The heat of combustion of C8H18, is 5509 kJ/mol. What is the heat of combustion of C8H18, in units of kJ/g?   Group of answer choices24.59 kJ/g48.29 KJ/g628475 kJ/g48290 kJ/g

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

A 698 g sample of a substance increases in temperature by 2550C when 32,000 J of energy is added. What is the specific heat of the substance?Group of answer choices125 J/g ºC45.8 J/g ºC0.180 J/g ºC0.296 J/g ºC

A fuel produces 9000 ks of heat when burnt. If thecalorific value of the fuel is 2000 kJ/kg, find theamount of fuel burnt..

Calculate the heat of the following reaction:C6H12O6 → 2C2H5OH + 2CO2Given the following heats of formation:C6H12O6                ΔH°f=  -1260 kJ/molC2H5OH                ΔH°f=  -277.7 kJ/molCO2                      ΔH°f=  -393.5 kJ/molGroup of answer choices-336.1 kJ/mol-1266 kJ/mol-22.6 kJ/mol-82.4 kJ/mol

Given the following enthalpies of formation in kJ/mol:CH4(g) = - 74.8           O3(g) = 143H2O(g) = - 242             CO2(g) = - 394what is the standard heat of reaction in kJ/mol for the reaction below?3 CH4(g) + 4 O3(g) 3 CO2(g) + 6 H2O(g)Question 6Select one:a.(3 x -394   +  6 x -242)   +   ( 3 x -74.8  +   4 x 143) b.(3 x -394   +  6 x -242)   -   ( 3 x 74.8  +   4 x  -143) c.(3 x -394   +  6 x -242)   -   ( 3 x -74.8  +   4 x 143) d.( 3 x -74.8  +   4 x  143)  -  (3 x -394   +  6 x -242)e.( 3 x -74.8  +   4 x  143)  +  (3 x -394   +  6 x -242)