The answer for the following problem is mentioned below.
- <u><em>Therefore the final temperature of the gas is 740 K</em></u>
Explanation:
Given:
Initial pressure of the gas (
) = 1.8 atm
Final pressure of the gas (
) = 4 atm
Initial temperature of the gas (
) = 60°C = 60 + 273 = 333 K
To solve:
Final temperature of the gas (
)
We know;
From the ideal gas equation;
we know;
P × V = n × R × T
So;
we can tell from the above equation;
<u> P ∝ T</u>
(i.e.)
<em> </em>
<em> = constant</em>
= 
Where;
= initial pressure of a gas
= final pressure of a gas
= initial temperature of a gas
= final temperature of a gas
= 
=
= 740 K
<u><em>Therefore the final temperature of the gas is 740 K</em></u>
Hey there!
MgCl₂
Find molar mass of magnesium chloride.
Mg: 1 x 24.305
Cl: 2 x 35.453
--------------------
95.211 grams
One mole of magnesium chloride has a mass of 95.211 grams.
We have 2.40 moles.
2.40 x 95.211 = 228.5
To 3 sig figs this is 229.
The mass of 2.40 moles of magnesium chloride is 229 grams.
Hope this helps!
Answer is in a pho
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ad it to a file host
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bit.
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Answer: Trade winds :)
Explanation: just took the test
72g H2O x 1 mol H2O/18.02g H2O = 3.99 mol H2O