Find ΔH° for the complete combustion of gaseous methoxyethane , C3H8O(g) , using the data below....

Find ΔH° for the complete combustion of gaseous methoxyethane , C3H8O(g) , using the data below.

C(s) + O2(g) → CO2(g)

ΔH°= -393.52 kJ/mol

H2(g) + ½O2(g) → H2O(l)

ΔH°= -285.83 kJ/mol

3C(s) + 4H2(g) + ½O2(g) → C3H8O(g)

ΔH°= -216.4 kJ/mol

ΔH° for the complete combustion of gaseous methoxyethane

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Calculate ΔH° for the reaction C4H4(g) + 2H2(g) → C4H8(g), using the following data: ΔH°combustion for...

Calculate ΔH° for the reaction C4H4(g) + 2H2(g) → C4H8(g), using the following data: ΔH°combustion for C4H4(g) = –2341 kJ/mol ΔH°combustion for H2(g) = –286 kJ/mol ΔH°combustion for C4H8(g) = –2755 kJ/mol A) –128 kJ B) 158 kJ C) –158 kJ D) 128 kJ E) None of these choices are correct.

Find ΔH° for the formation of liquid n-hexane, C6H14(l), using the data below. C(s) + O2(g)...

Find ΔH° for the formation of liquid n-hexane, C6H14(l), using the data below. C(s) + O2(g) → CO2(g) ΔH°= -393.52 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔH°= -285.83 kJ/mol C6H14(l) + 9½O2(g) → 6CO2(g) + 7H2O(l) ΔH°= -4163.13 kJ/mol The heat of formation of liquid n-hexane is AnswerkJ mol-1.

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?

Complete combustion of 7.70 g of a hydrocarbon produced 23.6 g of CO2 and 11.3 g...

Complete combustion of 7.70 g of a hydrocarbon produced 23.6 g of CO2 and 11.3 g of H2O. What is the empirical formula for the hydrocarbon? Insert the subscripts: CH

Given the following heats of formation (ΔH°f, 25°C) and heats of combustion (ΔH°c, 25°C) data, determine...

Given the following heats of formation (ΔH°f, 25°C) and heats of combustion (ΔH°c, 25°C) data, determine the heat of reaction for the liquid-phase esterification of lactic acid (C3H6O3) with ethanol (C2H5OH) to form ethyl lactate (C5H10O3) and liquid water at 25°C and 1 atm. C3H6O3 + C2H5OH --> C5H10O3 + H2O (liquid) The table below shows the standard heat of combustion and heat of reaction. Compound ΔH°c (25°C, 1 atm) kJ/mol ΔH°f (25°C, 1 atm) kJ/mol C3H6O3 - -687.0 C2H5OH...

Subjects