From the data below, calculate the total heat (in J) needed to convert 0.535 mol of...

From the data below, calculate the total heat (in J) needed to convert 0.535 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm:

b.p. at 1 atm: 78.5°C

ΔH o vap : 40.5 kJ/mol

cgas: 1.43 J/g·°C

cliquid: 2.45 J/g·°C

______J

Expert Solution

here is the answers, please see the images.

N.B-heat change at constant pressure is equal to the enthalpy change of the system.

queen_honey_blossom answered 1 year ago

From the following data, calculate the total heat (J) needed to convert 0.394 mol ethanol gas...

From the following data, calculate the total heat (J) needed to convert 0.394 mol ethanol gas at 401°C and 1 atm to liquid ethanol at 25.0°C and 1 atm. Boiling point at 1 atm 78.5°C cgas 1.43 J/g·°C cliquid 2.45 J/g·°C ΔH°vap 40.5 kJ/mol

Calculate the total heat (in J) needed to covert 0.333 mol of gaseous ethanol (CH3CH2OH) at...

Calculate the total heat (in J) needed to covert 0.333 mol of gaseous ethanol (CH3CH2OH) at 300 °C and 1 atm to liquid ethanol at 25.0°C and 1 atm. Use the following data: Normal bp = 78.5 °C, ΔHvap = 40.5 kJ mol-1, cgas = 1.43 J g-1 °C-1, cliq = 2.45 J g-1 °C-1.

Calculate the total amount of heat needed to convert 76.3g of water from -27 C to...

Calculate the total amount of heat needed to convert 76.3g of water from -27 C to 109 C. Cice = 37.6 J/(mol x °C) ; CH2O(l) = 75.4 J/(mol x oC); CH2O(g) = 33.1 J/(mol x oC) ∆Hofus = 6.02 kJ/mol; ∆Hovap = 40.7 kJ/mol

Calculate the total energy (in joules) needed to convert 15.0 grams of liquid ethanol at 25...

Calculate the total energy (in joules) needed to convert 15.0 grams of liquid ethanol at 25 0C to gas at 78 0C (boiling point). The specific heat of ethanol is 2.46 J/g 0C and the heat of vaporization is 841 J/g.

What is the total quantity of heat required to convert 0.45 moles of ice from –7.0...

What is the total quantity of heat required to convert 0.45 moles of ice from –7.0 °C to steam at 108.0 °C? ΔHfus = 334 J/g ΔHvap = 2260 J/g Cice(s) = 2.09 J/g⋅°C Cwater(l) = 4.18 J/g⋅°C Csteam(g) = 2.03 J/g⋅°C

Consider the following data: ΔvapH = 5.56 kJ/mol Specific heat capacity of N2(g) = 29.2 J...

Consider the following data: ΔvapH = 5.56 kJ/mol Specific heat capacity of N2(g) = 29.2 J mol-1 K-1 Specific heat capacity of N2(l) = 56.04 J mol-1 K-1 Boiling point of N2 = 77.355 K What is the energy in the form of heat released when 450 grams of nitrogen gas at 23.0 °C is converted to liquid nitrogen at -200.0 °C? Select one: a. 364 kJ b. 196 kJ c. 392 kJ d. 17.1 kJ

Suppose that 300.0 J of heat is transferred by conduction from a heat reservoir at a...

Suppose that 300.0 J of heat is transferred by conduction from a heat reservoir at a temperature of 415.0 K to another reservoir. Calculate the entropy change if the temperature of the second reservoir is 100.0 K

How much heat is needed to convert 888 g of ice at -30°C to steam at...

How much heat is needed to convert 888 g of ice at -30°C to steam at 136°C? (The specific heats of ice, steam, and liquid are 2.03 J/g · °C, 1.99 J/g · °C, and 4.18 J/g·°C, respectively. The heat of fusion is 6.02 kJ/mol and heat of vaporization is 40.79 kJ/mol.) ________ kJ

how much heat (in kj) is needed to convert 866 g of ice at -10 c...

how much heat (in kj) is needed to convert 866 g of ice at -10 c to steam at 126 c? spH of ice and steam are 2.03J/g*c and 1.99J/g*c, respectively.

How much heat is needed to convert 889 g of ice at -10°C to steam at...

How much heat is needed to convert 889 g of ice at -10°C to steam at 136°C? (The specific heats of ice, steam, and liquid are 2.03 J/g·°C, 1.99 J/g·°C, and 4.18 J/g·°C, respectively. The heat of fusion is 6.02 kJ/mol and heat of vaporization is 40.79 kJ/mol.) kJ

Question