A sample of an ideal gas at 1.00 atm and a volume of 1.98 L was placed in a weighted balloon and dropped into the ocean. As the sample descended, the water pressure compressed the balloon and reduced its volume. When the pressure had increased to 55.0 atm, what was the volume of the sample? Assume that the temperature was held constant.

Final Volume = 0.036 L

Explanation:

Initial Pressure P1 = 1 atm

Initial Volume V1 = 1.98L

Final Pressure T1 = 55.0 atm

Final Volume V2 = ?

Temperature was held constant

The formulae relating these variables is Charles Law. This law states that the volume of a gas is inversely proportional to the pressure of a gas system provided temperature is held constant. The equations given as;

V1P1 = V2P2

V2 = V1P1 / P2

V2 = 1.98 * 1 /  55

V2 = 0.036 L

the dissociation of nickel hydroxide is follows:

the concentration of hydroxide ion is

the equilibrium constant value of nickel hydroxide is = 6.1 * 10^-^1^6 and thus equilibrium equation can be written as:

thus, concentration of ni is 0.23 * 10^-^4 mol /l