What is the volume of a flask that contains 0.730 moles of Nitrogen at a pressure of 698 mmHg and a temperature of 35.4°C?

V = 20.1 L

Explanation:

Given data:

Volume of flask = ?

Number of moles of nitrogen gas = 0.730 mol

Pressure = 698 mmHg (698/760 = 0.92 atm)

Temperature = 35.4°C

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.

35.4+273 = 308.4 K

by putting values,

0.92 atm× V = 0.730 mol ×0.0821 atm.L/ mol.K × 308.4 K

V = 18.48 atm.L / 0.92 atm

V = 20.1 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