Ireally need with question one and two. i don’t remember how to do it and my notes aren’t making matters better

0.449 mole

We are given;

Volume of oxygen gas,V = 75.0 mL or 0.075 L

Pressure, P = 145 atm

Temperature, T = 22° C or 22 + 273 = 295 K

We are required to calculate the moles of Oxygen gas

We are going to use the ideal gas equation which states;

PV =nRT where, P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant,(0.082057 L atm/mol.K) and T is the temperature.

Therefore, to get n we use;

Therefore; the number of moles of Oxygen gas is 0.449 mole

35,410.99 torr

We are given

Initial Pressure of the gas, P1 = 30,400 torr

Initial temperature, T1 = 0°C or 273 K

Final temperature, T2 = 45°C or 318 K

We are required to find the final pressure, P1,

Therefore,

At varying temperature and pressure;

Thus;

Therefore; the new pressure in the container is 35,410.99 torr

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.  

its going to be mutualism cuz they both benefit from the relationship.

~batmans wife dun dun