1.
HCl is a strong acid and NaOH is a strong base. Hence, they will undergo neutralization reaction to form a salt and water as follows:
Note that the reaction is already balanced as both sides have same number of each type of atoms.
HCl is a strong acid and NH3 is a weak Lewis base. Hence, they form a acid-base complex as given below:
Note that the above reaction is also balanced.
Now, the balanced reaction between strong base NaOH and NH4Cl can be written as follows:
Note that this is simply a displacement reaction when cation of one reactant combines with anion of another.
2.
For a generic reaction
The enthalpy change for the reaction, , can be written in terms of the enthalpies of formation, , of the reactants and products as follows:
Where a, b, c and d are stoichiometric coefficients in the balanced reaction.
Hence, for our reactions:
The enthalpy of the neutralization reaction can be written as
For the second reaction:
The enthalpy of the reaction can be written as
Now, for the third reaction of NH4Cl and NaOH,
we can write the enthalpy change of the reaction as
Now, we have to prove that
Hence, lets evaluate the right hand side of the equation and check if it equals the LHS.
Hence, subtracting equation (2 ) from equation (1).
Note that the right hand side of the third step of the above equation is equal to enthalpy change calculated in equation 3.
Hence, it is proved.
1. Write balanced equations for the two reactions that will be carried out in this experiment...
Questions: 1. Write balanced equations for each of the four different acid-base reactions in this experiment. Include phases (s, 1, g, aq) for reactants and products. Naoteit HChagj- NaOH agl+ NH2 (09) t HUiagy NHz 491 HadtNaa (a4) Hao t NaCats HCaHso (44) NH4 ca) + C211202a) t 2. How does the enthalpy of neutralization change when you switch from a strong acid to a weak acid with the same base? From a strong base to a weak base with...
Show using Hess's Law how the enthalpy of reaction for HCLg + NaOH (you don't need specific numbers, just call it AH) minus the enthalpy of reaction for HCL) + NH3(aq) (call it AH) should be equal to the enthalpy of reaction for NaOH. + NH,CIQ). Show all work.
Show using Hess's Law how the enthalpy of reaction for HCLg + NaOH (you don't need specific numbers, just call it AH) minus the enthalpy of reaction for HCL) + NH3(aq) (call it AH) should be equal to the enthalpy of reaction for NaOH. + NH,CIQ). Show all work.
I know that this is the answer, but how do I cancel out equations to reach it ? Calculate the enthalpy change to be expected for the dissolution of NaOH ((s) and (aq) mean solid and aqueous) using Hess's Law: NaOH(s) NaOH(aq) Use the enthalpy change for NaOH-HCI pair that your class measured in this experiment, and the data from the following table: Reaction* AH(kJ/mol %H2(g) + 2Cl2(g) → HCl(g) - 92.31 Na(s) + 1202(g) + 12H2(g) → NaOH(s) -...
POST LABORATORY QUESTIONS 1. a. For the neutralization reaction that you carried out between HCl(aq) and NaOH (ag). how many moles of NaCl(aq) were produced? b. For the neutralization reaction that you carried out between HCl(aq) and NaOH() how many moles of NaCl(aq) were produced? 2. Calculate AHan for the neutralization of HCl(aq) and NaOH(aq) in kilojoules per mol of NaCl b. Calculate A Hexn for the neutralization of HCl (aq) and NaOH(s) in kilojoules per mol of NaCl 3....
4. Write balanced molecular and ionic equations for following reactions: a. CaCOs(s) and HCI(aq) b. Well 5CINi(NO32 NaOH and HCl(aq) c. HCI(aq) NH3(aq) d. CH3COOH(aq)+ NaOH(aq)
4. You will conduct the two solvation reactions and three neutralization reactions in this experiment. In the space provided below, write the balanced net ionic reaction equations from the descriptions. Use the table of thermodynamic data in your text (AHf(NaOH(s)= -425.61 kJ-mol) to calculate the molar enthalpy of the reactions. These will be the accepted values you will compare to the experimental values you calculate using data collected during the experiment. Part I: Solid sodium hydroxide is combined with water...
Write complete, balanced equations for each of the following reactions. If no reaction is predicted, enter "no reaction": (a) Mg(OH)2(aq) + H3PO4(aq) → (b) HCl(aq) + NaOH(aq) → (c) H3PO4(aq) + Ca(OH)2(aq) → (d) Fe(s) + CuSO4(aq) → (e) AgNO3(aq) + Cu(s) → (f) C5H12(g) + O2(g) →
Write the molecular, ionic, and net equations of the 5 following reactions. (Must be balanced if not already balanced) Cu2+ (s) + 2HNO3 (l) --> Cu(NO3)2 (s) + NO-2 (?) + H2O (l) Cu(NO3)2 (l) + NaOH (?) --> Cu(OH)2 (?) + NaNO3 (?) Cu(OH)2 (aq) --> CuO (s) + H2O (l) CuO (s) + H2SO4 (s) --> CuSO4 (aq) + H2O (l) CuSO4 (aq) + Mg2+ (s) --> MgSO4 (aq) + Cu2+ (s) I have placed question marks for...
Il. Results The objective of this experiment is to calculate the enthalpy of foermation for NH.CKs) (Reminder-beat of formation is the ΔΗ for the formation of one mole of a compound from the elements.) Write the balanoed chemical equation for the formation of 1 mole ot NILC1(S) from the elements Na (g). H: (B) and Clh (g. EQUATION (3): Use the two following equations and Equations (1) and (2), sound previously, to calculate the enthalpy formation for NIH.CI(s). Apply Hess's...