Part a an unopened can of soda has an aqueous co2 concentration of 0.21 m at 25.0 °c. what is the partial pressure of the gas in the can in torr? the henry's law constant for co2 at 25 °c is 3.4 × 10−2 mol/l-atm.

Partial pressure = 4689 torr

Explanation:

Given:

Concentration of CO2, c = 0.21 M= 0.21 mol/L

Henry's constant, k for CO2 = 3.4*10^-2 mol/L-atm

To determine:

the partial pressure, P

Calculation:

As per Henry's law, the concentration c of a gas is related to the pressure, p as follows:

Conversion from atm to torr

1 atm = 760 torr

answer: -

reaction:

na + cl ⇌ nacl

balanced chemical equation:

na + 2cl ⇌ nacl2

sodium + clorine goes to form sodium chloride (table salt).

the product is nacl2.

and the reactants are na and cl.

(note: if you don’t know what ⇌ means, read below: -

⇌(double head arrow) means reversible reaction).