The reaction produces heat.
The reaction produces heat
THE REACTION IS ENDOTHERMIC
The reaction shows that calcium hydroxide (Ca(OH)2) dissociates in water to form calcium ions (Ca2+) and hydroxide ions (OH-). This dissociation leads to the formation of two hydroxide ions for every one calcium ion.
In this reaction, Ca2+ reacts with NO2^1- to form Ca(NO2)2. The balanced chemical equation for this reaction is: Ca2+ + 2NO2^- → Ca(NO2)2.
The reaction shows calcium ions (Ca2+) reacting with hydroxide ions (OH-) to form solid calcium hydroxide (Ca(OH)2) and release heat of 16.71 kJ. This reaction is exothermic, as indicated by the negative enthalpy change.
This reaction is exothermic.
the reaction produces heat
This reaction is exothermic.
The reaction is endothermic.
The reaction produces heat.
The reaction produces heat
THE REACTION IS ENDOTHERMIC
If you mean Ca(OH)2(s) --> Ca2+(aq) + 2OH-(aq) this is the equation for the dissolving of calcium hydroxide in water.
The reaction shows that calcium hydroxide (Ca(OH)2) dissociates in water to form calcium ions (Ca2+) and hydroxide ions (OH-). This dissociation leads to the formation of two hydroxide ions for every one calcium ion.
In this reaction, Ca2+ reacts with NO2^1- to form Ca(NO2)2. The balanced chemical equation for this reaction is: Ca2+ + 2NO2^- → Ca(NO2)2.
The reaction ( \text{Ca(OH)}_2(s) \rightleftharpoons \text{Ca}^{2+}(aq) + 2 \text{OH}^-(aq) ) with a change in enthalpy (( \Delta H )) of -16.71 kJ indicates that the dissolution of solid calcium hydroxide in water is an exothermic process. This means that heat is released when calcium hydroxide dissolves, resulting in a slight increase in the temperature of the solution. The negative value of ( \Delta H ) suggests that the products (dissolved ions) are more stable than the reactant (solid calcium hydroxide) in terms of energy.
The reaction shows calcium ions (Ca2+) reacting with hydroxide ions (OH-) to form solid calcium hydroxide (Ca(OH)2) and release heat of 16.71 kJ. This reaction is exothermic, as indicated by the negative enthalpy change.