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. Enter your answer to three significant figures and enter only the numerical value in the answer box.
Calculate the mass of CO2(g).
Calculate the number of moles of CO2(g).
Calculate the density of CO2(g) in g/L.
Calculate the molar mass of CO2 assuming a temperature of 287.4 K.
Calculate the Gas constant, R, in L*atm/K*mol.
Calculate the % error of the value of the Gas constant, R.
Calculate the mass of CO2(g).
I don't know your set up and you didn't explain but it appears mass CO2 is 26.600-25.300 = ?
Calculate the number of moles of CO2(g).
mols = grams/molar mass
Calculate the density of CO2(g) in g/L.
At what temperature? 287.4 K. You have grams and you ave volume.
Calculate the molar mass of CO2 assuming a temperature of 287.4 K.
mols = grams/molar mass. You have mols and grams.
Calculate the Gas constant, R, in L*atm/K*mol.
PV = nRT. Substitute and solve for R.
Calculate the % error of the value of the Gas constant, R.
[(exp value-accepted value)/(accepted value]*100 = ?
Calculate the number of moles of CO2
1.3/44.01+.029 This doesnt work
I'm sorry, I don't have the necessary information to answer those questions. But hey, did you hear about the mathematician who's afraid of negative numbers? He'll stop at nothing to avoid them!
To calculate the mass of CO2(g), we need to find the difference in 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
The mass of CO2(g) is 1.300 g.
To calculate the number of moles of CO2(g), we can use the ideal gas law 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.
Rearranging the equation to solve for n, we get:
n = PV / RT
n = (1.032 atm * 148 mL) / (0.0821 L*atm/K*mol * 287.4 K)
n = (1.032 * 0.148) / (0.0821 * 287.4)
n = 0.1516 / 23.64
n ≈ 0.0064 mol
The number of moles of CO2(g) is approximately 0.0064 mol.
To calculate the density of CO2(g) in g/L, we can use the formula:
Density = Mass / Volume
Density = 1.300 g / (148 mL/1000)
Density = 1.300 g / 0.148 L
Density ≈ 8.7847 g/L
The density of CO2(g) is approximately 8.7847 g/L.
The molar mass of CO2 can be calculated using the formula:
Molar mass = Mass / Moles
Molar mass = 1.300 g / 0.0064 mol
Molar mass ≈ 203.125 g/mol
The molar mass of CO2 is approximately 203.125 g/mol.
The Gas constant, R, can be calculated using the formula:
R = PV / nT
R = (1.032 atm * 148 mL) / (0.0064 mol * 287.4 K)
R = (1.032 * 0.148) / (0.0064 * 287.4)
R ≈ 0.1333 / 1.8359
R ≈ 0.0727 L*atm/K*mol
The Gas constant, R, is approximately 0.0727 L*atm/K*mol.
To calculate the % error of the value of the Gas constant, R, we can use the formula:
% error = | (Theoretical Value - Experimental Value) / Theoretical Value | * 100
The theoretical value of the Gas constant is 0.0821.
% error = | (0.0821 - 0.0727) / 0.0821 | * 100
% error = | 0.0094 / 0.0821 | * 100
% error = 0.1143 * 100
% error ≈ 11.43%
The % error of the value of the Gas constant, R, is approximately 11.43%.
To answer each of the questions, we need to use the given data and apply the appropriate formulas and conversions. Let's go step by step:
1. Calculate the mass of CO2(g):
- We have the mass before reaction (26.600 g) and the mass after reaction (25.300 g).
- The mass of CO2(g) produced can be found by subtracting the mass after reaction from the mass before reaction:
Mass of CO2(g) = Mass before reaction - Mass after reaction
Mass of CO2(g) = 26.600 g - 25.300 g.
2. Calculate the number of moles of CO2(g):
- The number of moles can be found using the molar mass of CO2(g).
- The molar mass of CO2 is 44.01 g/mol.
- To calculate the number of moles, divide the mass of CO2(g) (from the previous step) by the molar mass:
Number of moles = Mass of CO2(g) / Molar mass of CO2.
3. Calculate the density of CO2(g) in g/L:
- The density of a gas can be calculated using the ideal gas law: PV = nRT.
- We have the pressure (1.032 atm), the temperature (287.4 K), and the number of moles (from the previous step).
- Rearranging the ideal gas law equation, we get: Density = (n * Molar mass) / (R * Temperature).
- Plug in the values to calculate the density.
4. Calculate the molar mass of CO2 assuming a temperature of 287.4 K:
- We have the density of CO2(g), the pressure, and the temperature.
- Rearranging the equation from step 3, we get: Molar mass = (Density * R * Temperature) / Pressure.
- Plug in the values to calculate the molar mass.
5. Calculate the Gas constant, R, in L*atm/K*mol:
- The gas constant can be determined by rearranging the ideal gas law equation: R = (PV) / (nT).
- Plug in the values to calculate the gas constant.
6. Calculate the % error of the value of the Gas constant, R:
- To calculate the percent error, you need two values - the known or accepted value and the calculated value.
- However, the given data does not provide a known or accepted value for the gas constant. Without this value, we cannot calculate the percent error.
By following these steps, you should be able to calculate the answers to the questions using the given data.