Optimistic Chemistry Problem Solving

a. What was the pressure of the vapor in the flask in atm?

Choose one of the following:

a) 0.957895 atm

b. What was the temperature of the vapor in K? The volume of the flask in liters?

Choose one of the following:

b) 372.05 K

c. What was the mass of condensed vapor that was present in the flask?

Choose one of the following:

c) 0.524 grams

d. How many moles of condensed vapor were present?

Choose one of the following:

d) 0.00725 moles

e. What is the mass of one mole of vapor?

Choose one of the following:

e) Molar mass gas = 30.54 g/mol

Answer:

a) 0.957895 atm

b) 372.05 K

c) 0.524 grams

d) 0.00725 moles

e) Molar mass gas = 30.54 g/mol

Let's break down the chemistry problem and solve it step by step with an optimistic mindset:

Step 1: Data Given

Mass of the flask = 53.256 grams

Volume = 5 mL

Temperature of water = 98.9 °C = 372.05 K

Mass obtained = 53.78 grams

The volume of the flask is known to be 231.1 mL = 0.2311 L

The absolute atmospheric pressure in the laboratory that day is 728 mm Hg

Step 2: Calculate the mass of the gas

Mass gas = 53.780 - 53.256 = 0.524 grams

Step 3: Calculate moles

p*V = n*R*T

with p = the pressure = 0.957895 atm

with V = the volume = 0.2311 L

with n = the number of moles gas = TO BE DETERMINED

with R = the gas constant = 0.08206 L*atm/mol * K

with T = the temperature = 372.05 K

n = (p*V)/(R*T)

n = (0.957895 * 0.2311) / (0.08206 * 372.05) = 0.00725 moles

Step 4: Calculate mass of the gas

Molar mass = mass / moles

Molar mass gas = 0.524 grams / 0.00725 moles = 30.54 g/mol

With a positive attitude and careful calculations, we have successfully solved the chemistry problem and found the answers we were looking for!