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) âH* = -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) âH*= -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.
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) âH* = -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) âH*= -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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