Question

What pressure is required to achieve a co2 concentration of 5.80×10−2 m at 20∘c?

Answer 1

To achieve a CO2 concentration of 5.80×10−2 M at 20∘C, a pressure of approximately 1.71 atm is required.

Step-by-step explanation:

To calculate the pressure required to achieve a CO2 concentration of 5.80×10−2 M at 20∘C, we can use Henry's law. Henry's law states that the concentration of a gas dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid.

The formula to calculate the pressure is given by:

P = (C / k)

Where P is the pressure, C is the concentration, and k is the Henry's law constant.

Plugging in the values, we get:

P = (5.80×10−2 M) / (3.4 × 10−2 M/atm) = 1.71 atm

Therefore, a pressure of approximately 1.71 atm is required to achieve a CO2 concentration of 5.80×10−2 M at 20∘C.

Answer 2

The concentration (c) of a gas at pressure (p) at a given temperature (T) through the Henry's constant kH

c = kH * p

at 20 C or 293 K, the henry's constant kH for CO2 = 0.037 mol/L-atm

Given concentration c = 0.0580 moles/L

Hence the pressure is given as:

p = c/kH = 0.0580 molesL-1/0.037 molL-1atm-1 = 1.57 atm

Pressure required is 1.57 atm