Question 5
Determine the mass (in g) of oxygen (Mc = 32.00) that occupies a volume of 146.7 cm? at a pressure of
106.5 kPa and a temperature of 167 °C. Give the answer to 3 significant figures
9

0.128 g

Explanation:

Given data:

Volume of gas = 146.7 cm³

Pressure of gas = 106.5 Kpa

Temperature of gas = 167°C

Mass of oxygen gas = ?

Solution:

Volume of gas = 146.7 cm³ (146.7 /1000 = 0.1467 L)

Pressure of gas = 106.5 Kpa (106.5/101 = 1.1 atm)

Temperature of gas = 167°C (167 +273.15 = 440.15 K)

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

n = PV/RT

n = 1.1 atm× 0.1467 L / 0.0821 atm.L/ mol.K   × 440.15 K

n = 0.1614 / 36.14 /mol

n = 0.004 mol

Mass of oxygen:

Mass = number of moles × molar mass

Mass = 0.004 mol × 32 g/mol

Mass = 0.128 g

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.