Answer:
Increase
Explanation:
According to Gay-Lussac Law,
The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.
Mathematical relationship:
P₁/T₁ = P₂/T₂
If the initial temperature and pressure is standard,
Pressure = 1 atm
Temperature = 273.15 K
then we increase the temperature to 400.0 K, The pressure will be,
1 atm / 273.15 K = P₂/400.0K
P₂ = 1 atm × 400.0 K / 273.15 K
P₂ = 400.0 atm. K /273.15 K
P₂ = 1.46 atm
Pressure is also increase from 1 atm to 1.46 atm.
The twin primes between 1 and 100 are; (3, 5), (5, 7), (11, 13), (17, 19), (29, 31), (41, 43), (59, 61), (71, 73). Hope this helped<3
Answer:
no, the correct answer is NaCI
Explanation:
you're welcome
Answer:
About 5 times faster.
Explanation:
Hello,
In this case, since the Arrhenius equation is considered for both the catalyzed reaction (1) and the uncatalized reaction (2), one determines the relationship between them as follows:

By replacing the corresponding values we obtain:

Such result means that the catalyzed reaction is about five times faster than the uncatalyzed reaction.
Best regards.