An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 30.0 atm and releases 74.4 kj of heat. before the reaction, the volume of the system was 7.20 l . after the reaction, the volume of the system was 2.00 l . calculate the total internal energy change, δe, in kilojoules. express your answer with the appropriate units.

The total change in internal energy would simply be calculated using the formula:

ΔU = -P (V2 – V1) + ΔH

where ΔU is the change in internal energy; P is constant pressure = 30 atm = 3,039,750 Pa; V2 is final volume = 2 L = 0.002 m^3; V1 is initial volume = 7.20 L = 0.0072 m^3; while ΔH is the heat = -74,400 J (heat released so negative)

Therefore:

ΔU =-3,039,750 Pa * (0.002 m^3 - 0.0072 m^3) + (- 74,400 J)

ΔU = - 58,593.3 J = - 58.6 kJ

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.

answer: your mm

explanation: