3 years ago

The vapor pressure of ethanol at 25°C is 7.828 kPa . Calculate the vapor pressure in atm .

1 answer:

8 0

<span>First you get 7.83 kPa = 7.83 * 10^4 Pa Then convert it to atm by using the relation 1 Pa = 9.8692 * 10^-6 atm, this gives you 7.83 kPa = 7.83 * 10^4 * 9.8692 * 10^-6 atm = 77.275836 * 10^-2 atm = 0.77275836 atm Now round to three significant digits, = 0.773 atm</span>

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125 ml of nitrogen gas is collected at 70.0 degrees Celsius. The pressure

dybincka [34]

Answer: Volume of the gas at STP is 22.53 L.

Explanation:

Given : Volume = 125 mL (as 1 mL = 0.001 L) = 0.125 L

Temperature = $70^{o}C = (70 + 273) K = 343 K$

Pressure = $125 kPa = 125 kPa \times \frac{0.01 atm}{1 kPa} = 1.25 atm$

According to the ideal gas equation, the volume of given nitrogen gas is calculated as follows.

PV = nRT

where,

P = pressure

V = volume

n = number of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

$1.25 atm \times V = 1 mol \times 0.0821 L atm/mol K \times 343 K\\V = \frac{1 mol \times 0.0821 L atm/mol K \times 343 K}{1.25 atm}\\= \frac{28.1603}{1.25} L\\= 22.53 L$