Nitrogen gas is introduced into a large deflated plastic bag. no gas is allowed to escape, but as more and more nitrogen is added, the bag inflates to accommodate it. the pressure of the gas within the bag remains at 1 \rm atm and its temperature remains at room temperature (20.0^\ c. how many moles n have been introduced into the bag by the time its volume reaches 22.4 \rm l?

The ideal gas law states PV = nRT. This can be rearranged to:

n = PV / RT

Pressure = 1 atm

Volume = 1 L

T = 293 K

R = 0.0821 atm L / mol K

n = PV / RT = 0.0416 mol nitrogen

for points guys

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.