Question

In: Chemistry

The combustion of 0.4196 g of hydrocarbon releases 17.55 kJ of heat. The masses of the...

The combustion of 0.4196 g of hydrocarbon releases 17.55 kJ of heat. The masses of the products are 1.418 g of carbon dioxide (CO2) and 0.290 g of water (H2O). The standard formation enthalpy for CO2(g) and H2O(l) are −393.5 kJ/mol and −285.8 kJ/mol, respectively.

(a) What is the empirical formula of the compound?



(b) If the approximate molar mass of the compound is 76 g/mol, calculate the standard enthalpy of formation.

Δ

H

o

f

=

kJ

mol

Solutions

Expert Solution

queen_honey_blossom answered 9 months ago
Next > < Previous

Related Solutions

Heat of Combustion and Enthalpy The heat of combustion of hexane is 45.6 kj/g. If you...
Heat of Combustion and Enthalpy The heat of combustion of hexane is 45.6 kj/g. If you burn all of a 1.20 g sample of hexane, and all of the heat is transferred to a pot of water determine the following: (a)The amount of heat in J, and the sign of the energy change (b)The amount of heat absorbed in water: (c) The final temperature of water if there are 250 g of water in the pot, and the intial water...
A system releases 65 kJ of heat and receives 82 kJ of work. What is ∆E?...
A system releases 65 kJ of heat and receives 82 kJ of work. What is ∆E? Is the process endothermic or exothermic?
The heat of combustion of benzoic acid (C6H5COOH) is -3226 kJ/mol. When 0.919 g of benzoic...
The heat of combustion of benzoic acid (C6H5COOH) is -3226 kJ/mol. When 0.919 g of benzoic acid was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose from 22.25 °C to 26.27 °C. What is the heat capacity (calorimeter constant) of the calorimeter?
an unkown hydrocarbon contain carbon hydrogen and oxygen combustion of 1.6 g of the hydrocarbon produces...
an unkown hydrocarbon contain carbon hydrogen and oxygen combustion of 1.6 g of the hydrocarbon produces 1.0286 g h2o and 3.7681 g co2. what is the empiral formula of this compound?
Complete combustion of 8.40 g of a hydrocarbon produced 25.4 g of CO2 and 13.0 g...
Complete combustion of 8.40 g of a hydrocarbon produced 25.4 g of CO2 and 13.0 g of H2O. What is the empirical formula for the hydrocarbon?
complete combustion of 3.70 g of a hydrocarbon produced 11.9 g of CO2 and 4.06 g...
complete combustion of 3.70 g of a hydrocarbon produced 11.9 g of CO2 and 4.06 g of H20. What is the empirical formula for the hydrocarbon?
Complete combustion of 8.00 g of a hydrocarbon produced 24.5 g of CO2 and 11.7 g...
Complete combustion of 8.00 g of a hydrocarbon produced 24.5 g of CO2 and 11.7 g of H2O. What is the empirical formula for the hydrocarbon?
Complete combustion of 8.50 g of a hydrocarbon produced 27.2 g of CO2 and 9.73 g...
Complete combustion of 8.50 g of a hydrocarbon produced 27.2 g of CO2 and 9.73 g of H2O. What is the empirical formula for the hydrocarbon?
Complete combustion of 7.60 g of a hydrocarbon produced 23.0 g of CO2 and 11.8 g...
Complete combustion of 7.60 g of a hydrocarbon produced 23.0 g of CO2 and 11.8 g of H2O. What is the empirical formula for the hydrocarbon? I got C4H10 but was incorrect.
Complete combustion of 7.90 g of a hydrocarbon produced 24.2 g of CO2 and 11.6 g...
Complete combustion of 7.90 g of a hydrocarbon produced 24.2 g of CO2 and 11.6 g of H2O. What is the empirical formula for the hydrocarbon?
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT