An ideal gas is held in a rigid container at temperature of 201∘C. Upon cooling the gas, the pressure decreases by a factor of 2.0, while the volume and the amount of gas remain constant. What must be the final temperature of the gas?

237 K

Explanation:

Given that,

Initial temperature, T₁ = 201⁰C = 474 K

Let P be the initial pressure. Upon cooling the gas, the pressure decreases by a factor of 2.0, while the volume and the amount of gas remain constant.

Final pressure = P/2

The relation between the pressure and temperature is as follows :

Put all the known values,

So, the final temperature of the gas is equal to 237 K.

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g