How much heat, in joules and calories, is needed to heat up 253 mL of water from 13.3 °C to 85.2 °C? Assume the density of water to be 1.00 g/mL.
How much heat, in joules and calories, is needed to heat up 253 mL of water from 13.3 °C to 85.2 °C? Assume the density of water to be 1.00 g/mL.
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter15: Energy And Chemical Change
Section: Chapter Questions
Problem 76A: How much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?
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How much heat, in joules and calories, is needed to heat up 253 mL of water from 13.3 °C to 85.2 °C? Assume the density of water to be 1.00 g/mL.
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Step 1
Given : Volume of water = 253 mL
Density of water = 1.00 g/mL
Initial temperature of water = 13.3 °C
And final temperature of water = 85.2 °C
Since mass = density X volume
=> mass of water = 1.00 X 253 = 253 g
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