you have set up the apparatus for this experiment and collected the following data: Atmospheric pressure- 721.o torr
temperature-22.0c
Gas constant- 0.0821 L atm/mol K
you then ran the experiment using 0.3234 g of alka seltzer and generated a volume of CO2 of 40.16 ml
How many moles of CO2 were produced?
To determine the number of moles of CO2 produced, 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.
Given:
Atmospheric pressure (P) = 721.0 torr
Temperature (T) = 22.0 °C = 22.0 + 273.15 = 295.15 K
Gas constant (R) = 0.0821 L atm/mol K
Volume (V) of CO2 produced = 40.16 ml = 0.04016 L
Substituting the values into the ideal gas law equation, we get:
(721.0 torr) * (0.04016 L) = n * (0.0821 L atm/mol K) * (295.15 K)
Now, let's solve for n, the number of moles of CO2:
(721.0 torr * 0.04016 L) / (0.0821 L atm/mol K * 295.15 K) = n
Calculating this equation gives us the number of moles of CO2 produced.
Note: Torr is equivalent to mmHg, and atm is a widely used pressure unit, so we can keep the units consistent and cancel them out during the calculations.