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

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

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