**Experiment Preparation: Water Bath Temperature Problem**A biology experiment requires the preparation of a water bath at 37.0°C (body temperature). The temperature of the cold tap water is 22.0°C, and the temperature of the hot tap water is 55.0°C. If a student starts with 90.0 g of cold water, what mass of hot water must be added to reach 37.0°C?**Concept Explanation:**This problem involves the concept of mixing water at different temperatures to achieve a desired final temperature. To solve this, we can use the principle of heat transfer, where the heat lost by the hot water will equal the heat gained by the cold water until thermal equilibrium is reached.---Note: This explanation is general and does not involve detailed calculations.

The system heat lost or gained will be equivalent to the mathematical product of the species mass…

A biology experiment requires the preparation of a water bath at 37.0°C (body temperature). The temperature of the cold tap water is 22.0°C, and the temperature of the hot tap water is 55.0°C. If a student starts with 90.0. g of cold water, what mass of hot water must be added to reach 37.0°C?

A biology experiment requires the preparation of a water bath at 37.0°C (body temperature). The temperature of the cold tap water is 22.0°C, and the temperature of the hot tap water is 55.0°C. If a student starts with 90.0. g of cold water, what mass of hot water must be added to reach 37.0°C?

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...

See similar textbooks

Related questions

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 378.0 mg sample…

A: mass = 378.0mg = 0.378g Initial Temperature = 30.4oC Final Temperature = 43.1oC Heat required = 20.1…

Q: Calculate the heat that must be supplied to a 500.0 g stainless steel vessel containing 450.0 g of…

A: The specific heat can be defined as the amount of heat per unit mass that is needed to raise the…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 0.85 kg sample…

A: Given: Mass of sample = 0.85 Kg = 850 g (Since 1 Kg = 1000 g) Initial…

Q: A 124.5 g sample of an unknown metal absorbs 1276.25 J of heat, upon which the temperature of the…

A: Given: The mass of the metal sample = 124.5 g The amount of heat absorbed by the metal = 1276.25 J…

Q: A 55.2 g piece of metal has a temperature of 90.4 °C before being placed into 102.5 g of water at…

Q: In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a…

A: The heat is related to mass, temperature change, and specific heat of a substance as: q=mc∆T

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 333.0 g sample…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 273.0 g sample…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 165.0 g sample…

A: We have been given initial temperature, final temperature, mass of sample and heat required to raise…

Q: How much energy as heat is required to raise the temperature of 50.00 mL of water from 25.55 °C to…

A: Given data Initial temperature of water, T1 = 25.55 °C Final temperature of water, T2 = 28.22 °C…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.87 kg sample…

Q: A sample of iron absorbs 62.3 J of heat, upon which the temperature of the sample increases from…

A: The amount of heat required is related to specific heat capacity as,…

Q: A chunk of lead at 91.7°C was added to 200.0 g of water at 15.5°C. The specific heat of lead is…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 196.0 g sample…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.04 kg sample…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 112.0 g sample…

A: Using the relation Q=mSΔT we can find specific heat capacity of substance.Where, Q= heatS= heat…

Q: A piece of metal was placed into a 75.00 grams of water. The temperature of the water increased from…

A: Given , mass of water = 75.00 g Initial temperature Ti= 22.02°C Final temperature, Tf = 25.04°C…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 671.0 mg sample…

Q: What is the specific heat of aluminum if the temperature of a 28.4 g sample of aluminum is increased…

A: The specific heat of a substance is defined as the amount of heat required to raise the temperature…

Q: hemist carefully measures the amount of heat needed to raise the temperature of a 886.0 mg sample of…

A: Specific heat capacity is amount of heat needed to increase one gram of substance by one degree

Q: The temperature of a brass bar by 10.0°C when it absorbs 2.00kJ of energy by heat. The mass of the…

Q: In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a…

Q: When 514 J of heat is added to a sample of liquid water, the temperature rises from 27.8°C to…

A: Specific heat capacity is the amount of heat needed to raise the temperature(usually 1°C) of given…

Q: On a mountaineering expedition, a climber heats water from 0°C to 50°C. Calculate the mass of water…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 1.82 kg sample…

A: Answer: Whenever a substance absorbs the heat, its temperature rises but the magnitude of that…

Q: ● A 156.0 g sample of a metal at 75.0°C is placed in 144.6 g of water at 20.0 °C. The temperature of…

A: Given that :Mass of metal (ms) is 156.0 gInitial temperature of metal is 75.0 °CMass of water(mw) is…

Q: A chunk of lead at 91.7°C was added to 400.0 g of water at 15.5°C. The specific heat of lead is…

A: Just apply Heat given = Heat taken

Q: What is the mass of an iron piece that cools from 57.8 °C to 26.4°C while releasing 7160.2 J of…

A: The working formula for this problem would be, q = m x Cp x dTwhere q is the total heat, m is the…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 693.0 g sample…

A: given, the mass of the sample = 693.0 g the temperature rises from initial temperature, T1 = 17.1 oC…

Q: A solution is made by mixing 197.3 g of ethanol initially at 10.5°C with 250.0 g of water initially…

A: We know that, according to the law of conservation of heat energy, energy gained or loss by the…

Q: What is the mass of an iron piece that cools from 50.2 °C to 27.8°C while releasing 351.7 J of heat?…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 631.0 g sample…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 206.0mg sample…

A: Given : Mass of sample = 206 mg = 0.206 g…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 663.0 mg sample…

A: Given Mass = 663 mg = 663 x 10-3 g Heat = 12.8 J T1 = 0°C T2 = 21.4°C

Q: When immersed in water, the temperature of a 102.1 gram sample of metal changes from 150.2 0C to…

Q: In the laboratory a student finds that it takes 54.9 Joules to increase the temperature of 11.0…

Q: How much energy would it take to heat a section of the copper tubing that weighs about 595.0 g ,…

Q: A 1401 kg1401 kg car is traveling down the road at 85.8 km/h.85.8 km/h. While traveling at this rate…

A: The kinetic energy of the vehicle in kilojoules is ≈ 398 kJ

Q: When 156 g of water at a temperature of 22.5°C is mixed with 65.1 g of water at an unknown…

A: This is a question from mixing of substances.

Q: The temperature of an object increases by 44.1 °C when it absorbs 3761 J of heat. The mass of the…

A: Q= mcΔT ……………………1 Where Q represents heat M represents mass of the system C denotes heat capacity ΔT…

Q: In the laboratory a student uses a "coffee cup" calorimeter to determine the specific heat of a…

Q: 55.0 g sample of nickel (specific heat = 0.433 J/g°C) at 100.0°C is added to 65.0 g of water at…

Q: If a 42.0g piece of steel at 75.0 degrees C is placed in 150.0 g of water at 25.5 degrees C, what is…

Q: A chemist carefully measures the amount of heat needed to raise the temperature of a 339.0 g sample…

Question

**Experiment Preparation: Water Bath Temperature Problem**

A biology experiment requires the preparation of a water bath at 37.0°C (body temperature). The temperature of the cold tap water is 22.0°C, and the temperature of the hot tap water is 55.0°C. If a student starts with 90.0 g of cold water, what mass of hot water must be added to reach 37.0°C?

**Concept Explanation:**

This problem involves the concept of mixing water at different temperatures to achieve a desired final temperature. To solve this, we can use the principle of heat transfer, where the heat lost by the hot water will equal the heat gained by the cold water until thermal equilibrium is reached.

---

Note: This explanation is general and does not involve detailed calculations.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A chemist carefully measures the amount of heat needed to raise the temperature of a 744.0 mg sample of a pure substance from -7.8 °C to 12.8 °C. The experiment shows that 3.60 J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
A chemist carefully measures the amount of heat needed to raise the temperature of a 506.0 g sample of a pure substance from -2.4 °C to 21.6 °C. The experiment shows that 29.6 kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
A chemist carefully measures the amount of heat needed to raise the temperature of a 1.45 kg sample of a pure substance from 36.3 °C to 56.3 °C. The experiment shows that 121. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Be sure your answer has the correct number of significant digits.
Which of the reactions are exothermic? 2 Mg(s) + O,(g) → 2 MgO(s) + heat O NH, (g) + HCI(g) → NH,CI(s) + heat AgCl(s) + heat – Ag*(aq) + Cl¯(aq) 2 Fe, 0, (s) + 3 C(s) + heat → 4Fe(s) + 3 CO, (g) O C(graphite) + 0,(g) → CO,(g) + heat O CH, (g) + 20,(g) → CO,(g) + 2 H,O(1) + heat
The specific heat capacity of silver is 0.2386 J/g °C. Assuming no loss of heat to the surroundings or to the calorimeter, determine the final temperature when 100.0 g of silver at 40.0°C is immersed in 60.0 g of water at 10.0°C.
It takes 47.0 J to raise the temperature of an 9.90 g piece of unknown metal from 13.0°C to 24.6 °C. What is the specific heat for the metal? Express your answer with the appropriate units.
The temperature of the cooling water as it leaves the hot engine of an automobile is 240 °F. After it passes through the radiator it has a temperature of 175 °F. Calculate the amount of heat transferred from the engine to the surroundings by 10 grams of water with a specific heat of 4.184 J/g °C.
A sample of aluminum absorbs 50.1 J of heat, upon which the temperature of the sample increases from 20.0 °C to 35.5 °C. If the specific heat of aluminum is 0.900 A J/g°C, what is the mass of the sample (in grams)?
A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt? How many moles of the unknown salt were used in the reaction ? _______ J?
What mass of water will change its temperature by 10 °C when 975 J of heat is added? The specific heat of water is 4.18 J/g 0C
A chemist carefully measures the amount of heat needed to raise the temperature of a 0.46 kg sample of a pure substance from 36.2 °C to 51.6 °C. The experiment shows that 33. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits.
3. A piece of metal with a mass of 97.6 grams was heated in a steam jacket to 94°C and then plunged into 243.6 grams of water at 21 °C, causing the temperature to rise to 24°C. What is the specific heat of metal? 4. How many cubic feet are there in a room measuring 6m x 10m x 3m?