Determine the pressure change when a constant volume of gas at 1.00 atm is heated from 20.0 c to 30.0 c

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Determine the pressure change when a constant volume of gas at 1.00 atm is heated from 20.0 C to 30.0 C

We have the following information:

P1 (initial pressure) = 1 atm

T1 (initial temperature) = 20 ºC (in Kelvin)

TK = TºC+273.15 → TK = 20+273.15 → T1 (initial temperature) = 293.15 K

P2 (final pressure) = ? (in atm)

T2 (final temperature) = 30 ºC (in Kelvin)

TK = TºC+273.15 → TK = 30+273.15 → T2 (final temperature) = 303.15 K

According to the Law of Charles and Gay-Lussac in the study of gases, we have an isochoric (or isovolumetric) transformation when its volume remains constant or equal, if the temperature increases, the pressure increases and, if the temperature decreases, the pressure also decreases, they are directly proportional.then we will have the following formula:

multiply the means by the extremes

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I Hope this helps, greetings ... Dexteright02! =)

the answer is true. hope it .

a. the law of proportion states the combination of 2 atoms in a specific ratio to produce multiple compounds such as the given statement of question ‘1st compound contains 88.8 % cu ’ indicates 88.8 g of cu is present along with 11.2 g oxygen in 100 g of compound whereas the statement ‘2st compound contains 79.9 % cu ’ indicates 79.9 g of cu is present along with 20.1 g oxygen in 100 g of compound

1st compound contains 88.8 g cu

for cu

m = 63 g /mol

atomic % = 88.8 /63 = 1.42

for o

m = 16 g /mol

atomic % = 11.2 /16 = 0.7

b. the emperical formula of 1st compound is

cu1.4o0.7

cu2o