Which expression gives the mass, in g, of ethanol required to produce 683.5 kJ of heat upon complete combustion?(Mr for ethanol = 46.0, ΔHθc=−1367 kJmol−1Δ𝐻𝑐𝜃=−1367 kJmol−1)A.     683.51367×46.0683.51367×46.0B.     1367683.5×46.01367683.5×46.0C.     683.5×46.01367683.5×46.01367D.     1367×46.0683.51367×46.0683.5

What mass of ethanol will release 410.0 J of heat when it cools from 32.2°C to 19.1°C? The specific heat of ethanol is 2.44 J/g°C. a 76.4 g b 12.8 g c 31.3 g d 7.49 g

Calculate the energy required to heat 795.0mg of ethanol from −2.4°C to 14.6°C. Assume the specific heat capacity of ethanol under these conditions is ·2.44J·g−1K−1 . Be sure your answer has the correct number of significant digits.

For combustion of ethanol C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l), the amount of heat produced as measured in bomb calormeter, is 1364.47 kJ/mol at 25°C. Assuming all gases are behaving ideally, the enthalpy of combustion ΔCH, for ethanol will be : (R = 8.314 kJ/mol)

At constant pressure, the combustion of 5.00 g of C2H6(g) releases 259 kJ of heat. What is ΔH for the reaction given below? 2 C2H6(g) + 7 O2(g)–> 4 CO2(g) + 6 H2O(l). Hint: Convert 5.0 grams to moles (divide by molar mass).  Divide 259 kJ by your answer to get kJ/mole reacted.  Next, multiply by 2 since there are 2 C2H6(g) in the balanced reaction. Group of answer choices1800 kJ3108 kJ5168 kJ2155 kJ

For the combustion reaction of ethanolCH3CH2OH(l)  +  3 O2(g)  →  2 CO2(g)  +  3 H2O(l)     ΔH  =  - 1368 kJ / mol CH3CH2OHchoose the correct energy profile: