Heat removed from the engine = mass of water * Specific heat of water* temperature difference
since specific heat is given in J/kmol. water mass of water need to be converted to molees
moles= mass/Molecular weight
moles of water = 10 kg/18= 0.556 kg mokes
Heat removed= 0.556 kg moles* 75.2 J/kmol* (373-293)=3345 Joules
A 10.0 kg sample of liquid water is used to cool an engine. Calculate the heat...
Liquid sodium is being considered as an engine coolant. How many grams of liquid sodium (minimum) are needed to absorb 3.30 MJ of energy in the form of heat if the temperature of the sodium is not to increase by more than 10.0 °C? Use Cp = 30.8 J/(K · mol) for Na(l) at 500 K. mass of Na(l): g
Given that the heat of fusion of water is -6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -13 ∘C.
Given that the heat of fusion of water is 6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J>mol · K, and that the heat capacity of H2O(s) is 37.7 J/mol · K, calculate the heat of fusion of water at – 10 °C.
Given that the heat of fusion of water is +6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -14 ∘C.
The heat of combustion of CH4 is 890.4 kJ/mol and the heat capacity of H2O is 75.2 J/mol×K. Part A Find the volume of methane measured at 298 K and 1.91 atm required to convert 1.17 L of water at 298 K to water vapor at 373 K.
Given that the heat of fusion of water is +6.02 kJ/mol, that the heat capacity of H2O(l) is 75.2 J/mol⋅K and that the heat capacity of H2O(s) is 37.7 J/mol⋅K, calculate the heat of fusion of water at -15 ∘C. Express your answer using two significant figures. deltaH= ___?____ kJ/mol
1) When 1336 J1336 J of heat energy is added to 47.6 g47.6 g of hexane, C6H14,C6H14, the temperature increases by 12.4 ∘C.12.4 ∘C. Calculate the molar heat capacity of C6H14. 2) Liquid sodium is being considered as an engine coolant. How many grams of liquid sodium (minimum) are needed to absorb 9.20 MJ9.20 MJ of energy in the form of heat if the temperature of the sodium is not to increase by more than 10.0 °C?10.0 °C? Use CP=30.8...
Calculate the amount of heat needed to transform, under standard conditions, 1.0 mol of liquid methanol at 273 K to 1.0 mol of methanol vapor at 373 K. Assume that Cp,m for liquid methanol and for methanol vapor are independent of temperature. (Enthalpy of vaporization of methanol 35.3 KJ/mol-1, Cp,m of methanol 81.6 JK-1/mol)
eral Chemistry 4th Edition University Science Books Liquid sodium is being considered as an engine coolant. How many needed to absorb 5.40 MJ of energy (in the form of heat) if the temperature of the sodium is not to increase by more than 10.0 "C? Use Cp 30.8 J/(K mol) for Na() at 500 K grams of liquid sodium (minimum) are Number
Liquid sodium is being considered as an engine coolant. How many grams of liquid sodium (minimum) are needed to absorb 9.10 MJ of energy in the form of heat if the temperature of the sodium is not to increase by more than 10.0 °C? Use ?P=30.8 J/(K⋅mol) for Na(l) at 500 K.