Use the universal gas formula
PV=nRT
where
P=pressure ( 0.980 atm)
V=volume (L)
T=temperature ( 23 ° C = 23+273.15 = 296.15 ° K)
n=number of moles of ideal gas (0.485 mol)
R=universal gas constant = 0.08205 L atm / (mol·K)
Substitute values,
Volume, V (in litres)
=nRT/P
=0.485*0.08205*296.15/0.980
= 12.0256 L
= 12.0 L (to three significant figures)
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Answer:
4.50 L
Explanation:
First we <u>calculate how many moles are there in 3.84 L of a 8.50 mol/L solution</u>:
- 3.84 L * 8.50 mol/L = 32.64 mol
Now, keeping in mind that
- Concentration = Mol / Volume
we can calculate the volume of a 7.25 mol/L solution that would contain 32.64 moles:
- Volume = Mol / Concentration
- Volume = 32.64 mol ÷ 7.25 mol/L
So we could take 4.50 L of the 7.25 mol/L solution and evaporate the solvent until only 3.84 L remain.
Answer:
Do you have options of answers for this question
Answer:
An element X reacts with oxygen to form XO
and with chlorine to form XCl
. XO
is a white solid that melts at high temperatures (above 1000 degrees C). Under usual conditions, XCl
is a colorless liquid with a boiling point of 58 degrees C.
Explanation:
Answer:
The amount of heat released is 11.3 KJ
Explanation:
H20(g) -> H20(l) + heat
This reaction is changing state from gaseous to liquid without changing the temperature. This heat is know as Latent heat. It is the energy required for a phase change.
Heat released by 5 g of water vapor (Q) = M × L
where M = mass of vapor
L= latent heat
Latent heat can be divide into 2
- Latent heat of fusion
- Latent heat of vaporization
Since we are change the gaseous state to liquid, we will be working with Latent heat of vaporization which has a value of 22.6 x 10 ∧5 J/kg
(Q) = M × L
= 0.005 x 22.6 x 10 ∧5
= 11300 J
= 11.3 KJ
