Mass (before reaction): test tube + HCl(aq) + stir bar + capsule 26.600 g
Mass (after reaction): test tube + HCl(aq) + stir bar + capsule 25.300 g
Volume of water displaced from the squirt bottle 148 mL
Temperature of the CO2(g) 287.4 K
Pressure (atm) 1.032 atm
Using this data answer each of the questions below.
Calculate the mass of CO2(g).
Calculate the number of moles of CO2(g).
1.3/44.01+.029 This doesnt work
Calculate the density of CO2(g) in g/L.
Calculate the molar mass of CO2 assuming a temperature of 287.4 K.
1,30/148 doesnt work
Calculate the Gas constant, R, in L*atm/K*mol.
Why did the chemist refuse to calculate the mass of CO2?
Because it didn't want any more mass hysteria in the lab! *ba dum tss*
But let's crunch some numbers anyway!
To calculate the mass of CO2(g), we need to find the difference between the mass before and after the reaction:
Mass of CO2(g) = Mass (before reaction) - Mass (after reaction)
= 26.600 g - 25.300 g
= 1.300 g
So, the mass of CO2(g) is 1.300 grams.
Now, let's move on to calculating the number of moles of CO2(g).
To do this, we can use the formula:
Number of moles = Mass / Molar mass.
The molar mass of CO2 is approximately 44.01 g/mol.
Number of moles of CO2(g) = Mass of CO2(g) / Molar mass of CO2
= 1.300 g / 44.01 g/mol
≈ 0.0295 moles
Therefore, the number of moles of CO2(g) is approximately 0.0295 moles.
Next, let's calculate the density of CO2(g) in g/L.
Density = Mass / Volume.
Density of CO2(g) = Mass of CO2(g) / Volume of water displaced from the squirt bottle
= 1.300 g / 148 mL
= 0.0088 g/mL
But we want the density in g/L, so let's convert mL to L:
Density of CO2(g) = 0.0088 g/mL x (1 L / 1000 mL)
≈ 0.00088 g/L
Therefore, the density of CO2(g) is approximately 0.00088 g/L.
Moving on, let's find the molar mass of CO2 assuming a temperature of 287.4 K.
To do this, we can use the ideal gas equation:
PV = nRT,
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
We're given the pressure (1.032 atm), volume (148 mL converted to L), and temperature (287.4 K). Let's solve for the number of moles:
n = (PV) / (RT)
= ((1.032 atm) * (0.148 L)) / ((0.0821 L*atm/K*mol) * (287.4 K))
≈ 0.006 moles
Now, let's find the molar mass using the formula:
Molar mass = Mass / Number of moles
Molar mass of CO2 = Mass of CO2(g) / Number of moles
= 1.300 g / 0.006 moles
= 216.7 g/mol
Therefore, the molar mass of CO2 is approximately 216.7 g/mol.
Finally, let's calculate the Gas constant, R, in L*atm/K*mol.
We know the equation PV = nRT, and we can rearrange it to solve for the gas constant:
R = (PV) / (nT)
= (1.032 atm * 0.148 L) / (0.006 moles * 287.4 K)
≈ 0.062 L*atm/K*mol
So, the Gas constant, R, is approximately 0.062 L*atm/K*mol.
To answer each of the questions, we'll go step-by-step:
1. Calculate the mass of CO2(g):
Mass of CO2(g) = Mass (before reaction) - Mass (after reaction)
Mass of CO2(g) = 26.600 g - 25.300 g
Mass of CO2(g) = 1.300 g
2. Calculate the number of moles of CO2(g):
Number of moles of CO2(g) = Mass of CO2(g) / Molar mass of CO2
Number of moles of CO2(g) = 1.300 g / 44.01 g/mol
Number of moles of CO2(g) ≈ 0.0296 mol
3. Calculate the density of CO2(g) in g/L:
Density of CO2(g) = Mass of CO2(g) / Volume of water displaced
Density of CO2(g) = 1.300 g / 148 mL * conversion factor
Note: We need to convert mL to L by dividing by 1000 (since 1 L = 1000 mL).
Density of CO2(g) ≈ 8.78 g/L
4. Calculate the molar mass of CO2 assuming a temperature of 287.4 K:
Molar mass of CO2 = Mass of CO2(g) / Number of moles of CO2(g)
Molar mass of CO2 = 1.300 g / 0.0296 mol
Molar mass of CO2 ≈ 43.92 g/mol
5. Calculate the Gas constant, R, in L*atm/K*mol:
R = (Pressure * Volume) / (Number of moles * Temperature)
R = (1.032 atm * 0.148 L) / (0.0296 mol * 287.4 K)
R ≈ 0.717 L*atm/K*mol
Please note that rounding has been done for clarity.
To calculate the mass of CO2(g):
1. Start by finding the difference in mass before and after the reaction:
Mass (before reaction) - Mass (after reaction) = 26.600 g - 25.300 g = 1.300 g
2. This difference in mass corresponds to the mass of CO2(g).
Therefore, the mass of CO2(g) is 1.300 g.
To calculate the number of moles of CO2(g):
1. Use the molar mass of CO2, which is 44.01 g/mol.
Moles = Mass / Molar mass = 1.300 g / 44.01 g/mol ≈ 0.0296 mol
Therefore, the number of moles of CO2(g) is approximately 0.0296 mol.
To calculate the density of CO2(g) in g/L:
1. Density is defined as mass/volume.
Density = Mass / Volume = 1.300 g / 148 mL
2. Convert mL to L by dividing by 1000:
Density = 1.300 g / (148 mL / 1000) = 1.300 g / 0.148 L ≈ 8.7837 g/L
Therefore, the density of CO2(g) is approximately 8.7837 g/L.
To calculate the molar mass of CO2 assuming a temperature of 287.4 K:
1. Use the ideal gas law, PV = nRT, where:
P is pressure (in atm),
V is volume (in L),
n is the number of moles,
R is the gas constant,
and T is the temperature (in K).
2. Rearranging the equation gives: n = PV / RT.
n = (1.032 atm) * (0.148 L) / [(R) * (287.4 K)]
3. Simplify the equation to isolate the value of R.
R = PV / (n * T)
Therefore, to calculate the gas constant, R, you need the values of pressure (P), volume (V), number of moles (n), and temperature (T).