1) Calculate the mass of NaHCO3 required to generate 50mL of CO2, at 1 atm. pressure and 25*C.
Do I need to use PV=nRT?
where for n it will be both my n's from C and O2 together?
2) Solubility of CO2 in water at 25* is 0.145g in 100mL. Assuming the solubility of CO2 is the same in the acetic acid solution as in water, how much CO2 (in mL) might be dissolved in the 5,0mL used for each reaction?
Here do I simply do (0.145g / 100mL)x5.0 mL?
1. First, balance the equation. Yes, use PV = nRT to solve for moles CO2, the convert mols CO2 to mols NaHCO3, and from there to grams NaHCO3.
2. I think you're on the money for #2.
thank you Bob!
1) To calculate the mass of NaHCO3 required to generate 50 mL of CO2 at 1 atm and 25°C, you can indeed use the ideal gas law equation, PV = nRT. However, in this case, you need to consider the reaction stoichiometry between NaHCO3 and CO2.
The balanced chemical equation for the reaction is:
2NaHCO3(s) -> Na2CO3(s) + CO2(g) + H2O(g)
From this equation, we can see that for every 2 moles of NaHCO3, 1 mole of CO2 is produced. Therefore, you need to determine the number of moles of CO2 and convert it to mass using the molar mass of CO2.
1 mole of any gas occupies a volume of 22.4 liters or 22.4 x 1000 mL at standard temperature and pressure (STP). According to the ideal gas law, PV = nRT, you can rearrange it to solve for n (number of moles):
n = PV / RT
To calculate the number of moles of CO2, substitute the given values:
P = 1 atm
V = 50 mL = 50/1000 L
R = 0.0821 L atm/mol K (ideal gas constant)
T = 25°C + 273.15 = 298.15 K (convert to Kelvin)
n = (1 atm) x (50/1000 L) / (0.0821 L atm/mol K x 298.15 K)
Now, since you mentioned using "n" from both carbon (C) and oxygen (O2) together, it seems you might be confused. The correct interpretation is that you need to find the number of moles of CO2 rather than considering individual elements.
After obtaining the moles of CO2, you can convert it to grams using the molar mass of CO2 (44.01 g/mol) since the question asks for the mass of NaHCO3 required.
2) To determine how much CO2 (in mL) might be dissolved in the 5.0 mL acetic acid solution, you cannot simply use the equation (0.145 g / 100 mL) x 5.0 mL because the solubility of CO2 is given in grams per 100 mL of water, and the question asks for the amount of CO2 dissolved in acetic acid solution.
However, since the solubility of CO2 in acetic acid is assumed to be the same as in water, you can use the ratio of solubilities to calculate the amount of CO2.
First, find the solubility of CO2 in the acetic acid solution:
Solubility of CO2 in the acetic acid solution = (Solubility of CO2 in water) x (Volume of acetic acid solution / Volume of water)
Using the given values:
Solubility of CO2 in water = 0.145 g/100 mL
Volume of acetic acid solution = 5.0 mL
Volume of water = 100 mL
Now, substitute these values into the equation:
Solubility of CO2 in the acetic acid solution = (0.145 g/100 mL) x (5.0 mL / 100 mL)
Calculate the result to find the solubility of CO2 in the acetic acid solution. Note that the solubility is in grams per mL.
Please note that the actual amount of CO2 dissolved in the acetic acid solution may depend on various other factors, such as temperature, pressure, and the nature of the solution.