To calculate the gauge pressure at which CO2 is pumped, we need to first understand the concept of specific gravity.
Specific gravity is the ratio of the density of a substance to the density of a reference substance. In this case, the reference substance is typically water.
The specific gravity of CO2 is given as 0.367. This means that CO2 is 0.367 times as dense as water.
Assuming the pressure unit is in pascals, we can calculate the density of CO2 at 335 K using the ideal gas law:
PV = nRT
Where:
P = Pressure (in pascals)
V = Volume (in m^3)
n = Number of moles
R = Ideal gas constant (8.314 J/(mol·K))
T = Temperature (in Kelvin)
To simplify the calculation, we can assume that the volume of CO2 is constant.
Next, we can determine the number of moles of CO2 using the specific gravity and the molar mass of CO2.
The molar mass of carbon dioxide is approximately 44.01 g/mol.
Given that the specific gravity is 0.367, it means that the density of CO2 is 0.367 times the density of water (1000 kg/m^3). Therefore, the density of CO2 can be calculated as:
density_CO2 = 0.367 * 1000 kg/m^3
Finally, we can calculate the gauge pressure using the density:
density_CO2 = moles_CO2 * molar_mass_CO2 / volume_CO2
Simplifying, we get:
P = (moles_CO2 * molar_mass_CO2 / volume_CO2) * R * T
Since the volume is constant, we can ignore it:
P = (moles_CO2 * molar_mass_CO2) * R * T
Using the relationships above, we can calculate the gauge pressure at which CO2 is pumped.
Carbon dioxide, as a gas, at 335 K is pumped at a very high pressure into an oil-well. If CO2 has a specific gravity of 0.367, then, calculate the gauge pressure at which CO2 is pumped.
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