How much energy is required to increase the temperature of 36.0 g of h2o from –20 °c to 50 °c, keeping in mind the following: vice ≈ 2.00 j/g×c liquid water ≈ 4.00 j/g×c δhfusion ≈ 6000 j/mol

2.06 x 10⁴ J

Explanation:

The process takes place in three steps. First, the ice is heated from -20 °C to 0 °C. Then the ice undergoes a phase change to water. Finally, the water is heated from 0 °C to 50 °C.

The heat energy required for the first step is as follows:

Q = mcΔT = (36.0 g)(2.00 Jg⁻¹°C⁻¹)(0 °C - (-20 °C)) = 1440 J

The heat energy required for the phase change (where L is the heat of fusion) is then calculated. Grams are converted to moles using the molar weight of water (18.02 g/mol)

Q = ML = (36.0 g)(mol/18.02g)(6000 J/mol) = 11987 J

Finally, the heat energy required to raise the temperature of the water to 50°C is calculated:

Q = mcΔT = (36.0 g)(4.00 Jg⁻¹°C⁻¹)(50 °C - 0 °C) = 7200 J

Adding all of the heat energy values together gives:

(1440 + 11987 + 7200) J = 20627 J

The final answer is 2.06 x 10⁴ J

the total distance that martina travels that day is

(distance from home to mom's office) plus (distance from mom's office to school)

plus (distance from school to library) plus (distance from library to friend's house)

plus (distance from friend's house to martina's house).

(we don't know what any of these distance actually is.)