Answer:
6.14×10²³ molecules
Step-by-step explanation:
Data obtained from the question include:
Volume (V) = 10.5L
Temperature (T) = 40°C
Pressure (P) = 252 kPa
Next, we shall determine the number of mole of CO2 present.
This can be obtained by using the ideal gas equation:
PV = nRT
Volume (V) = 10.5L
Temperature (T) = 40°C = 40°C + 273 = 313K
Pressure (P) = 252 kPa
Gas constant (R) = 8.31 KPa.L/Kmol
Number of mole (n) =.?
PV = nRT
252 x 10.5 = n x 8.31 x 313
Divide both side by 8.31 x 313
n = (252 x 10.5) /(8.31 x 313)
n = 1.02 mole
Therefore, 1.02 mol of CO2 is present.
Now, we can obtain the number of molecules of CO2 present as follow:
From Avogadro's hypothesis, 1 mole of any substance contains 6.02×10²³ molecules.
This means that 1 mole of CO2 also contains 6.02×10²³ molecules.
Now, if 1 mole of CO2 contains 6.02×10²³ molecules,
Then 1.02 mole will contain = 1.02 x 6.02×10²³ = 6.14×10²³ molecules.
Therefore, 6.14×10²³ molecules of CO2 is present.