What will the pressure of a gas be that contains 4.00 moles at a temperature of 88˚C in a container with a volume of 5.00 Liters?

P = 23.78 atm

Explanation:

Given data:

Number of moles of gas = 4.00 mol

Temperature = 88°C

Volume of gas = 5 L

Pressure of gas = ?

Solution;

The given problem will be solve by using general gas equation,

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

Now we will convert the temperature.

88 + 273 = 362 K

P = nRT/V

P = 4 mol ×0.0821 atm.L/ mol.K  ×362 K /  5 L

P = 118.88 atm /5

P = 23.78 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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the answer would be b i believe