How much heat is liberated when 0.113 mole of sodium
reacts with excess water according to the following equation?
DH = -368 kJ/mol rxn
2Na + 2H2O ==> 2NaOH + H2
368 kJ x (0.113 mol/2 mol) = ?
2Na + 2H2O → H2 + 2NaOH is the balanced equation. from that, .113 mole/2=.0565 x -368 = -20.79kj or 20.79 kj heat is created in the reaction.
To calculate the heat liberated when 0.113 mole of sodium reacts with excess water, we can use the given enthalpy change (ΔH) of the reaction.
The enthalpy change (ΔH) of the reaction is -368 kJ/mol rxn. This means that 1 mole of sodium reacting with water releases 368 kJ of heat.
To find the heat liberated when 0.113 mole of sodium reacts, we can use a proportion:
(0.113 mole / 1 mole) = (heat liberated / -368 kJ)
Let's solve for the heat liberated:
heat liberated = (0.113 mole / 1 mole) * -368 kJ
heat liberated = -41.584 kJ
Therefore, when 0.113 mole of sodium reacts with excess water, approximately -41.584 kJ of heat is liberated. Note that the negative sign indicates that the reaction is exothermic, meaning heat is released.
To calculate the amount of heat liberated in the reaction, we need to use the given value of ΔH (enthalpy change) and the number of moles of sodium participating in the reaction.
The equation provided is:
2 Na + 2 H2O -> 2 NaOH + H2
From the balanced equation, we can see that 2 moles of sodium react to form 368 kJ of heat (ΔH = -368 kJ/mol rxn). This means that the reaction produces 368 kJ of heat for every 2 moles of sodium.
So, we need to find the amount of heat produced when 0.113 moles of sodium reacts with water.
To find the amount of heat for a given number of moles, we can set up a proportion:
(0.113 moles of sodium / 2 moles of sodium) = (x kJ of heat / 368 kJ of heat)
Cross-multiplying, we get:
0.113 moles of sodium * 368 kJ of heat = 2 moles of sodium * x kJ of heat
Simplifying the equation:
x = (0.113 moles of sodium * 368 kJ of heat) / 2 moles of sodium
x = 20.9 kJ
Therefore, when 0.113 moles of sodium reacts with excess water, approximately 20.9 kJ of heat is liberated.