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.
The heat of combustion of CH4 is 890.4 kJ/mol and the heat capacity of H2O is...
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.
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
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
The experimentally determined heat of combustion of methane is 50.1 kJ/g. Calculate the heat of combustion of methane in kJ/mol. Molar mass of methane CH4 = 16 g/mol CH4(g) + 2 O2(g) → CO2 (g) + 2 H2O(l)
34 kJ of heat was added to 6.5 moles of solid H2O at –27 oC. What will be the final temperature of the H2O? The molar heat capacity of H2O (s) is 37.8 J mol–1 oC–1, and the molar heat capacity of H2O (l) is 75.2 J mol–1 oC–1. The heat of fusion of water is 6.03 kJ mol–1.
The heat of combustion of liquid cumene (C9H12) is -5215.5 kJ/mol at 1 atm and 298 K a) What is the energy of combustion at 1 atm and 298 K? Ecomb = kJ/mol b) Use Thermodynamic Properties to determine its heat of formation. Hf = kJ/mol
5) How much heat is required to convert 0.05kg of water at 298 K to super-steam at 423 K. The boiling point of water is 373 K. Cm [H2O (l)] = 75.4 J/(mol. ℃) Cm [H2O (g)] = 33.6 J/(mol. ℃) ΔHvap = 40.67 75.4 J/mol
1. Calculate the amount of heat (q) produced by the combustion of 4.05 g CH4 (ΔHcomb = -890.4 kJ/mol). 2. Construct a table listing all the data and values you will need to record or find to calculate the specific heat of a single Vienna sausage. Be sure to indicate whether you will need to measure these values or find them from another source. Also make sure you leave enough space for recording these values (with units!) (HINT: Remember q...