Answer :
Final answer:
To calculate the amount of water vapor required to occupy a 1981 mL flask at 0.97 atm and 97.6 degrees Celsius, we can use the ideal gas law. The formula is PV = nRT, where P is the pressure in atm, V is the volume in liters, n is the number of moles of the gas, R is the ideal gas constant, and T is the temperature in Kelvin. By rearranging the formula and plugging in the given values, we can find the number of moles of water vapor and convert it to grams using the molar mass of water.
Explanation:
To calculate the amount of water vapor required to occupy the given flask, we can use the ideal gas law. The formula is:
PV = nRT
Here, P is the pressure in atm, V is the volume in liters, n is the number of moles of the gas, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the volume to liters: 1981 mL = 1.981 L. We also need to convert the temperature to Kelvin: 97.6°C + 273.15 = 370.75 K.
Next, let's rearrange the equation to solve for the number of moles of water vapor:
n = PV / RT
Plugging in the values:
n = (0.97 atm)(1.981 L) / [(0.0821 L·atm/mol·K)(370.75 K)]
Solving this equation gives us the value of n, which represents the number of moles of water vapor. To convert moles to grams, we can use the molar mass of water (18 g/mol).
Finally, we calculate the mass of water vapor:
Plugging in the calculated value of n, we can find the mass of water vapor required to occupy the flask.
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