At 983 torr of pressure, 1.62 grams of a gas dissolves in 2.0L of water at 10'C. What mass of gas will dissolved in 2.0L of water at 1432 torr and 10'C

To determine the mass of gas dissolved in 2.0L of water at 1432 torr and 10°C, we can use the concept of Henry's Law.

Henry's Law states that the solubility of a gas in a liquid at a given temperature is directly proportional to the partial pressure of the gas above the liquid.

The equation for Henry's Law is:

C = k * P

where:
C is the concentration of the dissolved gas in the liquid (in this case, in grams per liter - g/L),
k is the Henry's Law constant for the specific gas at the given temperature, and
P is the partial pressure of the gas (in this case, in torr).

Given that 1.62 grams of the gas dissolved in 2.0L of water at a pressure of 983 torr, we can first calculate the Henry's Law constant (k) for this gas at 10°C.

Now, we have two sets of data:
- 1.62 grams in 2.0L of water at 983 torr
- Unknown mass in 2.0L of water at 1432 torr

The first step is to calculate the Henry's Law constant (k) for the gas at 10°C using the given data.

k = C / P

Plugging in the values:
k = 1.62 g / (2.0 L * 983 torr)

Calculate the value of k using these numbers, and then substitute it into the equation to find the mass of gas dissolved at 1432 torr.

mass = C * (1432 torr / k)

Plugging in the values:
mass = C * (1432 torr / k) * 2.0 L

By substituting the values, you can calculate the mass of gas dissolved in 2.0L of water at 1432 torr and 10°C.