Generally enthalpy values are given in kJ/mol. However, convert the enthalpy of neutralization value of -110.83...
Generally enthalpy values are given in kJ/mol. However, convert the enthalpy of neutralization value of -110.83 kJ/molNaOH to BTU/gram NaOH. BTU stands for British thermal unit. (Put your answer in 3 significant figures)
Given the following information below, use Hess’s Law to calculate the enthalpy of formation for sodium oxide:
Na (s) + HCl (l) à NaCl (aq) + ½ H2 (g) ∆HRx = -397.9 kJ/mol
Na2O (s) + 2 HCl (l) à 2 NaCl (aq) + H2O ∆HRx = -652.8 kJ/mol
H2 (g) + ½ O2 (g) à H2O (g) ∆HRx = -287 kJ/mol
2 Na (s) + ½ O 2 (g) à Na 2O (s) ∆ HRx = __________ kJ/mol
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Generally enthalpy values are given in kJ/mol. However, convert
the enthalpy of neutralization value of -110.83...
Generally enthalpy values are given in kJ/mol. However, convert the enthalpy of neutralization value of -100.57...
Generally enthalpy values are given in kJ/mol. However, convert the enthalpy of neutralization value of -100.57 kJ/mol NaOH to BTU/gram NaOH. BTU stands for British thermal unit. (Put your answer in 3 significant figures)
How can i calculate the enthalpy of reaction for both neutralization reactions (HCL + NaOH) and...
How
can i calculate the enthalpy of reaction for both neutralization
reactions (HCL + NaOH) and (Citric acid + NaHCO3) with units of
Kj/mol?
Enthalpy of formation:
Hcl (aq): -167.2 kj/mol
NaOH (aq): -469.6 kj/mol
citric acid (aq): not sure
NaHCO3 (s): -947.7 kj/mol
neutralization reactions that occur when an acid reacts with a base. HCI (aq) + NaOH (aq) → H20 (1) + NaCl (aq) HzC6H50, (citric acid) (aq) + 3 NaHCO3 (s) → Na2C8H:07 (aq) + 3 CO2...
THe enthalpy of neutralization of HCN (aq) with NaOH (aq) is -12.0 kJ/mol. Using your value...
THe enthalpy of neutralization of HCN (aq) with NaOH (aq) is -12.0 kJ/mol. Using your value for the enthalpy of neutralization of H+(aq) with OH-(aq) and the technique used in question 2, determine the enthalpy of ionization of HCN. Compare the relative amounts of ionization of HCL and HC2H3O2. Which is the stronger acid? Question 2. The neutralization of HC2H3O2 (aq) by NaOH(aq) (part C) can be considered to be the sum of the neutralization of H+(aq) by OH-(aq) (part...
Applying Hess’s Law, from the enthalpies of reactions, 2NaCl(s) + H2O(l) --> 2HCl(g) + Na2O(s) ΔH...
Applying Hess’s Law, from the enthalpies of reactions, 2NaCl(s) + H2O(l) --> 2HCl(g) + Na2O(s) ΔH = + 507.31 kJ NO(g) + NO2(g) + Na2O(s) --> 2NaNO2(s) ΔH = − 427.14 kJ NO(g) + NO2(g) --> N2O(g) + O2(g) ΔH = − 42.68 kJ 2HNO2(l) --> N2O(g) + O2(g) + H2O(l) ΔH = + 34.35 kJ Calculate the enthalpy change (ΔHrxn) for the reaction: HCl(g) + NaNO2(s) --> HNO2(l) + NaCl(s) (You should show work to get credit) 5-Magnesium burns...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table provided, calculate the enthalpy of reaction ΔH°rxn (in kJ) for each of the following reactions: Standard Enthalpies of Formation substance ΔHf° in kJ/mol Mg(s) 0 MgO(s) -601.6 HCl(aq) -167.2 MgCl2(aq) -801.2 H2(g) 0 H2O(l) -285.8 Reaction #1: Mg (s) + 2HCl (aq) è MgCl2 (aq) + H2 (g) Reaction #2: MgO (s) + 2HCl (aq) è MgCl2 (aq) + H2O (l) 2. (4 pts.)...
Calculate the enthalpy change for the following reactions. Balance the equation and calculate the enthalpy change:...
Calculate the enthalpy change for the following reactions. Balance the equation and calculate the enthalpy change: 9. MgO(s) + H, (g) + Mg(s) + H,O(1) Mg(s) + 12 0,) ► MgO(s) AH =-602 kJ H,(s) + 0,(9) H,00 AH = –242 kJ 602 kJ - 242 kJ = 360 kJ = AH 10. NaCl(s) + H2O → Na+ (aq) + Cl(aq) NaCl(s) → Nat(g) + CH) Nat(g) + CHg) → Na*(aq) + Cl(aq) AH =? AH = 788 kJ/mol AH...
I know that this is the answer, but how do I cancel out equations to reach...
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) -...
3) Calculate the AH,º for the following reactions based on the standard heat of enthalpy of each compound. AH° (kJ/...
3) Calculate the AH,º for the following reactions based on the standard heat of enthalpy of each compound. AH° (kJ/mol): HCl(g) → -92.3, NaCl(s) →-411.0, NaOH(s) →-426.7. H2O(g) +-241.8 SO2(g) → -296.8, H2S(g) → -20.0, O2(g) → 0.0, H2O(l) →-285.8 a) NaOH(s) + HCl(g) ----> NaCl(s) + H2O(g) b) 2 H2S(g) + 3 O2(g) ---> 2 H2O(l) + 2 SO2(g)
calculate the standard enthalpy change (in kJ/mol) for each of the following reactions. Ni(s) + Cl2(g)...
calculate the standard enthalpy change (in kJ/mol) for each of the following reactions. Ni(s) + Cl2(g) → NiCl2(s) kJ/mol B2O3(s) + 3 H2(g) → 2 B(s) + 3 H2O(l) kJ/mol 2 KOH(s) + CO2(g) → K2CO3(s) + H2O(g) kJ/mol 2 Cu(s) + Cl2(g) → 2 CuCl(s) kJ/mol
The following table lists some enthalpy of formation values for selected substances. Substance ΔfH∘ΔfH∘ (kJ mol−1)(kJ...
The following table lists some enthalpy of formation values for selected substances. Substance ΔfH∘ΔfH∘ (kJ mol−1)(kJ mol−1) CO2(g)CO2(g) −393.5−393.5 Ca(OH)2(s)Ca(OH)2(s) −986.1−986.1 H2O(l)H2O(l) −285.8−285.8 CaCO3(s)CaCO3(s) −1207−1207 H2O(g)H2O(g) −241.8−241.8 Part A: Determine the enthalpy for this reaction: Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l) C a ( O H ) 2 ( s ) + C O 2 ( g ) → C a C O 3 ( s ) + H 2 O ( l ) Express your answer in kJ mol−1 k J m o l...
How
can i calculate the enthalpy of reaction for both neutralization
reactions (HCL + NaOH) and (Citric acid + NaHCO3) with units of
Kj/mol?
Enthalpy of formation:
Hcl (aq): -167.2 kj/mol
NaOH (aq): -469.6 kj/mol
citric acid (aq): not sure
NaHCO3 (s): -947.7 kj/mol
neutralization reactions that occur when an acid reacts with a base. HCI (aq) + NaOH (aq) → H20 (1) + NaCl (aq) HzC6H50, (citric acid) (aq) + 3 NaHCO3 (s) → Na2C8H:07 (aq) + 3 CO2...
Calculate the enthalpy change for the following reactions. Balance the equation and calculate the enthalpy change: 9. MgO(s) + H, (g) + Mg(s) + H,O(1) Mg(s) + 12 0,) ► MgO(s) AH =-602 kJ H,(s) + 0,(9) H,00 AH = –242 kJ 602 kJ - 242 kJ = 360 kJ = AH 10. NaCl(s) + H2O → Na+ (aq) + Cl(aq) NaCl(s) → Nat(g) + CH) Nat(g) + CHg) → Na*(aq) + Cl(aq) AH =? AH = 788 kJ/mol AH...
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) -...
3) Calculate the AH,º for the following reactions based on the standard heat of enthalpy of each compound. AH° (kJ/mol): HCl(g) → -92.3, NaCl(s) →-411.0, NaOH(s) →-426.7. H2O(g) +-241.8 SO2(g) → -296.8, H2S(g) → -20.0, O2(g) → 0.0, H2O(l) →-285.8 a) NaOH(s) + HCl(g) ----> NaCl(s) + H2O(g) b) 2 H2S(g) + 3 O2(g) ---> 2 H2O(l) + 2 SO2(g)
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