The volume of the stock solution that has a concentration of 1.5 M SO2 and is diluted to a 0.54 M solution with a volume of 0.18 L is 0.065L.
<h3>How to calculate volume?</h3>
The concentration of a solution can be calculated using the following formula:
C1V1 = C2V2
Where;
- C1 = initial concentration = 1.5M
- C2 = final concentration = 0.54M
- V1 = initial volume = ?
- V2 = final volume = 0.18L
1.5 × V1 = 0.54 × 0.18
1.5V1 = 0.0972
V1 = 0.0972 ÷ 1.5
V1 = 0.065L
Therefore, the volume of the stock solution that has a concentration of 1.5 M SO2 and is diluted to a 0.54 M solution with a volume of 0.18 L is 0.065L.
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Answer:
2-chloro-4-methylpentanal.
Explanation:
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In this case, according to the chemical compound:
CH3-CH-CH2-CH-CHO
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CH3 Cl
We can see the main functional group is an starting carbonyl, which means this is an aldehyde. Moreover, we can see a Cl-substituent on the second carbon and a methyl substituent on the fourth carbon. Therefore, the IUPAC name turns out: 2-chloro-4-methylpentanal.
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Answer:
0.861 L
Explanation:
We are given pressure, volume, and temperature, so let's apply the Combined Gas Law:
(P₁V₁)/T₁ = (P₂V₂)/T₂
Convert the temperatures to degrees Kelvin.
25.0°C -> 298 K, 100.0°C -> 373 K
Plug in the initial conditions on the left, then the final/new on the right, and solve for the unknown:
(165(2.5))/298 = (600(V₂))/373
V₂ = (165(2.5)(373))/(298(600))
V₂ = 0.861 L
The output density is given as kg/m 3, lb/ft 3, lb/gal(US liq) and sl/ft 3. Specific weight is given as N/m 3 and lb f / ft 3.
The gas inside the can and the can’s volume are both constant.
The gas pressure increases with increasing temperature.
The can will burst if the pressure becomes great enough.
The gas law that applies is Gay-Lussac’s law.
