108. A 25.0-mL sample of ethanol (density initially at 7.0 °C is mixed with 35.0 mL of water (density beaker. Assuming that no heat is lost, what is the final temperature of the mixture? 0.789 g/mL) 1.0 g/mL) initially at 25.3 °C in an insulated 1

108. A 25.0-mL sample of ethanol (density initially at 7.0 °C is mixed with 35.0 mL of water (density beaker. Assuming that no heat is lost, what is the final temperature of the mixture? 0.789 g/mL) 1.0 g/mL) initially at 25.3 °C in an insulated 1

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.45PAE: 9.45 What happens to the temperature of a material as it undergoes an endothermic phase change? If...

See similar textbooks

Related questions

Q: If the specific heat of water is 4.18J/g°C and 325J of heat is added to 56.75g of water, how much…

A: We have to calculate the temperature change when 325 J of heat is added to 56.75 g of water.Specific…

Q: A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample…

Q: When 151.0 mL of water at 26.0 C is mixed with 71.0 mL of water at 85.0 C, what is the final…

Q: A 125-g piece of aluminum (specific heat of 0.900 J/gC) is heated to 95°C and placed into a 375-g…

A: Solution:- Mass (m) of aluminium piece = 125 g Specific heat capacity (ca) of aluminium = 0.900…

Q: A beaker contained 62.09 g of water at 19.6°C. A 86.23-g sample of metal at 75°C was placed in it,…

A: Mass of water = 62.09 g Initial temperature of water = 19.60C Mass of metal = 86.23 g Initial…

Q: A container filled with 7.81 kg of water underwent a temperature change from 24.19 "C to 28.08 °C.…

A: The amount of heat required to one gram of substance to raise the temperature of one degree…

Q: What is the AT of a 48 g piece of copper, after absorbing 328 J of heat. Copper has a specific heat…

A: Specific heat capacity is defined as the quantity of heat absorbed by 1 g of substance to raise the…

Q: A sample of iron was heated to 112.0 °C, then placed into 260 g of water at 22.8 °C. The temperature…

Q: what is the anwser to A student heats a 200 g sample of water from 20oC to 80oC. The specific heat…

A: The answer to the following question is-

Q: 97. How much heat in kilojoules is required to heat 56 L of water from an initial temperature of 85…

A: Volume of water, V = 56 L or 56000 mL Density of water, ρ = 1 g/mL Determine the mass of water, m –…

Q: How much heat is required to warm 1.50 L of water from 25.0°Cto 100.0°C? (Assume a density of 1.00…

A: We can solve this problem by using the following relation: q=m×c×△T Where: q=Heatc=specific heat(…

Q: The table lists the specific heat values of several substances. Substance Specific heat (cal/g.°C)…

A: Heat energy is given by q = m * C * ΔT where q = heat energy m = mass of the substance C = specific…

Q: A 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

A: Specific heat: It is defined as the amount of heat required to raise the temperature of the…

Q: 175 g of water was heated from 15°C to 88°C. How many kilocalories (kcal) of heat were absorbed by…

Q: The specific heat of a 70 g sample is 0.069 J/(g·K). If it absorbs 96 J when it is heated from a…

A: Heat energy required to raise the temperature of body of 1gram of mass to 1°c is known specific…

Q: What would be the final temperature of 1 gallon of water (3.785 L) if you added 1.218 x 103 kJ of…

A: we need to find the final temperature of water under given conditions

Q: A 44.3 g sample of water at 100.00 °C (specific heat of water = 4.184J/g.°C) was placed in an…

Q: A 217.3 g water bath is heated to 99.7 ˚C from 22.5 ˚C. How much heat was absorbed by the water, in…

A: Given, mass of water =217.3 g initial temperature, Ti=22.5 °C final temperature, Tf=99.7°C specific…

Q: A piece of unknown metal weighs 348 g. When the metal piece absorbs 6.64 kJ of heat, its temperature…

A: Given: Mass, m = 348 g Heat, q = 6.64 kJ Tf = 43.6oC Ti = 22.4oC

Q: How do I calculate the specific heat of metal if 1027 joules of energy are needed to raise the…

A: q = m .C . ΔT WHERE heat = q = 1027 J mass of metal = m = 42.9 g specific heat of metal = C =…

Q: A 7.37 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

A: Given, Mass of sample = 7.37 gMass of water = 150 g Mass of solution = 157.37 g Initial temperature…

Q: 12. An aluminum kettle weighs 1.05 kg.(a) What is the heat capacity of the kettle?(b) How much heat…

A: (a) Given that mass of aluminium kettle =1.05 kg = 1050 g Now, heat capacity is explained as the…

Q: 4) You are told that a chemical reaction is exothermic. How could you test whether the statement is…

Q: A 67.4 g piece of titanium (specific heat = 0.523 J/g °C) is heated to 95.8 °C. It is then put in to…

Q: A 248.5 g water bath is heated to 98.2 ˚C from 22.2 ˚C. How much heat was absorbed by the water, in…

A: Specific heat and heat of the Substance are interrelated with each other by - Q = C m ∆T Here, Q =…

Q: 12. An aluminum kettle weighs 1.05 kg. (a) What is the heat capacity of the kettle? (b) How much…

Q: How much energy(in Joules) is required to heat 3.00g of water from 23.0 oC to 100.0 oC?

A: Given data: The mass of water m = 3.00 g. Initial temperature T1 = 23.0°C. Final temperature T2 =…

Q: 1.64 L of hydrochloric acid are mixed with 735 mL of ammonia in a calorimeter. The initial…

A: Solution - According to the question - Given - 1.64 L = 1.64 * 10000 = 1640 ml Total volume = 1640 +…

Q: Directions: Please complete this worksheet on a separate piece of paper. 1. What is the specific…

A: Given : 1. Mass of aluminum = 28.4 gm Heat given = 207 J Increase in temperature = 8.1 ° C 2.…

Q: A 39 g aluminum spoon (specific heat 0.904 J/g-°C) at 25°C is placed in 178 mL (177 g) of coffee at…

A: A definite quantity of heat is used up in raising temperature of substances. For substance that…

Q: If 2.500KJ of heat are added to 50.0g of water at 25.00 °C, what would be the final temperature of…

Q: The specific heat of copper is 0.385 J/g°C. Calculate the final temperature when 25.0 g of copper…

Q: When 126.0 mL of water at 26.0 ° C is mixed with 66.0 mL of water at 85.0 ° C, what is the final…

A: Given are two samples of water. The mass of water in two samples can be calculated as

Q: How many Joules of energy would be required to heat 35g of water from 23C to 29C?

A: Specific heat capacity of a substance can be defined as the amount of energy required to raise…

Q: When 156.0 mL of water at 26.0°C is mixed with 86.0 mL of water at 85.0°C, what is the final…

A: Convert the given mL of water into mass.Given, density of water = 1.00 g/mL

Q: Because water has such a high specific heat capacity, it heats and cools more slowly than land. How…

A: Given that,

Q: The table lists the specific heat values of several substances. Substance Specific heat (cal/g. C)…

A: Specific heat capacity: The amount of heat required to increase the temperature of one gram of a…

Q: 559.4 J of heat was added to 8.00 g of water. The final temperature of the water was measured as…

A: Given: Heat Energy (Q)= 559.4 J Mass of water (m)= 8.00 g Final Temperature (T2) = 64.2 0C Specific…

Q: What is the change in temperature of a 13.6 g sample of water that absorbs 1,524 J of heat?

A: q = mc∆T q is the amount of heat energy absorbed m is the mass of substance c is the specific heat…

Q: How much heat is needed to raise the temperature of a 2.5 g piece of copper wire from 20. °C to 80.…

A: When the temperature rise of a 1 g of substance takes place by 1°C, some amount of heat is required…

Q: he freezing point of mercury is -38.8°C. What quantity of energy, in joules, is released to the…

A: The density of liquid mercury =13.6 g/cm3. The mass of mercury = 1.00 mL × 13.6 = 13.6 g Hg.

Q: -Calorimetry Questions 1. A 24.6 g sample of nickel is heated to 110.0 °C and then placed in a…

Q: A 110.-g sample of copper (specific heat capacity = 0.20 J/°C g) is heated to 82.4°C and then placed…

A: Given : Mass of copper = 110 g Specific heat capacity of copper = 0.20 J/°C.g Initial temperature of…

Q: The temperature of 34.7 g H2O changes from 27 °C to 53 °C. What is the heat associated with this…

Q: A 475-g sample of water absorbs 25.1 kJ of heat. If the initial temperature of water is 19.0oC, what…

A: Given: Mass of water sample(m) = 475 g Heat(q) = 25.1 KJ OR 25100 J Initial temp. (T1) = 19°C…

Q: A 23-g sample dissolved in water absorbs heat, increasing its temperature from 30°C to 45 °C. What…

Q: The density of aluminum is 2.7 g/cm3 and its specific heat is 0.9 J/g.0. A piece of 9.7 cm3 aluminum…

A: Recall the following relation according to law of calorimetry Q=mC×∆tHere Q is amount of…

Q: A 4.8 sample of water starting 56 C loses 448 J of energy in the form of heat. What is the final…

Q: What will be the final temperature when a 25.0 g block of aluminum (initially at 25 °C) absorbs 10.0…

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

Question

108. A 25.0-mL sample of ethanol (density
initially at 7.0 °C is mixed with 35.0 mL of water
(density
beaker. Assuming that no heat is lost, what is the final
temperature of the mixture?
0.789 g/mL)
1.0 g/mL) initially at 25.3 °C in an insulated
1

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

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 steps with 5 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?
If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?
9.95 How much heat is required to convert 250 g of water from liquid at 23°C: into steam at 107°C? (The necessary heat capacities and enthalpy changes can be found in the chapter or online.)
How much heat, in joules and in calories, is required to heat a 28.4-g (1-oz) ice cube from 23.0 C to 1.0 C?
If 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.)
Draw a diagram like Figure 2.11 that illustrates the change in enthalpy for the chemical reaction C s 2H2 g CH4 g Which is exothermic by 74.8 kJ/mol.
9.45 What happens to the temperature of a material as it undergoes an endothermic phase change? If heat is added, how can the temperature behave in this manner?
How much heat is evolved when 1255 g of water condensesto a liquid at 100°C?
What quantity of heat energy would have to be applied to a 25.1 -g block of iron in order to raise the temperature of the iron sample by 17.5 °C? (See Table 10.1.)
When steam condenses to liquid water, 2.26 kJ of heat is released per gram. The heat from 168 g of steam is used to heat a room containing 6.44 104 g of air (20 ft 12 ft 8 ft). The specific heat of air at normal pressure is 1.015 J/(gC). What is the change in air temperature, assuming the heat from the steam is all absorbed by air?
The reaction of 50 mL of acid and 50 mL of base described in Example 5.5 increased the temperature of the solution by 6.9 degrees C. How much would the temperature have increased if loo mL of acid and 100 mL of base had been used in the same calorimeter starting at the same temperature of 22.0 C? Explain your answer.
Equal masses of liquid A, initially at 100C, and liquid B, initially at 50C, are combined in an insulated container. The final temperature of the mixture is 80C. All the heat flow occurs between the two liquids. The two liquids do not react with each other. Is the specific heat of liquid A larger than, equal to, or smaller than the specific heat of liquid B?