Answer:
Option 5. 179L
Explanation:
The reaction is:
2 HCl + Na₂CO₃ → 2NaCl + H₂O + CO₂
The amount of collected CO₂ is 8 moles.
We apply the Ideal Gases Law at STP
STP are 1 atm of pressure and 273K of T°
P . V = n . R . T
1atm . V = 8 mol .0.082L.atm/mol.K . 273K
V = (8 mol .0.082L.atm/mol.K . 273K) / 1 atm = 179 L
Halogens (atoms with 7 valence electrons) and Hydrogen
or generally, atoms with their shells almost full
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:
the atomic mass number for boron is 5
Explanation:
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