Problem: Which one of the following statements is FALSE?The first law of thermodynamics says that the energy lost by the system must be gained by the surroundings.A positive ΔH corresponds to an endothermic process.The enthalpy change for a reaction is independent of the state of the reactants and products.The change of internal energy is the sum of heat and workIf work is done by the system, the sign of work is negative

FREE Expert Solution
81% (26 ratings)
Problem Details

Which one of the following statements is FALSE?

  1. The first law of thermodynamics says that the energy lost by the system must be gained by the surroundings.
  2. A positive ΔH corresponds to an endothermic process.
  3. The enthalpy change for a reaction is independent of the state of the reactants and products.
  4. The change of internal energy is the sum of heat and work
  5. If work is done by the system, the sign of work is negative

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Endothermic & Exothermic Reactions concept. You can view video lessons to learn Endothermic & Exothermic Reactions. Or if you need more Endothermic & Exothermic Reactions practice, you can also practice Endothermic & Exothermic Reactions practice problems.

How long does this problem take to solve?

Our expert Chemistry tutor, Sabrina took 2 minutes and 7 seconds to solve this problem. You can follow their steps in the video explanation above.