temperature. 5. Use the Ideal Gas Law to calculate the number of moles (n) of carbon dioxide required to fill a 6 x 9-inch bag. Record the number of moles (n) in Data Table 1. n= PV RT %3D
temperature. 5. Use the Ideal Gas Law to calculate the number of moles (n) of carbon dioxide required to fill a 6 x 9-inch bag. Record the number of moles (n) in Data Table 1. n= PV RT %3D
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help with step #5 and #7-9.
Transcribed Image Text:Data Table 1: Model Air Bag
Activity
|Vol. of 6×9 in bag
Room Pressune in atm
Data & Observations
1.2 Liters
25.4mm x
1.00 atm-1.003 atm.
760mm
30.19inches*
1.00in.
Room temp.in Kelvin.
30°C + 273=303 K
1.00m.
Moles of COz nequired to
linflate bag at room temp.
and pressune
Balanced equation for the
reaction of NaHC03 &
CH3 COOH to produce CO2
Massot NaHcO3 needed
Hor the rraction (84.0glmal)
V6l.of vinegar requined
(0.833Maccticacid)
n=PV
RT
![to fill a resealable plastic bag with carbon
dioxide gas. The goal is to determine the exact
1. NaHCO,(s) + CH,COOH(aq) -
stoichiometric amounts of sodium bicarbonate
and acetic acid that will react to completely fill a
2. H,CO,(aq) + CH,COONA(aq) →
sealed bag without bursting it.
3. H,O(1) + CO,(g) + CH,COONa(aq)
1. The volume of each 6 x 9-inch resealable bag
7. In Data Table 1, write a balanced equation for
only the reactants and products in bold print
is 1.20 liters.
2. The current air pressure in inches of mercury
can be found on local weather reports or by
an internet search using the keywords, "air
pressure for XXXXX" (where XXXXX is the
local zip code).
shown above in lines 1 and 3. Line 1 are the
reactants and line 3 are the products.
8. Beginning with the moles of carbon dioxide
determined in step 5 and the balanced
chemical equation, calculate the grams of
sodium bicarbonate reactant [MW = 84.0 g/
3. Convert the air pressure from inches of
mercury to the nearest 0.01 atmospheres
using the following conversion (and record
in Data Table 1):
%3D
mol] needed to produce this number of moles
of carbon dioxide. Record your results in Data
Table 1.
inches
x 25.4 mm x 1.00 atm
1.00 inch
atm
84.0 g
grams = molHcOs
mol
CO2 x molar ratio HCO3: CO,
760. mm
4. Measure the room temperature in °C with a
thermometer. Convert to Kelvin by adding
stoichiometric coefficient HCO,
stoichiometric coefficient CO2
molar ratio HCO3: CO2 =
273, and record in Data Table 1 as Kelvin
9. The source of acetic acid is a solution
of vinegar, which is 0.833 M acetic acid.
Beginning with the number of moles of
carbon dioxide determined in step 5 and the
balanced chemical equation, calculate the
volume of vinegar solution required. Record
temperature.
5. Use the Ideal Gas Law to calculate the
number of moles (n) of carbon dioxide
required to fill a 6 x 9-inch bag. Record the
number of moles (n) in Data Table 1.
PV
n =
your results in Data Table 1.
RT
6. Examine the reaction of the weak base,
volume mL =
%3D
(molco, × molar ratio CH, COOH: CO2) × 1000 mL
sodium bicarbonate (NaHCO.), and the
weak acid found in vinegar, acetic acid
(CH,COOH). The products are the aqueous
0.833 mol
1 L
1L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffb555586-9f31-4c15-934a-3aec181a2382%2Faac6e77d-208d-4291-b89f-068982324797%2Ftfn9ge_processed.jpeg&w=3840&q=75)
Transcribed Image Text:to fill a resealable plastic bag with carbon
dioxide gas. The goal is to determine the exact
1. NaHCO,(s) + CH,COOH(aq) -
stoichiometric amounts of sodium bicarbonate
and acetic acid that will react to completely fill a
2. H,CO,(aq) + CH,COONA(aq) →
sealed bag without bursting it.
3. H,O(1) + CO,(g) + CH,COONa(aq)
1. The volume of each 6 x 9-inch resealable bag
7. In Data Table 1, write a balanced equation for
only the reactants and products in bold print
is 1.20 liters.
2. The current air pressure in inches of mercury
can be found on local weather reports or by
an internet search using the keywords, "air
pressure for XXXXX" (where XXXXX is the
local zip code).
shown above in lines 1 and 3. Line 1 are the
reactants and line 3 are the products.
8. Beginning with the moles of carbon dioxide
determined in step 5 and the balanced
chemical equation, calculate the grams of
sodium bicarbonate reactant [MW = 84.0 g/
3. Convert the air pressure from inches of
mercury to the nearest 0.01 atmospheres
using the following conversion (and record
in Data Table 1):
%3D
mol] needed to produce this number of moles
of carbon dioxide. Record your results in Data
Table 1.
inches
x 25.4 mm x 1.00 atm
1.00 inch
atm
84.0 g
grams = molHcOs
mol
CO2 x molar ratio HCO3: CO,
760. mm
4. Measure the room temperature in °C with a
thermometer. Convert to Kelvin by adding
stoichiometric coefficient HCO,
stoichiometric coefficient CO2
molar ratio HCO3: CO2 =
273, and record in Data Table 1 as Kelvin
9. The source of acetic acid is a solution
of vinegar, which is 0.833 M acetic acid.
Beginning with the number of moles of
carbon dioxide determined in step 5 and the
balanced chemical equation, calculate the
volume of vinegar solution required. Record
temperature.
5. Use the Ideal Gas Law to calculate the
number of moles (n) of carbon dioxide
required to fill a 6 x 9-inch bag. Record the
number of moles (n) in Data Table 1.
PV
n =
your results in Data Table 1.
RT
6. Examine the reaction of the weak base,
volume mL =
%3D
(molco, × molar ratio CH, COOH: CO2) × 1000 mL
sodium bicarbonate (NaHCO.), and the
weak acid found in vinegar, acetic acid
(CH,COOH). The products are the aqueous
0.833 mol
1 L
1L
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