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Explain Bot 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.