Chemical reaction between solid ammonium chloride and solid barium hydroxide octahydrate 2NH4Cl(s)+Ba(OH)*8H2O(s)->2NH3(aq)+BaCl2(aq)+10H2O(l) the change in heat for this reaction is 54.8kJ how much energy would be absorbed if 24.9g of NH4Cl reacts
Jennifer: all these problems are straightforward. I will be happy to check your work. Is there something specific you don't understand?
To calculate the energy absorbed during the reaction of 24.9g of NH4Cl, we need to use the concept of stoichiometry and the given change in heat for the reaction.
Stoichiometry is a relationship between the amounts of reactants and products involved in a chemical reaction. In this case, the balanced chemical equation tells us that 2 moles of NH4Cl react to produce 54.8 kJ of energy.
First, we need to convert the given mass of NH4Cl to moles. We can use the molar mass of NH4Cl to do so:
Molar mass of NH4Cl = (1 x atomic mass of N) + (4 x atomic mass of H) + (1 x atomic mass of Cl)
Molar mass of NH4Cl = (1 x 14.01 g/mol) + (4 x 1.01 g/mol) + (1 x 35.45 g/mol)
= 53.49 g/mol
Now we can calculate the number of moles of NH4Cl:
moles of NH4Cl = mass of NH4Cl / molar mass of NH4Cl
= 24.9 g / 53.49 g/mol
Next, we can use the stoichiometry of the balanced equation to find the energy absorbed during the reaction:
moles of NH4Cl reacted : moles of energy absorbed = 2 : 54.8 kJ
moles of energy absorbed = (moles of NH4Cl reacted × moles of energy absorbed) / 2
= (moles of NH4Cl reacted × 54.8 kJ) / 2
Finally, we can substitute the calculated value of moles of NH4Cl and solve for the energy absorbed:
energy absorbed = (moles of NH4Cl × 54.8 kJ) / 2
Plug in the value of moles of NH4Cl and calculate the energy absorbed.