A gas is contained in a thick walled balloon. When the pressure changed from 1.21 atm to 2.52 atm, the volume changes from 3.75 to 1.72 L and the temperature changed from 293 k to k
Answers
Answer:
this is your answer
By applying the formula
=(2.95 atm 7.456L / 212p²k ) /(379k × 4.782 L) = 2.57 atm
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Answer:
The pressure changes from 1.21 atm to 2.52 atm, the volume changes from 3.75 L to 1.72 L and the temperature changes from 293 K to n.
Explanation:
Step 1: -----> P = pressure (atm)
-----> V = volume (L)
-----> T = temperature (K)
-----> n = number of moles
Step 2:According to the problem, it seems like pressure (P), volume (V), and temperature (T) are all changing. The problem never brings up whether the number of moles (n) has changed. Therefore, the number of moles (n) must have been held constant.
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Step 3:If you need to know what the temperature changes to....
When the number of moles is held constant, you can find the change in the other variables using the Combined Gas Law equation:
P₁V₁ / T₁ = P₂V₂ / T₂
In this formula, "P₁", "V₁", and "T₁" represent the initial pressure, volume, and temperature. "P₂", "V₂", and "T₂" represent the final pressure, volume, and temperature. You can find the final temperature by plugging in the given values and simplifying.
P₁ = 1.21 atm P₂ = 2.52 atm
V₁ = 3.75 L V₂ = 1.72 L
T₁ = 293 K T₂ = ? K
P₁V₁ / T₁ = P₂V₂ / T₂ <----- Equation
(1.21 atm)(3.75 L) / (293 K) = (2.52 atm)(1.72 L) / T₂ <----- Insert values
0.015486 = (2.52 atm)(1.72 L) / T₂ <----- Simplify left side
0.015486 = 4.3344 / T₂ <----- Multiply 2.52 and 1.72
0.015486 x T₂ = 4.3344 <----- Multiply both sides by T₂
T₂ = 279.885 <----- Divide both sides by 0.015486
T₂ = 280 K <----- Answer in correct sig figs
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