119.7kPa
Explanation:
Given parameters:
Pressure of gas in balloon = 111kPa
Temperature of gas = 22°C
Final temperature = 45°C
Unknown:
Final pressure = ?
Solution:
Since the gases in the balloon have the same number of moles. We can apply a derivative of the combined gas law to solve this problem.
At constant volume the pressure of a given mass of gas varies directly with the absolute temperature.
P1 is the initial pressure
P2 is the final pressure
T1 is the initial temperature
T2 is the final temperature
convert from celcius to kelvin:
tK = 273 + tC
T1 = 273 + 22 = 295K
T2 = 273 + 45 = 318K
P2 = 119.7kPa
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Ideal gas brainly.com/question/13064292
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-- Free neutrons collide with Uranium nuclei.
If one is absorbed, then
-- the Uranium nucleus falls apart,
producing
-- smaller nuclei,
-- energy,
and
-- more free neutrons.
Answer:
Ionic Compound
Explanation:
To identify the type of chemical bond in a molecule, look at the atoms that make up the compound. If there are two nonmetals, it is a covalent bond. If the two atoms are metals, it is a metallic bond. If one atom is a metal and the other is a nonmetal, it is an ionic bond. Ionic compounds are also known as salts. You can identify KBr as an ionic compound because potassium is a metal and a salt.
Hope this helps
Since V is 5 times larger than C
A) 0V = 25C
25C to 0C = -25
-25 / 5 = -5
so 0C = -5 V
B)
20V x 5 = 100 C
Need more than that to answer this question
