Hey, I need help finding out how many moles of CO2 is produced from this reaction. Any help is appreciated, thanks.
Mass of empty Erlenmeyer flask (g): 88.000 g
Mass of Erlenmeyer flask and 20 mL H2SO4: 112.198 g
Mass of 20 mL H2SO4: 24.198 g
Trial I
Mass of Na2CO3 added to flask (g): 1 g
Moles of Na2CO3 added to flask (FW=105.989): 0.00641 mol
Calculate initial mass of reactants (H2SO4 and Na2CO3 in flask (g)
Add your answers from 1b and Trial I a : 113.198 g
Final mass of flask and contents after reaction as recorded on balance (g): 112.783 g
Mass of CO2 (initial mass minus final mass [c – d]) (g): 0.415 g
Moles of CO2 produced in the reaction (MW = 44.010): ??
To find the moles of CO2 produced in the reaction, we need to calculate the mass of CO2 produced and then convert it to moles using the molar mass of CO2.
Given:
- Initial mass of reactants (H2SO4 and Na2CO3 in flask) = 113.198 g
- Final mass of flask and contents after reaction = 112.783 g
- Mass of CO2 (initial mass minus final mass) = 0.415 g
- Molar mass of CO2 (MW) = 44.010 g/mol
To find the moles of CO2 produced:
1. Calculate the mass of CO2 produced:
Mass of CO2 = Initial mass - Final mass
Mass of CO2 = 113.198 g - 112.783 g
Mass of CO2 = 0.415 g
2. Convert the mass of CO2 to moles:
Moles of CO2 = Mass of CO2 / Molar mass of CO2
Moles of CO2 = 0.415 g / 44.010 g/mol
Moles of CO2 = 0.00943 mol
Therefore, the moles of CO2 produced in the reaction is approximately 0.00943 mol.
To find the number of moles of CO2 produced in the reaction, we can use the mass of CO2 (0.415 g) and the molar mass of CO2 (44.010 g/mol).
First, let's calculate the moles of CO2:
Moles of CO2 = Mass of CO2 / Molar mass of CO2
Moles of CO2 = 0.415 g / 44.010 g/mol
Moles of CO2 = 0.00943 mol
Therefore, the number of moles of CO2 produced in the reaction is 0.00943 mol.