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| Question | Answer |
| What is the Enthalpy Change of a Reaction? | The enthalpy change when the amount of reactants shown in the equation react under standard conditions to give the products in their standard states. |
| What is the Enthalpy Change of Combustion? | The enthalpy change when one mole of the substance is burnt in excess oxygen under their standard conditions. |
| What is the Enthalpy Change of Formation? | The enthalpy change when one mole of a substance is formed form its elements in their standard states. |
| Define exothermic. | Put simply; this is when heat is released into the surroundings. Enthalpy of the products is significantly lower than the enthalpy of its reactants - therefore showing a negative value to indicate a decrease in enthalpy (from reactants to products). Exothermic reactions also release energy to form bonds. |
| Define endothermic. | Put simply; this is when heat is taken in from its surroundings. Enthalpy of the products is significantly higher than its reactants - therefore showing a positive value to indicate the increase in enthalpy (from reactants to products). Endothermic reactions also take in energy to break bonds. |
| State Hess' Law. | The enthalpy change of a reaction depends on the initial and final states of a reaction - independent of the route by which it occurs. |
| State the term enthalpy. | The heat content / energy stored in a chemical system. |
| State the standard conditions. | The conditions required for all enthalpy calculations to occur - in which substances must also be in their standard states / most stable physical states. |
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