Respuesta :
0.0169 bars pressure (in atm and in bars) is exerted by a column of methanol (ch3oh) 225 m high, the density of methanol is 0.787 g/cm3.
To calculate the pressure exerted by a column of methanol, we need to use the ideal gas law equation:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. First, we need to determine the volume of the methanol column. Since the density of methanol is 0.787 g/cm3 and the height of the column is 225 m, we can calculate the volume of the column using the formula:
Volume = density * height
= 0.787 g/cm3 * 225 m
= 177.175 cm3
Next, we need to convert the volume to liters. Since 1 liter is equal to 1000 cm3, the volume of the methanol column is 177.175 cm3 / 1000 cm3/L = 0.177175 L.
Now we can use the ideal gas law equation to calculate the pressure exerted by the methanol column. Let's assume that the temperature is 25°C, which is 298.15 K. The ideal gas constant is 8.31 J/mol*K. Since the molar mass of methanol is 32.04 g/mol, the number of moles of methanol in the column is:
Number of moles = mass / molar mass
= 0.787 g/cm3 * 225 m / 32.04 g/mol
= 0.049 mol
Plugging these values into the ideal gas law equation, we get:
P = (0.049 mol * 8.31 J/molK) / (0.177175 L * 298.15 K)
= 1693.6 J/LK
To convert this pressure to atmospheres (atm), we can use the conversion factor 1 atm = 101325 Pa. The pressure in atm is therefore:
P (atm) = 1693.6 J/L*K / 101325 Pa/atm
= 0.0167 atm
To convert the pressure to bars, we can use the conversion factor 1 bar = 100000 Pa. The pressure in bars is therefore:
P (bar) = 1693.6 J/L*K / 100000 Pa/bar
= 0.0169 bar
To know more about methanol please refer: https://brainly.com/question/24077457
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