressure (20.0 atm) to units of Pascals, as the ideal gas constant (R) is typically given in those units. The conversion factor is 1 atm = 101,325 Pa.
Once you have converted the pressure to Pascals, you can proceed with the equation:
PV = nRT
Where:
P = Pressure in Pascals (Pa)
V = Volume in liters (L) at STP (standard conditions are 1 atm and 273.15 K)
n = Number of moles of gas
R = Ideal gas constant, which is approximately 0.0821 L · atm/mol · K
T = Temperature in Kelvin (K)
Now, let's solve the equation using the given values:
P = 20.0 atm * 101,325 Pa/atm = 2,026,500 Pa
V = unknown (volume of the underwater environment at a depth of 200m below the surface)
n = 2.00 x 10^7 moles (given)
R = 0.0821 L · atm/mol · K (constant)
T = 273.15 K (standard temperature)
Plug in the values into the formula and rearrange to solve for V:
V = (n * R * T) / P
V = (2.00 x 10^7 moles * 0.0821 L · atm/mol · K * 273.15 K) / 2,026,500 Pa
Now, you can calculate V to find the volume of the underwater environment at STP needed to hold 2.00 x 10^7 moles of gas.