You want to quickly set up a temporary water bath in your lab with a volume of 10.0 L and a temperature of 37.0 °C. You only have hot water from your hot water faucet (temperature = 52.6 °C) and cold water from your cold water faucet (temperature = 22.0 °C). What volume of hot water (in liters) must you mix with cold water to get 10.0 L of 37.0 °C water? Assume the specific heat of the water is 4.184 J/g･K and that the water has a density of 1.00 g/mL.
You want to quickly set up a temporary water bath in your lab with a volume of 10.0 L and a temperature of 37.0 °C. You only have hot water from your hot water faucet (temperature = 52.6 °C) and cold water from your cold water faucet (temperature = 22.0 °C). What volume of hot water (in liters) must you mix with cold water to get 10.0 L of 37.0 °C water? Assume the specific heat of the water is 4.184 J/g･K and that the water has a density of 1.00 g/mL.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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You want to quickly set up a temporary water bath in your lab with a volume of 10.0 L and a temperature of 37.0 °C. You only have hot water from your hot water faucet (temperature = 52.6 °C) and cold water from your cold water faucet (temperature = 22.0 °C). What volume of hot water (in liters) must you mix with cold water to get 10.0 L of 37.0 °C water? Assume the specific heat of the water is 4.184 J/g･K and that the water has a density of 1.00 g/mL.
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Step 1: Law of conservation of energy!
VIEWStep 2: Calculation for total mass of water required!
VIEWStep 3: Calculation for heat lost by hot water!
VIEWStep 4: Calculation for heat gained by cold water!
VIEWStep 5: Calculation for unknown y
VIEWStep 6: Calculation for volume of hot water required!
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