(c) For a given process at constant pressure, _x001F_H is negative. Is the process endothermic or exothermic?

Verified step by step guidance

Step 1: Understand the terms 'endothermic' and 'exothermic'. An endothermic process absorbs heat from the surroundings, while an exothermic process releases heat to the surroundings.

Step 2: Recognize that the symbol ΔH represents the change in enthalpy, which is the heat change at constant pressure.

Step 3: Note that a negative ΔH indicates that the system is losing heat to the surroundings.

Step 4: Connect the concept of a negative ΔH with the definition of an exothermic process, which is characterized by the release of heat.

Step 5: Conclude that if ΔH is negative, the process is exothermic, as it involves the release of heat to the surroundings.

Related Practice

During a deep breath, our lungs expand about 2.0 L against an external pressure of 101.3 kPa. How much work is involved in this process (in J)?

574

views

Textbook Question

How much work (in J) is involved in a chemical reaction if the volume decreases from 33.6 L to 11.2 L against a constant pressure of 90.5 kPa?

747

views

Open Question

(a) Under what condition will the enthalpy change of a process equal the amount of heat transferred into or out of the system? (b) During a constant-pressure process, the system releases heat to the surroundings. Does the enthalpy of the system increase or decrease during the process? (c) In a constant-pressure process, _x001F_H = 0. What can you conclude about _x001F_E, q, and w?

Open Question

Assume that 2 moles of water are formed according to the following reaction at constant pressure (101.3 kPa) and constant temperature (298 K): 2 H2(g) + O2(g) → 2 H2O(l). (b) Calculate _x001F_E for the reaction using your answer to (a).

Open Question

Suppose that the gas-phase reaction 2 NO(g) + O2(g) → 2 NO2(g) were carried out in a constant-volume container at constant temperature. (a) Would the measured heat change represent _x001F_H or _x001F_E? (b) If there is a difference, which quantity is larger for this reaction? (c) Explain your answer to part (b).