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11 Dec 2019

the reaction between hydrogen and oxygen to yeild water vapor has H = -484kj. How much PV work is done, and what is the value of E in kilojoules for the reaction of .50 mol H2 with .25 mol of O2 at atmospheric preassure if the volume change is -5.6L?

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13 Dec 2019
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Related questions

2H2(g)+O2(g)----->2H2O(g) ?H=-484 KJ



How much PV work is done, and what is the value of ?E for thereaction of .50 mol of H2 with .25 mol of O2 at atmposphericpressure if the volume change is -5.6L?


I know delta E=DeltaH *PDeltaV, but how do I find PV work, andwhere do I use mols?

Used in welding metals, the reaction of acetylene with oxygen hasdeltaH = -1256.2 kJ
C2H2 (g) + 5/2 O2 (g) ---> H2O (g) + 2CO2 (g) deltaH = -1256.2kJ
How much PV work is done (in kilojoules) and what is the value ofdeltaE (in kilojoules) for the reaction of 6.50g of acetylene atatmospheric pressure if the volume change is -2.80 L?

1/ the total volume of hydrogen gass needed to fill the Hindenburge was 2x10^8 liters at 1 atm and 25*C. How Much energy was evolved when it burned ?

H2(g) + .5O2(g) ----> H2O(I) รขยˆย†H* = -286Kj

2/ The heat of formation of iron(III) oxide is -826KJ/mol. Calculate the heat of the reaction when a 55.8 g sample of iron is reacted with an excess of oxygen gas.

4Fe(s) + 3O2(g) -----> 2Fe2O3(s)

3/ the vapor pressure of water at 25*Celcius is 23.8 torr. Determine the mass of glucose( molar mass= 180g/mol) needed to add to 500 grams of water to change the vapor pressure to 23.1 torr.

4/ Consider the reaction H2(g) + .5O2(g) ----> H2O(I) รขยˆย†H*= -286 Kj

which of the following is true?

A/ The reaction is exothermic

B/ The reaction is endothermic

C/ The enthalpy of the products is less than that of the reactants.

D/ Heat is absorbed by the system

E/ The reaction is exothermic and the enthalpy of the products is less than that of the reactants.

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