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tigry1 [53]
3 years ago
8

What is the molecular weight of a gas that diffuses through a porous membrane 2.17 times faster than Xe?

Chemistry
1 answer:
vivado [14]3 years ago
8 0

Answer: The molecular weight of the gas 28. The gas is probably N2

Explanation:Please see attachment for explanation

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Air containing 20.0 mol% water vapor at an initial pressure of 1 atm absolute is cooled in a 1- liter sealed vessel from 200°C t
chubhunter [2.5K]

Answer:

This solution is quite lengthy

Total system = nRT

n was solved to be 0.02575

nH20 = 0.2x0.02575

= 0.00515

Nair = 0.0206

PH20 = 0.19999

Pair = 1-0.19999

= 0.80001

At 15⁰c

Pair = 0.4786atm

I used antoine's equation to get pressure

The pressure = 0.50

2. Moles of water vapor = 0.0007084

Moles of condensed water = 0.0044416

Grams of condensed water = 0.07994

Please refer to attachment. All solution is in there.

6 0
3 years ago
When water reacts with potassium metal the hydrogen produced ignites explosively on the surface of water .What cause the ignitio
Julli [10]

Answer:

Pottasium reacts with water vigorously and the reation is exothermic. The heat released causes the hydrogen released to ignite

Explanation:

7 0
3 years ago
The density of copper is listed as 8.94g/cm​ 3​ . Two students each make three density determinations of samples of the substanc
amm1812

Answer:

Density of the copper = 8.94g/cm^3

Student A results = 7.3gm/cm^3 ,9.4 gm/cm^3 , 8.3gm/cm^3

Student B results = 8.4 gm/cm^3 , 8.8 gm/cm^3 , 8gm/cm^3

From the observations we conclude that

Student A's result is accurate but not  precise as the trials noted are not close to each other.

Student B's result is accurate and precise as the trials noted are close to each other.

Mean density of student A = 7.3 + 9.4 + 8.3 /3 = 8.33gm/cm^3

Mean density of student B = 8.4 + 8.8 + 8 /3 = 8.4 gm/cm^3

both the densities of A and B are 0.5 away from the actual density.

5 0
3 years ago
A sample of krypton gas with a volume of 10.00 L has a temp of 303 K and exerts
marshall27 [118]

<u>Answer:</u> The final volume will be 14.85 L.

<u>Explanation:</u>

To calculate the final volume when temperature increases, we use Charles' Law.

This law states that volume is directly proportional to the temperature of the gas if number of moles and pressure remains constant.

V\propto T\\\\\frac{V_1}{T_1}=\frac{V_2}{T_2}

where,

V_1\text{ and }T_1 = Initial volume and temperature

V_2\text{ and }T_2 = Final volume and temperature

We are given:

V_1=10L\\&#10;T_1=303K\\&#10;V_2=?L\\&#10;T_2=450K

Putting values in above equation, we get:

\frac{10L}{303K}=\frac{V_2}{450K}

V_2=14.85L

Hence, the final volume of the gas is 14.85L

7 0
3 years ago
How many moles of CO2 are produced from the combustion of 5.25 moles of CH3OH?
iVinArrow [24]

First, we write the reaction for CH3OH combustion

CH3OH+3/2O2--->CO2+2H2O

for 1 mole of methanol, we get 1 mole of CO2, therefore for 5,25 moles of methanol we will get 5,25 moles of CO2

4 0
3 years ago
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