Question

The henry's law constant (k) for carbon monoxide in water at 25°c is 3.10× 10-2 mol/(l·atm). how many grams of co will dissolve in 1.00 l of water if the partial pressure of co2is 2.75 atm?

Answer 1

`3.75\text{ g}`

Step-by-step explanation:

Here, we want to calculate the mass that would dissolve

Mathematically:

`\begin{gathered} mass\text{ = number of moles }*\text{ molar mass} \\ \end{gathered}`

The molar mass of carbon (iv) oxide is 44 g/mol

Thus, we have the number of moles as:

`number\text{ of moles = }(mass)/(44)`

According to Henry's law:

`C\text{ = KP}`

Where;

C is the concentration of dissolved gas

K is the Henry's constant

P is the pressure

Now, from the question, we have:

k = 3.2 * 10^-2

P = 2.75

C is the number of moles per liter which we will represent by the number of moles

Thus, we have it that:

`\begin{gathered} (mass)/(44)\text{ = 3.10 }*\text{ 10}^(-2)\text{ }*2.75 \\ \\ mass\text{ = 3.75 g} \end{gathered}`