How many molecules would there be in 10.5 L of carbon dioxide at 40.0 C and 252 kPa

6.14×10²³ molecules

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.

the answer would be a

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.