What is the density of wet air with 75% relative humidity at 1atm and 300K? Given : vapour pressure of #H_2O# is 30 torr and average molar mass of air is 29g/mol?
#a)# #"1.174 g/L"#
#b)# #"1.156 g/L"#
#c)# #"1.178 g/L"#
#d)# #"1.143 g/L"#
In this case we have
This variant on the ideal gas law, assuming air is an ideal gas, can be used to find its density:
where:
In a given volume of air at a given temperature and total pressure, the density for ideal gases is additive, i.e.
Thus, the density of the wet air is given by:
By signing up, you agree to our Terms of Service and Privacy Policy
To calculate the density of wet air, we first need to find the partial pressure of water vapor using the given relative humidity and vapor pressure of water at the given temperature. Then, we can use Dalton's Law of Partial Pressures to find the partial pressure of dry air. Finally, using the ideal gas law, we can calculate the density of wet air.

Calculate the partial pressure of water vapor:
 Relative humidity = 75%
 Vapor pressure of water (at 300K) = 30 torr
 Partial pressure of water vapor = (Relative humidity / 100) * Vapor pressure of water

Calculate the partial pressure of dry air:
 Partial pressure of dry air = Total pressure  Partial pressure of water vapor

Use the ideal gas law to find the density of wet air:
 PV = nRT
 Density = (total mass) / (total volume)
 Total mass = mass of dry air + mass of water vapor
 Total volume = volume of dry air + volume of water vapor

Substitute known values and calculate the density of wet air.
By signing up, you agree to our Terms of Service and Privacy Policy
To calculate the density of wet air with 75% relative humidity at 1 atm and 300 K, we first need to find the partial pressure of water vapor using the given vapor pressure of H2O at 75% relative humidity. Then, we can use the ideal gas law to find the total pressure of the wet air. Finally, we can use the ideal gas law again to find the density of wet air.

Calculate the partial pressure of water vapor: Partial pressure of water vapor = Relative humidity * Vapor pressure of water at given temperature Partial pressure of water vapor = 0.75 * 30 torr = 22.5 torr

Find the total pressure of the wet air: Total pressure of wet air = Atmospheric pressure  Partial pressure of water vapor Total pressure of wet air = 1 atm  (22.5 torr / 760 torr/atm) ≈ 0.970 atm

Use the ideal gas law to find the density of wet air: PV = nRT n = m/M (where n is the number of moles, m is the mass, and M is the molar mass) Density = (m/V) = (P*M) / (RT)
Density of wet air = (Total pressure * Molar mass of air) / (Universal gas constant * Temperature) Density of wet air = (0.970 atm * 29 g/mol) / (0.0821 atmL/molK * 300 K) ≈ 1.07 g/L
So, the density of wet air with 75% relative humidity at 1 atm and 300 K is approximately 1.07 g/L.
By signing up, you agree to our Terms of Service and Privacy Policy
When evaluating a onesided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a onesided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a onesided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a onesided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
 Given the equation #C_2H_6(g) + O_2(g) > CO_2 (g) + H_2O(g)# (not balanced), what is the number of liters of #CO_2# formed at STP when 240.0 grams of #C_2H_6# is burned in excess oxygen gas?
 The temperature of a balloon increases from 25 K to 50 K. What will the final volume of the balloon be if it was 1 L before the temperature change?
 A 2.0 L container of nitrogen had a pressure of 3.2 atm. What volume would be necessary to decrease the pressure to 1 atm?
 A volume of 50.0 milliliters of an ideal gas at STP increases to 100 milliliters. If the pressure remains constant, what must the new temperature be?
 The pressure in a car tire is 205 kPa at 303 K. After a long drive, the pressure is 238 kPa. What is the temperature of the air in the tire?
 98% accuracy study help
 Covers math, physics, chemistry, biology, and more
 Stepbystep, indepth guides
 Readily available 24/7