T₁ = 27°C = 27 + 273 = 300K, V₁ = 6 L,
T₂ = 150°C = 150 + 273 = 423K, V₂ = ?,
By Charles' Law: V₁/T₁= V₂/T₂
6/300 = V₂/423
423*(6/300) = V₂
8.46 = V₂
Volume at 150°C =8.46 L.
Answer:
Explanation:
Hello,
In this case, we can compute the required volume by using the ideal gas equation as shown below:
Thus, solving for the volume and considering absolute temperature (in Kelvins), we obtain:
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Answer:
10.6 grams is approximately 0.10 moles. So you would need about 0.10 moles of sulfuric acid. That converts to about 9.80 grams.
Explanation:
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Answer:
0.107 mole of SO2.
Explanation:
1 mole of a gas occupy 22.4 L at standard temperature and pressure (STP).
With the above information, we can simply calculate the number of mole of SO2 that will occupy 2.4 L at STP.
This can be obtained as follow:
22.4 L contains 1 mole of SO2.
Therefore, 2.4 L will contain = 2.4/22.4 = 0.107 mole of SO2.
Therefore, 0.107 mole of SO2 is present in 2.4 L at STP.
