Question

A balloonist begins a trip in a helium-filled balloon in early morning when the temperature is 15°C. By mid-afternoon, the temperature is 30.°C. Assuming the pressure remains at 1.00 atm, for each mole of helium, calculate the following:
(e) ΔH for the process (in J)

Answer 1

ΔH(enthalpy change) for the process is 311.775J.

The amount of heat released or absorbed during a reaction that takes place under constant pressure is referred to as the enthalpy change. The sign for it is H, which can be read as "ΔH." Note that only reactions carried out under constant pressure are covered by the phrase "enthalpy change."

Enthalpy is significant because it tells us how much heat is there in a system (energy). Heat is crucial because it allows us to produce useful work. In terms of a chemical process, an enthalpy shift reveals how much enthalpy was gained or lost. Enthalpy is the system's heat energy.

A reaction is endothermic if the enthalpy of the products is larger than the enthalpy of the reactants, as indicated by a positive ΔH value. This indicates that higher energy products were created from lower energy reactants and that the higher energy change was a result of energy absorption from the environment.

Cp =5/2 R

Enthalpy change= nCpΔT

Enthalpy change= 1×5/2 R × (T2 − T1)

Enthalpy change=  $\frac{5*8.314}{2}$ × 15

Enthalpy change = 311.775 J

To know more about Enthalpy change refer to:  brainly.com/question/4526346

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