If 1.45 l of water is initially at 25.0 c, what will its temperature be after absorption of 9.4 x 10^-2kwh of heat?

Fisrt let you must know the heat capacit of water Cp which is equal to 4.184 J/ g C
then convert kWh to J9.4 X 10^-2kWh= 9.4 X 10^-2kJh/s( 3600 s / 1 hr) ( 1000 J / 1 kJ)
= 338400 Jthe formulaH = mCpdeltaTwhere H is the heatm is the massCp is the heat capacitydelta T is the change in temperature
so338400 J = (1.45 L) ( 1000 g / L) (4.184 J/ g C) deltaTsolve for DeltaT
deltaT = 55.78 Cso the new TT = 55.78 C + 25 CT = 80.78 C

Answer) by studying proton collisions hope this : )