5.36 litars of nitrogen gas are at :25°C and 733 mm Hg
What would be the volume at 129 86 and 1.5 atm

4.6L

Explanation:

Use the equation (P1*V1)/(T1)=(P2*V2)/(T2)

P= pressure

V= volume

T= temperature in kelvins (remember K= C + 273)

Convert atm to mmHg or vise versa

1.5atm*(760mmhg/1atm)= 1140mmHg

(733mmHg * 5.36L)/(298K)=(1140mmHg * V)/(402K)

V= 4.6 or 4.65L (depending on sig figs)

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.