How much 6M HCl and NaHCO3 are required to make 1 quart of CO2?
Here is a worked example of a stoichiometry problem.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Convert 1 qt to L (I assume that is at STP)
Post your work if you get stuck.
To determine how much 6M HCl (hydrochloric acid) and NaHCO3 (sodium bicarbonate) are required to make 1 quart of CO2, we need to understand the chemical reaction that occurs between these two substances.
The reaction between HCl and NaHCO3 produces carbon dioxide (CO2), water (H2O), and sodium chloride (NaCl), and it can be represented by the following equation:
HCl + NaHCO3 -> CO2 + H2O + NaCl
To determine the amount of each reactant required, we need to consider the stoichiometry of the reaction. The stoichiometry is a way to relate the number of moles of reactants and products in a balanced chemical equation.
In this case, the stoichiometry tells us that for every one mole of NaHCO3, one mole of CO2 is produced. Therefore, we only need to know the amount of NaHCO3 required to produce 1 quart of CO2.
To calculate the amount of NaHCO3 needed, we need to convert the volume of CO2 (1 quart) to moles. We will use the ideal gas law to do this. The ideal gas law equation is as follows:
PV = nRT
Where:
P = Pressure of the gas
V = Volume of the gas
n = Number of moles of the gas
R = Ideal gas constant
T = Temperature in Kelvin
Since we know the volume of CO2 (1 quart), we need to convert it to a standard unit like liters. 1 quart is equal to approximately 0.946 liters.
Next, we need to determine the temperature and pressure conditions at which the reaction is taking place. For simplicity, let's assume standard temperature and pressure (STP), which is 0 degrees Celsius (273 Kelvin) and 1 atmosphere of pressure.
Now we can calculate the number of moles of CO2 using the ideal gas law equation. Rearranging the equation, we have:
n = PV / RT
Plugging in the values:
n = (1 atm) * (0.946 L) / (0.0821 atm L/mol K * 273 K)
Calculating the right side of the equation:
n = 0.041 moles of CO2
Since the stoichiometry tells us that one mole of NaHCO3 produces one mole of CO2, we need 0.041 moles of NaHCO3.
Finally, to calculate the amount of 6M HCl required, we need to consider the balanced chemical equation again. The stoichiometry tells us that for every one mole of NaHCO3, one mole of HCl is required. Therefore, we also need 0.041 moles of 6M HCl.
To convert moles to grams, you would need to know the molar mass of each substance involved in the reaction. In this case, the molar mass of NaHCO3 is approximately 84 grams/mol, while the molar mass of HCl is approximately 36.5 grams/mol. Therefore, you can multiply the number of moles by the molar mass to determine the mass required.
It's important to note that handling chemicals like HCl and NaHCO3 can be dangerous, and it is always advised to follow proper safety precautions and consult appropriate sources for accurate measurements and procedures. This explanation is for educational purposes only and should not be considered as a guide for conducting experiments.