How to use Hess's Law to calculate enthalpy for the reaction?

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I have a serious Chemistry question, please help?

Use Hess's law and the measured mean enthalpy changes for the NaOH-HCl and NH3-HCl reactions to calculate the enthalpy change to be expected for the reaction? NaOH + NH3Cl ------> NaCl + NH3 + H2O Compare your experimental value with the one you have just calculated. The correct value is only -3.9KJ/mol. Try to explain any disrepency between the eperimental and calculated values and between these values and the correct value?

Answer:

(1) NaOH + HCl ===> NaCl + H2O /\H = x (2) NH3 + HCl ===> NH4Cl /\H = y x and y are minus-numbers...

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How to use Hess's Law to calculate enthalpy for the reaction?

Given the thermochemical equations H2 (g) + Br2 (g) => 2HBr (g) deltaH = -72 kJ H2 (g) => 2H (g) deltaH = 436 kJ Br2(g) => 2Br (g) deltaH = 224 kJ calculate the enthalphy change for H(g) + Br (g) => HBr (g) also if you could also solve this...

Answer:

we have to calculate delta H for : H + Br ------> HBr let, H2 + Br2 -----> 2HBr ......delta H...

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Use Hess' Law to calculate the enthalpy of formation of methanol (CH3OH)?

Methanol (wood alcohol) is extremely useful as a fuel, as a solvent, and as an antifreeze. However, it is also extremely poisonous; your body changes it into formaldehyde and formic acid after it is ingested. Drinking as little as 10 mL will cause permanent...

Answer:

First reverse the first equation and get CO2 + H2O-->CH3OH + 1.5O2 delta H=+726.4kj/mol Next double...

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Use Hess's law to calculate ΔH for the reaction below. N2(g) + 2 O2(g) 2 NO2(g)?

Consider the following data. N2(g) + O2(g) 2 NO(g) ΔH = +180.7 kJ 2 NO(g) + O2(g) 2 NO2(g) ΔH = -113.1 kJ 2 N2O(g) 2 N2(g) + O2(g) ΔH = -163.2 kJ Use Hess's law to calculate ΔH for the reaction below. N2(g) + 2 O2(g) 2 NO2(g)...

Answer:

You only need to use the first two equations. NO is a catalyst because it is a product in the first...

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Use Hess's law and the following equations to calculate ΔH for the reaction N2(g) +?

Use Hess's law and the following equations to calculate ΔH for the reaction N2(g) + 2O2(g) N2O4(g). (Show your work.) 2NO2(g) N2O4(g) ΔH = –57.0 kJ/mol N2(g) + O2(g) 2NO(g) ΔH = 180.6 kJ/mol 2NO2(g) 2NO(g) + O2(g) ΔH = ...

Answer:

THERMO

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Using Hess's Law, calculate the molar enthalpy of reaction for the combustion of ethene in kJ/mol.?

im not fully understanding of hess law but i got -1411 kj/mol for an answer

Answer:

That looks the right sort of order, and you've definitely got the sign correct, but without the figures...

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Calculate the enthalpy of the reaction: 2NO(g) + O2(g) --> 2NO2(g)?

Calculate the enthalpy of the reaction: 2NO(g) + O2(g) --> 2NO2(g) given the following reactions and enthalpies of formation: 1/2 N2(g) + O2(g) --> NO2(g), delta H *A = 33.2 kJ 1/2 N2(g) + 1/2O2(g) --> NO(g), delta H *B= 90.2 kJ Calculate the...

Answer:

The Hess law is used to discover the reaction's entalphy and doing it, you must cancel the same substances...

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Can someone good at calculating reaction enthalpy changes help me with this problem?

Usually I'm great with problem solving, math, chem, ect., but I can't figure it out for the life of me: Calculate the reaction enthalpy for the following reaction: 5CO2 + Si3N4 --> 3SiO + 2N20 + 5CO It gives me the following enthalpies and tells me...

Answer:

1) multiply first reaction by 3 2) do nothing to second reaction The result: 3CO + 3SiO2 --> 3SiO...

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Calculate enthalpy for the reaction?

I have a few problems I really need help on the first is: A) Use the (Delta)H^degree) data given to calculate (Delta)H^degree sign) for the reaction: C2H4(g) + H2(g) -> C2H4 Data: C2h4(g) + 3.5O2 -> 2CO2(g) + 3H2O(l) DeltaH^degree (KJ) -1560 C...

Answer:

1) first equation - flip it 2) second equation - leave untouched 3) third equation - divide by 2 Your...

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Use bond enthalpies to estimate the enthalpy change for the reaction of hydrogen with ethylene. H2(g) + C2?

(a) Use bond enthalpies to estimate the enthalpy change for the reaction of hydrogen with ethylene. H2(g) + C2H4(g) → C2H6(g) kJ (b) Calculate the standard enthalpy change for this reaction, using heats of formation. kJ Why does this value differ...

Answer:

Some discussion and examples: http://www.chemteam.info/Thermochem/Hess… reactants ---> one...

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