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 temperature is 25.0 degrees Celsius (the heat capacity of water is 4.184 J/(g*degrees Celsius)

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

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

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?

For a butanol combustion process (formation enthalpy -332,000 kJ / kmol) C4H10O with an excess of...

For a butanol combustion process (formation enthalpy -332,000 kJ / kmol) C4H10O with an excess of 25% air (reagents are at standard conditions T = 25 C, P = 1atm). Determine: a. Adiabatic flame temperature b. If the products come out at a temperature of 600 K, determine the heat generated in the combustion chamber.

The enthalpy of combustion of solid carbon to form carbon dioxide is 2393.7 kJ/mol carbon, and...

The enthalpy of combustion of solid carbon to form carbon dioxide is 2393.7 kJ/mol carbon, and the enthalpy of combustion of carbon monoxide to form carbon dioxide is 2283.3 kJ/ mol CO. Use these data to calculate DH for the reaction 2C + O2 > 2CO

The enthalpy of combustion of octane is 5074.9 kJ/mol and its density is 703 kg/m3 ....

The enthalpy of combustion of octane is 5074.9 kJ/mol and its density is 703 kg/m3 . On a mild winter day a room of volume 40 m3 needs to be warmed up from 10 to 20 OC? (Consider: cair = 0.718 J/g K; dair = 1.225 g/L).

Calculate the enthalpy change for the reaction below given the standard heat of combustion for ammonia,...

Calculate the enthalpy change for the reaction below given the standard heat of combustion for ammonia, NH3, is -226 kJ/mol. 4NH3 (g) + 5O2(g) --> 4NO(g) + 6H2O(g)

Use standard heat of formations to find the heat for the combustion of 5.0 g of...

Use standard heat of formations to find the heat for the combustion of 5.0 g of Methane gas CH4 to form carbon dioxide and water vapor

The standard enthalpy of fusion of water is 6.01 kJ/ mol, the molar heat capacity at...

The standard enthalpy of fusion of water is 6.01 kJ/ mol, the molar heat capacity at a constant pressure of liquid water can be assumed to be constant at 75.5 J/mol*K, thoughout the liquid phase, and the standard enthalpy of vapoziration is 40.7 kJ/mol at the boiling point. Calculate the total entropy change (in SI units), for heating one mole of water, starting with ice just below the melting point and going to just above the boiling point at standard...

If a substance has a heat of condensation of –1.46 kJ/g and a heat of sublimation...

If a substance has a heat of condensation of –1.46 kJ/g and a heat of sublimation of 4.60 kJ/g, what is its heat of solidification in kJ/g? Answer: 1.46-4.60 kJ/g can you explain me why the asnwer is 1.46-4.60 kJ/g

At 25°C, the standard enthalpy of combustion of gaseous propane (C3H8) is –2219.0 kJ per mole...

At 25°C, the standard enthalpy of combustion of gaseous propane (C3H8) is –2219.0 kJ per mole of propane, and the standard enthalpy of combustion of gaseous propylene (C3H6) is –2058.3 kJ per mole of propylene. What is the standard enthalpy change for the following reaction at 25°C? C3H6(g) + H2(g) → C3H8(g) Substance ∆H°f (kJ/mol) CO2(g) –393.5 H2O(l) –285.8 a) +160.7 kJ b) –160.7 kJ c) +104.7 kJ d) –20.4 kJ e) –125.1 kJ

Subjects