Calculate the pressure of the CO₂ (g) in the container at 425 K.

The pressure of the CO₂ = 0.995 atm

The complete question

A student is doing experiments with CO2(g). Originally, a sample of gas is in a rigid container at 299K and 0.70 atm. The student increases the temperature of the CO2(g) in the container to 425K.

Calculate the pressure of the CO₂ (g) in the container at 425 K.

Gay Lussac's Law

When the volume is not changed, the gas pressure is proportional to its absolute temperature

P₁=0.7 atm

T₁=299 K

T₂=425 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

it's c. elements are placed in rows based on how may valencies electrons have.