How much ice (in grams) would have to melt to lower the temperature of 352 mL of water from 25 x1fC to 5 x1fC? (Assume the density of water is 1.0 g>mL.)
Added by Bill F.
Step 1
Given that the temperature change is from 25°C to 5°C, the heat required is: Q = 352 mL * 4.18 J/g°C * (25°C - 5°C) Q = 352 g * 4.18 J/g°C * 20°C Q = 29552 J Show more…
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How much ice (in grams) would have to melt to lower the temperature of 352 mL of water from $25^{\circ} \mathrm{C}$ to $5^{\circ} \mathrm{C} ?$ (Assume the density of water is 1.0 $\mathrm{g} / \mathrm{mL.} )$
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