Answer:
The answer to your question is V2 = 1.3 l
Explanation:
Data
Pressure 1 = P1 = 1.5 atm
Volume 1 = V1 = 2.50 l
Temperature 1 = T1 = 22°C
Pressure 2 = P2 = 3 atm
Volume 2 = V2 = ?
Temperature 2 = T2 = 35°C
Process
1.- Convert temperature to °K
T1 = 22 + 273 = 295°K
T2 = 35 + 273 = 308°K
2.- Use the combine gas law to solve this problem
P1V1/T1 = P2V2/T2
-Solve for V2
V2 = P1V1T2 / T1P2
3.- Substitution
V2 = (1.5 x 2.5 x 308) / (295 x 3)
4.- Simplification
V2 = 1155 / 885
5.- Result
V2 = 1.3 l
Answer:
One that “Can be answered by conducting an experiment”
Explanation:
Answer:
the atoms of the original substances gain, lose and even share their very own electrons. write the symbols of the elements that form the compound. Write down the valency, and lastly go over valencies. This is all I got so far. I hope this helps
Explanation:
Answer:
Final temperature is 302 K
Explanation:
You can now initial volume with ideal gas law, thus:
V = 
Where:
n are moles: 2 moles
R is gas constant: 0,082 
T is temperature: 300 K
P is pressure: 1 atm
V is volume, with these values: <em>49,2 L</em>
The work in the expansion of the gas, W, is: 1216 J - 34166 J = <em>-32950 J</em>
This work is:
W = P (Vf- Vi)
Where P is constant pressure, 1 atm
And Vf and Vi are final and initial volume in the expansion
-32950 J = -1 atm (Vf-49,2L) × 
Solving: <em>Vf = 49,52 L</em>
Thus, final temperature could be obtained from ideal gas law, again:
T = 
Where:
n are moles: 2 moles
R is gas constant: 0,082
P is pressure: 1 atm
V is volume: 49,52 L
T is final temperature: <em>302 K</em>
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I hope it helps!
Answer:
<u>C</u>
Explanation:
The percent composition of an atom in a molecule gives information regarding the relative amount of mass an atom contributes to a molecule.
