Question

show the title, formula, substitution, and solution for each calculation?

I don't know how to calculate the answers that are already prefill in the boxes.

Data Table A
Unknown Letter	W
Mass of empty flask with Foil (g)	93.58
Mass of flask, foil and condensed liquid (g)	94.17
Mass of condensed gas (g)	187.75
Temperature (C)	100
Temperature (K)	373.15
Pressure (mmHg)	748.2
Pressure (atm)	0.984
Volume of gas (mL)	148
Volume of gas (L)	0.148
Molar mass calculated (g/mol)	124.11

Answer 1

Data that is measured physically at the time of experiment   (these variables have to be measured physically by instruments)

mass of empty flask with foil = 93.58 g

mass of flask, foil and condensed liquid = 94.17 g

Temperature of gas = 100^oC

Pressure = 748.2 mmHg

Volume of gas = 148 mL

Data calculated

mass of condensed gas = (mass of flask, foil and condensed liquid) - (mass of empty flask with foil)

mass of condensed gas = (94.17 g) - (93.58 g)

mass of condensed gas = 0.59 g

pressure of gas (atm) = (pressure of gas in mmHg) * (1 atm / 760 mmHg)

pressure of gas (atm) = 748.2 mmHg * (1 atm / 760 mmHg)

pressure of gas (atm) = 0.984 atm

Volume of gas collected (L) = (volume of gas in mL) * (1 L / 1000 mL)

Volume of gas collected (L) = (148 mL) * (1 L / 1000 mL)

Volume of gas collected (L) = 0.148 L

Temperature of gas (K) = (temperature of gas in ^oC) + 273.15

Temperature of gas (K) = 100 + 273.15

Temperature of gas (K) = 373.15 K

moles of gas = [pressure of gas (atm) * (Volume of gas collected (L)] / [Temperature of gas (K) * R]

where R = gas constant = 0.0821 L-atm/mol-K

moles of gas = [(0.984 atm) * (0.148 L)] / [(373.15 K) * (0.0821 L-atm/mol-K)

moles of gas = 0.00476 mol

molar mass of gas = (mass of condensed gas) / (moles of gas)

molar mass of gas = (0.59 g) / (0.00476 mol)

molar mass of gas = 124.11 g/mol