Atmospheric pressure 728.0torr
temperature 25.8 oc
gas constant 0.08206 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?

1,57 x 10-3 mol de CO2

Explanation:

The general equation of ideal gases can be used to solve the problem. Previously, the units of the supplied data must be converted in order to use this equation.

1- Use conversion factor to keep all data in the same units:

Atmospheric pressure:

760.0 torr _____ 1 atm

728.0 torr _____ X = 0.9579 atm

Calculation:

Temperature:

T (K) = t (° C) + 273.15 = 25.8 ° C + 273.15 = 298, 95 K

Volume of gas obtained:

1000 mL CO2 _____ 1 L

40.16 mL CO2 _____ X = 0.04016 L

Calculation:

2- Now, using the general equation of ideal gases, you can clear and calculate the number of moles obtained from CO2 gas:

If: PxV = n x R x T

So:

Where:

• P: Gas pressure in atm

• V: Volume of gas in L

• N: Number of moles of gas

• R: Gas constant (L.atm / mol.K)

• T: Temperature in K

3- Placing the values and solving the equation, the result is obtained:

n = (0.9579 atm x 0.04016 L) / (0.08206 L.atm / mol.K x 298.95 K) = 0.0015681 mol of CO2

If the result becomes scientific notation, it is equal to 1, 57 x 10-3 mol

Therefore, 1.57 x 10-3 moles of CO2 were produced

electron microscopy and scanning tunneling microscopes gives us a greater understanding of atoms by being able to see the atom itself, and lets us see some atomic reactions.

explanation: