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 in air to produce a
bright light and is often used in fireworks displays.
The
combustion of magnesium produces magnesium
oxide solid. This reaction releases
1203 kJ of energy.
3-Write a balanced thermochemical equation for the combustion of
magnesium.
(b) How much heat (in kJ) is released by the combustion of 8.33 g
of magnesium?
4. Applying Hess’s Law, from the enthalpies of reactions,
Homework Answers
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Applying Hess’s Law, from the enthalpies of reactions,
2NaCl(s) + H2O(l) --> 2HCl(g) + Na2O(s) ΔH...
Help me get the answer -78.5 2) Use Hess's law to calculate the enthalpy of the...
Help me get the answer -78.5
2) Use Hess's law to calculate the enthalpy of the reaction below using the following information. [Ans: -78.5] HCl(g) + NaNO2(s) → HNO2(1) + NaCl(s) AH=? 2NaCl(s) + H2O(l) + 2HCl(g) + Na2O(s) NO(g) + NO2(g) + Na2O(s) - 2NaNO3(s) NO(g) + NO2(g) N2O(g) + O2(g) 2HNO2(1) - N2O(g) + O2(g) + H2O(1) AH = 507 kJ AH = -427 kJ AH = -43 kJ AH = 34 kJ
Use the enthalpies for the given reactions to compute the standard enthalpy change (ΔH°) for the...
Use the enthalpies for the given reactions to compute the standard enthalpy change (ΔH°) for the reaction: 6 C (s) + 7 H2(g) → C6H14 (l) ΔHrxn = ? C6H14 (l)+19/2O2 (g)→6CO2(g)+ 7H2O(g). ΔH=–3505.8kJ C(s) + O2 (g) → CO2(g) ΔH=–393.5kJ H2(g) + 1/2 O2(g) → H2O(g). ΔH = – 242.0 kJ
Using Hess’s Law to Calculate ΔH Calculate ΔH for 2 NO(g) + O2(g) → N2O4(g) using...
Using Hess’s Law to Calculate ΔH Calculate ΔH for 2 NO(g) + O2(g) → N2O4(g) using the following information: N2O4(g)2 NO(g) + O2(g)→→2 NO2(g)2 NO2(g)ΔHΔH==+57.9 kJ−114.1 kJ Calculate for using the following information: Select one 2.7 kJ -55.2 kJ -85.5 kJ -171.0 kJ +55.2 kJ
Use Hess' Law to calculate the ΔH for the following reaction from the data given below....
Use Hess' Law to calculate the ΔH for the following reaction from the data given below. Na2CO3(s) + 2HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l) ΔH = _________ Na2CO3(s) → CO2(g) + Na2O(s) ΔH = 319.8 kJ 2NaCl(aq) + H2O(l) → 2HCl(aq) + Na2O(s) ΔH = +348.0 kJ
(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.)...
Use Hess’s law to calculate ∆H° forthe reaction:C(s) + 2H2(g) +½O2(g) → CH3OH(l)...
Use Hess’s law to calculate ∆H° for the reaction:C(s) + 2H2(g) + ½O2(g) → CH3OH(l) ∆H°∘= ?using only the following data:H2(g) + ½O2(g) → H2O(l) ∆H°= -285.8 kJC(s) + O2(g) → CO2(g) ∆H°= -393.5 kJ2CH3OH(g) + 3O2(g) → 2CO2(g) + 4H2O(l) ∆H°= -1452.8 kJ
Part A Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of fo...
Part A Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ 12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ Express your answer with the appropriate units. Part B Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ 2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ H2O(l)→H2O(g), ΔH∘D=+44 kJ Express your answer with the appropriate units.
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH′s. C5H12(l...
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH′s. C5H12(l)+8O2(g)→5CO2(g)+6H2O(g), ΔH= -3244.8 kJ C(s)+O2(g)→CO2(g), ΔH= -393.5 kJ 2H2(g)+O2(g)→2H2O(g), ΔH= -483.5 kJ Express your answer to for significant figures.
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH values: C5H12(l)+8O2(g)→5CO2(g)+6H2O(g),...
Calculate ΔHrxn for the following reaction: 5C(s)+6H2(g)→C5H12(l) Use the following reactions and given ΔH values: C5H12(l)+8O2(g)→5CO2(g)+6H2O(g), ΔH= -3244.8 kJ C(s)+O2(g)→CO2(g), ΔH= -393.5 kJ 2H2(g)+O2(g)→2H2O(g), ΔH= -483.5 kJ
Consider the following chemical reaction. NH3(g) + 2 O2(g) → HNO3(aq) + H2O(l) Calculate the change...
Consider the following chemical reaction. NH3(g) + 2 O2(g) → HNO3(aq) + H2O(l) Calculate the change in enthalpy (ΔH) for this reaction, using Hess' law and the enthalpy changes for the reactions given below. (1a) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l); ΔH = −1166.0 kJ/mol (2a) 2 NO(g) + O2(g) → 2 NO2(g); ΔH = −116.2 kJ/mol (3a) 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g); ΔH = −137.3 kJ/mol
Help me get the answer -78.5
2) Use Hess's law to calculate the enthalpy of the reaction below using the following information. [Ans: -78.5] HCl(g) + NaNO2(s) → HNO2(1) + NaCl(s) AH=? 2NaCl(s) + H2O(l) + 2HCl(g) + Na2O(s) NO(g) + NO2(g) + Na2O(s) - 2NaNO3(s) NO(g) + NO2(g) N2O(g) + O2(g) 2HNO2(1) - N2O(g) + O2(g) + H2O(1) AH = 507 kJ AH = -427 kJ AH = -43 kJ AH = 34 kJ
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