A sample of the inhalation anesthetic gas Halothane, in a 500-mL cylinder has a pressure of 2.3 atm at 0°C. What will be the pressure of the gas if its temperature is warmed to 37°C (body temperature)? (Hint: Which law will you apply if the volume is constant?)

The pressure will increase to a pressure of 2.6 atm

Explanation:

Step 1: Data given

Volume = 500 mL = 0.500L

Pressure = 2.3 atm

Temperature = 0°C = 273 K

Temperature is warmed to 37 °C = 310 K

Volume will stay constant

Step 2: Calculate the new pressure

p1/T1 = p2/T2

⇒with p1 = the initial pressure = 2.3 atm

⇒with T1 = the initial temperature = 0 °C = 273 K

⇒with p2 = the new pressure = TO BE DETERMINED

⇒with T2 = the new temperature = 37 °C = 310 K

2.3 atm / 273 K  = p2 / 310 K

p2 = 2.6 atm

The pressure will increase to a pressure of 2.6 atm

it means there are 3 atoms of oxygen

the positions which points up in upward carbon and down in downward carbon are axial

and vice versa holds true for equatorial positions

so the correct answer with labelled diagram will be