work. AIso exp 3. An empty 500. mL flask has a mass of 15.011 g. When the flask

Question

work. AIso exp 3. An empty 500. mL flask has a mass of 15.011 g. When the flask is filled with a gas to a pressure of 1.23 atm at 20°C, its mass increases to 16.101 g. Assume that the ideal gas law equation applies and calculate the approximate molar mass of the gas. Be sure to include dimensional analysis and consideration of significant figures in your work. Also explicitly show any algebraic steps you use. 4. Solid potassium carbonate reacts with aqueous hydrochloric acid to form aqueous potassium chloride, water, and gaseous carbon dioxide (equation shown below). A 0.550 g sample of potassium carbonate produced carbon dioxide gas that is collected using water displacement at 1.03 atm and 25°C. Assume the vapor pressure of water is 23.8 torr at 25°C. What is the volume in milliliters of carbon dioxide gas produced? Be sure to include dimensional analysis and consideration of significant figures in your work. Also explicitly show any algebraic steps you use K2co, (s) + 2 HCI (g) 2 KCI (aq) + H2O (l) + CO2 (g) n is nlaced in a 15.0 L vessel at

Explanation / Answer

3)

we have:

P = 1.23 atm

V = 500 mL

= (500/1000) L

= 0.500 L

T = 20 oC

= (20+273) K

= 293 K

find number of moles using:

P * V = n*R*T

1.23 atm * 0.5 L = n * 0.08206 atm.L/mol.K * 293 K

n = 2.60*10^-2 mol

mass = 16.101 - 15.011 = 1.090 g

we have below equation to be used:

number of mol = mass / molar mass

2.60*10^-2 mol = (1.090 g)/molar mass

molar mass = 42.6 g/mol

Answer: molar mass = 42.6 g/mol

Feel free to comment below if you have any doubts or if this answer do not work

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