How much energy in kJ must be absorbed to heat up a volume of ocean water 2 m high by 20 km wide by 30 km deep by 3°C? (The density of sea water is about 1.02 g/mL; it requires about 4.2 J to heat up 1 g of sea water 1 K.) (C = 75.291 J/mol.K for H₂O; q = C_cal$\Delta$T)

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The correct answer is D.The energy required to heat up the water is given by the equation q = CcalΔT, where Ccal is the specific heat capacity of water, ΔT is the change in temperature, and q is the energy required.The specific heat capacity of water is 4.2 J/gK, and the change in temperature is 3°C. The volume of water is 2 m high by 20 km wide by 30 km deep, which is 1.2 x 10^12 m^3. The density of sea water is 1.02 g/mL, so the mass of the water is 1.2 x 10^12 kg.Therefore, the energy required to heat up the water is:q = CcalΔT = (4.2 J/gK)(3°C)(1.2 x 10^12 kg) = 1.5 x 10^13 kJ

How Much Energy in KJ Must Be Absorbed to Heat Δ\DeltaΔ

How Much Energy in KJ Must Be Absorbed to Heat $\Delta$