The volume of a sample of hydrogen gas was decreased from 14.65 l to 7.94 l at constant temperature. if the final pressure exerted by the hydrogen gas sample was 5.02 atm, what pressure did the hydrogen gas exert before its volume was decreased?

The pressure the hydrogen gas exerted before its volume was decreased is 2.7207 atm.

Explanation:

Using Boyle's law

Given ,  

V₁ = 14.65 L

V₂ = 7.94 L

P₁ = ?

P₂ = 5.02 atm

Using above equation as:

The pressure the hydrogen gas exerted before its volume was decreased is 2.7207 atm.

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

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