Answer:
112.92 s.
Explanation:
Let M₁ be the molar mass of N₂O
Let t₁ be the time taken for N₂O to effuse.
Let M₂ be the molar mass of I₂
Let t₂ be the time taken for I₂ to effuse.
Molar mass (M₁) of N₂O = (14×2) + 16 = 28 + 16 = 44 g/mol
Time (t₁) of effusion of N₂O = 47 s
Molar mass (M₂) of I₂ = 127 × 2 = 254 g/mol
Time (t₂ ) of effusion of I₂ =?
The time take for the same amount of I₂ to effuse can be obtained as follow:
t₂/t₁ = √(M₂/M₁)
t₂/47 = √(254 / 44)
Cross multiply
t₂ = 47 × √(254 / 44)
t₂ = 112.92 s
Therefore, it will take 112.92 s for the same amount of I₂ to effuse.
A. P1, V1, T1, P2, and V2: 3.5 atm, 3.2 L, 323 K, 1.5 atm, and 2.6 L, respectively
B. The problem is asking you to determine T2, the temperature of the gas based on the conditions above
C. Since pressure, volume, and temperature are all changing and are all interrelated, the combined gas law is best for this problem:
P1 • V1 P2 • V2
———— = ————
T1 T2
D. Substituting in all of the values above:
(3.5)(3.2) (1.5)(2.6)
————— = —————
(323) T2
(11.2) (3.9)
——— = ———
(323) T2
(3.9)
0.03467 = ———
T2
(3.9)
T2 = ————— = 112.49 K
0.03467
The second temperature under these conditions would be about 112.49 K.
Hope this helps!
Answer:
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