Answer:
The answer to your question is P = 0.18 atm
Explanation:
Data
mass of O₂ = 0.29 g
Volume = 2.3 l
Pressure = ?
Temperature = 9°C
constant of ideal gases = 0.082 atm l/mol°K
Process
1.- Convert the mass of O₂ to moles
16 g of O₂ -------------------- 1 mol
0.29 g of O₂ ---------------- x
x = (0.29 x 1)/16
x = 0.29/16
x = 0.018 moles
2.- Convert the temperature to °K
Temperature = 9 + 273 = 282°K
3.- Use the ideal gas law ro find the answer
PV = nRT
-Solve for P
P = nRT/V
-Substitution
P = (0.018 x 0.082 x 282) / 2.3
-Simplification
P = 0.416/2.3
-Result
P = 0.18 atm
Answer:
A. Ernest Rutherford
B.Bohr
C. Eugen Goldstein
D.. Santiago Ramon y cajal
E.john Dalton
F.isobars - a line drawn on a weather map connecting points of equal pressure is called isobars.
example.. argon 40
potassium 40
.two differences between isobars and isotopes.
isobars are those elements which have different atomic number but the same mass number. while isotopes are those elements having the same atomic number and different mass number..
two uses of isotopes.
uranium 235 - for nuclear fission and as fuel in unclear reactors.
# an isotope cobalt - used In the treatment for cancer
# an isotope iodine - used in treatment of goiter.
Explanation:
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Answer:
A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is 0.67 atm.
Step by Step Explanation?
Boyle's law states that in constant temperature the variation volume of gas is inversely proportional to the applied pressure.
The formula is,
P₁ x V₁ = P₂ × V₂
Where,
P₁ is initial pressure = 1 atm
P2 is final pressure = ? (Not Known)
V₁ is initial volume = 10 L
V₂ is final volume = 15 L
Now put the values in the formula,
\begin{gathered}\rm 1\times 10 = P_2\times 15\\\\\rm P_2 = \frac{10}{15\\} \\\\\rm P_2 = 0.67\end{gathered]
Therefore, the answer is 0.67 atm.
Answer:
ok
Explanation:
do you still need the answer sorry