A sample of chlorine gas has a pressure of 7.25 kPa at 20.0°C. What will its pressure be at 60.0°C if its volume remains constant?

A. 2.42 kPa

B. 8.24 kPa

C. 21.8 kPa

D. 6.38 kPa

The new pressure is 8.24 kPa (answer B is correct)

Explanation:

Step 1: Data given

Pressure of a sample chlorine gas = 7.25 kPa = 0.07155194 atm

Temperature = 20.0 °C = 293 K

The temperature increase to 60 °C = 333 K

The volume stays constant

Step 2: Calculate the new pressure

P1/T1 = P2/T2

⇒with P1 = the initial Pressure of a sample chlorine gas = 7.25 kPa = 0.07155194 atm

⇒with T1 = the initial temperature = 20.0 °C = 293 K

⇒with P2 = the new pressure = TO BE DETERMINED

⇒with T2 = the increased temperature = 60.0 °C = 333 K

0.07155194 atm / 293 K = P2 / 333 K

P2 = 0.08132 atm = 8.24 kPa

7.25 Kpa / 293 K = P2 / 333 K

P2 = 8.24 kPa

The new pressure is 8.24 kPa (answer B is correct)

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