At the Henry's Law constant for carbon dioxide gas in water is . Calculate the mass in grams of gas that can be dissolved in of water at and a partial pressure of . Round your answer to significant digits.

The question is incomplete, here is the complete question:

At 25°C Henry's Law constant for carbon dioxide gas in water is 0.031 M/atm . Calculate the mass in grams of gas that can be dissolved in 425. mL of water at 25°C and at a partial pressure of 2.92 atm. Round your answer to 2 significant digits.

The mass of carbon dioxide that can be dissolved is 1.7 grams

Explanation:

To calculate the molar solubility, we use the equation given by Henry's law, which is:

where,

= Henry's constant =

= molar solubility of carbon dioxide gas

= partial pressure of carbon dioxide gas = 2.92 atm

Putting values in above equation, we get:

To calculate the mass of solute, we use the equation used to calculate the molarity of solution:

Given mass of carbon dioxide = ? g

Molar mass of carbon dioxide = 44 g/mol

Molarity of solution =

Volume of solution = 425 mL

Putting values in above equation, we get:

Hence, the mass of carbon dioxide that can be dissolved is 1.7 grams

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

c, liquids evaporate, creating a gas