which one of the following statements is false? group of answer choices if qp for a process is negative, the process is exothermic. the change in internal energy, de, for a process is equal to the amount of heat absorbed at constant volume, qv. the change in enthalpy, dh, for a process is equal to the amount of heat absorbed at constant pressure, qp. a bomb calorimeter measures dh directly.

The false statement is: 'A bomb calorimeter measures ΔH directly'. This is incorrect as a bomb calorimeter measures the change in internal energy not the change in enthalpy.

Explanation:

The false statement is: 'A bomb calorimeter measures ΔH directly'. This is incorrect because a bomb calorimeter measures the heat produced by a reaction at constant volume, which corresponds to the change in internal energy (ΔE) not the change in enthalpy (ΔH). In a calorimetry, an exothermic reaction will transfer thermal energy from the system to its surroundings, and the heat (q) is negative. Conversely, an endothermic process absorbs heat, meaning thermal energy is transferred from the surroundings to the system, and q is positive.

The change in internal energy for a process is indeed equal to the amount of heat absorbed at constant volume (qv) and the change in enthalpy, ΔH, for a process is equal to the amount of heat absorbed at constant pressure (qp).

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