At 25 °c and 775 torr, carbon dioxide has a solubility of 0.0347 m in water. what is its solubility at 25 °c and 1470 torr?

Answer : The solubility at is, 0.0658 M

Explanation :

According to the Henry's Law, the solubility of a gas in a liquid is directly proportional to the pressure of the gas.

or,

where,

= initial solubility of carbon dioxide gas = 0.0347 M

= final solubility of carbon dioxide gas = ?

= initial pressure of carbon dioxide gas = 775 torr

= final pressure of carbon dioxide gas = 1470 torr

Now put all the given values in the above formula, we get the final solubility of the carbon dioxide gas.

Therefore, the solubility at is, 0.0658 M

part 1: the half-life of the element is 22 years.

part 2: it will take 132.02 year for the sample to decay from 308.0 g to 4.8125 g.

explanation:

part 1: there are two ways to determine the half life time.

first way: the half life time can be determined directly from its definition as it is the time required for the sample to decay to its half concentration.

from the data the initial concentration was 45.0 g and decayed to its half value (22.5 g) in 22.0 years.

second way: the radio active decay is considered first order reaction so we can use the laws of first order reactions.

k = (1/t) ln (a/a-x), where k is the rate constant of the reaction,

t is the time of the reaction

a is the initial concentration of the reactant

a-x is the remaining concentration at time (t)

a = 45.0 g the initial concentration at t = 0 year.

at t = 22 year, a-x = 22.5 g

then k = (1/22 year) ln (45.0 g/ 22.5 g) = 0.0315 year-1.

the half-life time (t1/2) = ln 2/ k = 0.693/ k =0.693/ 0.0315 = 22 years.

part 2:

using the same law k = (1/t) ln (a/a-x),

using the given data; a = 308.0 g and a-x = 4.8125 g and the calculated k from the part 1 (k = 0.0315 year-1)

t = (1/k) ln (a/a-x) = (1/0.0315) ln (308.0/ 4.8125) = 132.02 years

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noun

the practice of taking someone else's work or ideas and passing them off as one's own.

explanation: