A weather balloon is inflated to a volume of 26.7 L at a pressure of 748 mmHg and a temperature of 28.4 °C. The balloon rises in the atmosphere to an altitude where the pressure is
400. mmHg and the temperature is -15.6 °C.

Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

42.64 L

Explanation:

Using the combined law equation as follows:

P1V1/T1 = P2V2/T2

Where;

P1 = initial pressure (mmHg)

P2 = final pressure (mmHg)

V1 = initial volume (L)

V2 = final volume (L)

T1 = initial temperature (K)

T2 = final temperature (K)

According to the information in this question,

P1 = 748mmHg

P2 = 400mmHg

V1 = 26.7 L

V2 = ?

T1 = 28.4 °C = 28.4 + 273 = 301.4K

T2 = -15.6 °C = -15.6 + 273 = 257.4K

Using P1V1/T1 = P2V2/T2

748 × 26.7/301.4 = 400 × V2/257.4

66.26= 1.554 V2

V2 = 66.26 ÷ 1.554

V2 = 42.64 L

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.

po-215 i got it right on the quiz