A solution of 62.4 g of a covalent compound in enough water to make 1.000 L of solution has an osmotic pressure of 0.305 atm at 25°C. Assume the covalent compound does not dissociate in the solution. Based on these data, what is the molar mass (in g/mol) of covalent? Round your answer to the nearest whole number and do not include units with your answer.

4.99 × 10³ g/mol

Explanation:

Step 1: Given  and required data

Step 2: Calculate the molarity (M) of the solution

The osmotic pressure is a colligative pressure. For a covalent compound, it can be calculated using the following expression.

π = M × R × T

M = π / R × T

M = 0.305 atm / (0.0821 atm.L/mol.K) × 298 K

M = 0.0125 M

Step 3: Calculate the moles of solute (n)

We will use the definition of molarity.

M = n / V

n = M × V

n = 0.0125 mol/L × 1.000 L = 0.0125 mol

Step 4: Calculate the molar mass of the compound

0.0125 moles of the compound weigh 62.4 g. The molar mass is:

62.4 g/0.0125 mol = 4.99 × 10³ g/mol

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

thats how its supposed to be