Agas that exerts a pressure of 2.15 atm in a container with a volume of 0.0900 l will exert a pressure of atm when transferred to a container with a volume of a 4.75 l

Given:

Initial pressure exerted by the gas P1 = 2.15 atm

Initial volume of the container V1 = 0.0900 L

Final volume of the new container V2 = 4.75 L

To determine:

Pressure P2 exerted by the gas in the new container

Explanation:

The ideal gas equation is given as-

PV = nRT

where n = moles of the gas

R = gas constant and T = temperature

Since the values of n, R, T do not change when the gas is transferred to the new container, we have the relation

PV = constant

or, P1V1 = P2V2

P2 = P1V1/V2 = 2.15 * 0.0900/4.75 = 0.041 atm

Ans: The pressure exerted by the gas in the new container is 0.041 atm

the mass of the cathode increases because ions from the solution get reduced to atoms and become part of the cathode.

explanation:

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answer is: nuclear fusion produces elements that are heavier than helium.

nuclei combine to form a heavier nucleus, releasing energy.  

for example, fusion of hydrogen atoms at the sun.  

this fusion nuclear reaction is in the inner core of the sun and hydrogen (atomic number 1) is conveted into helium (atomic number 2).  

the inner core is the central region of the sun and all solar energy is produced in the core by nuclear fusion.