What is meant by an exothermic reaction?, is a reaction which gives out heat energy to the surroundings., is a reaction which absorbs heat energy from the surroundings., What is meant by an endhothermic reaction?, is a reaction which absorbs heat energy from the surroundings., is a reaction which gives out heat energy to the surroundings., What is meant by enthalpy change? , the amount of heat given out in during a reaction , the amount of heat given taken in during a reaction, the amount of heat given out or taken in during a reaction is always the same, the amount of heat given out or taken in during a reaction, What type of reaction is it when the enthalpy change ΔH is positive?, Exothermic, Endothermic, What type of reaction is it when the enthalpy change ΔH is negative?, Exothermic, Endothermic, NaOH(aq) + HNO₃(aq) → NaNO₃(aq) + H₂O(l) ΔH = -57.3 kJ What is the enthalpy change if 2 moles of sodium hydroxide are completely neutralised, ΔH = -57.3 kJ, ΔH = 2 × (-57.3) = -114.6 kJ, ΔH = -2 × (-57.3) = 114.6 kJ, ΔH = 57.3 kJ, State whether the following are exothermic or endothermic reactions: Decomposing zinc carbonate, Exothermic, Endothermic, State whether the following are exothermic or endothermic reactions: Respiration, Exothermic, Endothermic, State whether the following are exothermic or endothermic reactions: Photosynthesis, Exothermic, Endothermic, Measuring enthalpy changes experimentally using..., Calorimetry, Hess’s law, Enthalpy cycles, Formula of ΔHf?, ΔHf = ΔH1 + ΔH2, ΔHf = ΔH2 + ΔH1, ΔHf = ΔH1 - ΔH2, ΔHf = ΔH2 - ΔH1, ΔH⦵f[Fe2O3(s)]=-842.2 kJ/mol and ΔH⦵f[Al2O3(s)]=-1675.7 kJ/mol, ∆Hr = 833.5 kJ/mol, ∆Hr = -833.5 kJ/mol, Find ∆Hr! N≡N = 941 kJ/mol ; H-H = 432 kJ/mol ; N-H = 391 kJ/mol , 2237 kJ/mol, 1064 kJ/mol, -54.5 kJ/mol, -109 kJ/mol, , Bonds formed - Bonds broken, Bonds broken - Bonds formed, , ∆Hr = 381+243 + (331+431), ∆Hr = 331+431 - (381+243), ∆Hr = 381+243 - (331+431), ∆Hr = -(381+243) - (331+431), Standard enthalpy change of formation is, C(graphite) + O2(g) —> CO2(g), C2H5OH(l) + 3O2(g) —> 2CO2(g) + 3H2O(l), 4C(graphite) + O2(g) + 6H2(g) —> 2C2H5OH(l), Standard enthalpy change of combustion is, C2H5OH(l) + 3O2(g) —> 2CO2(g) + 3H2O(l), 2C2H5OH(l) + 6O2(g) —> 4CO2(g) + 6H2O(l), Standard enthalpy change of neutralisation is, 2HCl(aq) + 2NaOH(aq)→ 2NaCl(aq) + 2H2O(l), HCl(aq) + NaOH(aq)→ NaCl(aq) + H2O(l), The enthalpy change when solutions of an acid and an alkali react together under standard conditions to produce ONE MOL OF WATER., STANDARD ENTHALPY CHANGE OF COMBUSTION, STANDARD ENTHALPY OF NEUTRALISATION, The enthalpy change when ONE MOLE of a compound is formed in its standard state from its elements in their standard states., STANDARD ENTHALPY CHANGE OF FORMATION, STANDARD ENTHALPY CHANGE OF COMBUSTION, The enthalpy change when ONE MOLE of a substance undergoes complete combustion under standard conditions. All reactants and products are in their standard states., STANDARD ENTHALPY CHANGE OF COMBUSTION, STANDARD ENTHALPY OF NEUTRALISATION, , Pressure = 101 kPa and Temperature = 298K, Pressure = 101 Pa and Temperature = 298K, The total enthalpy change in a chemical reaction is independent of the route by which the chemical reaction takes place as long as the initial and final conditions are the same. Its definition of, Calorimetry, Hess's Law, On complete combustion, 16g of methane raised the temperature of 100g water from 22°C to 27°C. If c = 4.18, calculate its enthalpy of combustion!, 2090 kJ/mol, 2.09 kJ/mol, On complete combustion, methane raised the temperature of 100g water from 22°C to 27°C. If c = 4.18, calculate its heat energy!, 2.09 J, 2090 J, , Exothermic, Endothermic, , Exothermic, Endothermic, ∆H positive, because, ΔH(reactants) > ΔH(products), ΔH(products) > ΔH(reactants).

Enthalpy Changes

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