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goldenfox [79]
1 year ago
11

A sealed container of N2 gas has a pressure of 836 kPa at 54.7 ∘ C. After it is left out in the sun the pressure increases by 79

.9 kPa. What is the new temperature of the container?
Chemistry
1 answer:
Anuta_ua [19.1K]1 year ago
5 0
P1=836kPa
T1=54.7+273=327.7K
P2=836+79.9=915.9kPa
T2=?
T2=T1*P2/P1
=327.7*915.9/836
=359K=86 degree celsius
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Given that the initial rate constant is 0.0110s−1 at an initial temperature of 21 ∘C , what would the rate constant be at a temp
gulaghasi [49]

The rate constant is mathematically given as

K2=2.67sec^{-1}

<h3>What is the Arrhenius equation?</h3>

The rate constant for a particular reaction may be calculated with the use of the Arrhenius equation. This constant can be stated in terms of two distinct temperatures, T1 and T2, as follows:

ln(\frac{K2}{K1})= (\frac{Ea}{R})*(\frac{1}{T1}-\frac{1}{T2})

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T1= 21+273.15

T1= 294.15K

T2= 200  

T2=200+273.15

T2= 473.15K

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Hence, in  j/mol R Ea is

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ln(\frac{K2}{0.0110})= (\frac{35.5*1000}{8.314})*(\frac{1}{294.15}-\frac{1}{473.15}\\\\ln(\frac{K2}{0.0110})=5.492

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K2/0.0110 =242.74

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In conclusion, rate constant

K2=2.67sec^{-1}

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A gas occupies a volume at 34.2 mL at a temperature of 15.0 C and a pressure of 800.0 torr. What will be the volume of this gas
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The answer is 34.1 mL.
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