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Trial |
Barometric Pressure (atm) |
Temperature (°C) |
Mass of Chemical (g) |
Water Displaced (mL) |
---|---|---|---|---|
Trial 1 NaHCO_{3} |
1.006973 |
20C |
1.0g |
.057L |
Trial 2 NaHCO_{3} |
1.006973 |
20C |
1.0g |
.085L |
Trial 3 Na_{2}CO_{3} |
1.006973 |
21C |
1.0g |
.042L |
Trial 4 Na_{2}CO_{3} |
1.006973 |
20C |
1.1g |
.036L |
PART A Show your calculation for the molar volume of CO2 from Trial 1 according to your experimental data. Show all work, values, and units in your calculations in order to receive full credit. Your work must be complete, logical, and presented in the correct sequence of operations
PART B Show your calculation for the molar volume of CO2 from Trial 2 according to your experimental data. Show all work, values, and units in your calculations in order to receive full credit. Your work must be complete, logical, and presented in the correct sequence of operations
PART C Show your calculation for the molar volume of CO2 from Trial 3 according to your experimental data. Show all work, values, and units in your calculations in order to receive full credit. Your work must be complete, logical, and presented in the correct sequence of operations.
PART D Show your calculation for the molar volume of CO2 from Trial 4 according to your experimental data. Show all work, values, and units in your calculations in order to receive full credit. Your work must be complete, logical, and presented in the correct sequence of operations.
PART E What is the average experimental molar volume of the gas of all 4 trials? Show all work, values, and units in your calculations in order to receive full credit. Your work must be complete, logical, and presented in the correct sequence of operations.
PART F What is the percent error in your calculation? Show all work, values, and units in your calculations in order to receive full credit. Your work must be complete, logical, and presented in the correct sequence of operations
Trial |
Barometric Pressure (atm) |
Temperature (°C) |
Temperature (K) |
Mass of Chemical (g) |
Water Displaced (mL) |
---|---|---|---|---|---|
Trial 1 NaHCO_{3} |
1.006973 |
20 |
20 + 273 = 293 |
1.0 |
57 |
Trial 2 NaHCO3 |
1.006973 |
20 |
293 |
1.0 |
85 |
Trial 3 Na2CO3 |
1.006973 |
21 |
21 + 273 = 294 |
1.0 |
42 |
Trial 4 Na2CO3 |
1.006973 |
20 |
293 |
1.1 |
36 |
A. The no. of moles of NaHCO3 = 1 g / 84 g mol^{-1} = 0.012 mol
NaHCO3 + H2O NaOH + H2O + CO2
1 mole of NaHCO3 produces 1 mole of CO2
According to the ideal gas equation, PV = nRT
i.e. V = nRT/P
= 0.012 mol * 0.0821 L atm mol^{-1} K^{-1} * 293 K / 1.006973 atm
= 0.284 L
Therefore, the molar volume of CO2 = 0.284 L / 0.012 mol = 23.7 L/mol
Similarly, you can determine the molar volume in the remaining trails.
All the best!!!
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