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Sagot :
Answer:
T = 4.062V
Explanation:
from PV = nRT => T = PV/RT
P = 1 atm
V = Final Volume
n = 3 moles
R = 0.08206 L·atm/mol·K
T = ?
T = 1 atm · V(Liters)/(3 moles)(0.08206L·atm/mol·K) = 4.062·V(final) Kelvin
The temperature of the balloon is 406 K
We'll begin by listing out what was given from the question. This is shown below:
Volume (V) = 100 L
Mole of oxygen (n) = 3 moles
Pressure (P) = 1 atm
Temperature (T) =?
We can obtain the temperature of the balloon by using the ideal gas equation as shown below:
PV = nRT
NOTE:
P is the pressure.
V is the volume.
n is the number of mole
R is the gas constant (0.0821 atm.L/Kmol)
T is the temperature.
Applying the ideal gas equation, we have:
PV = nRT
1 × 100 = 3 × 0.0821 × T
100 = 0.2463 × T
Divide both side by 0.2463
T = 100 / 0.2463
T = 406 K
Therefore, the temperature of the balloon is 406 K
Learn more: https://brainly.com/question/17046345
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