Copy of Speent/d/1x04x_GDcrqdfD6R-r8-Pxn3rXs2vicUh-H7MN4NWds0/edit?pli.100%Normal textArlal Narrow1.Specific Heat/Calorimetry/Reaction Energyq = m-C-ATCalculating Heat Evolved or Absorbed1. The temperature of 13.5g of water increased from 15.0°C to 37.0°C.How much heat was absorbed by the water?2. The temperature of 15.5g of ethanol decreased from 27.5°C to 15.5°CHow much heat was released from the ethanol?3. A7.5g mass of pure silver absorbed 175J of heat.What was the final temperature of the silver if the initial temperature wa4. A nugget of pure gold absorbed 276 J of heat. Its temperature rose fromWhat was the mass of the gold nugget?

“Since you have asked multiple questions, we will solve the first question for you. If you want any…

Answered: 1. The temperature of 13.5g of water…

Science

Chemistry

1. The temperature of 13.5g of water increased from 15.0°C to 37.0°C. How much heat was absorbed by the water?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 52E: Before the introduction of chlorofluorocarbons, sulfur dioxide (enthalpy of vaporization, 6.00...

See similar textbooks

Related questions

Q: Consider the chemical equation 2 A + 3 B ---> 4 C + D The reaction enthalpy is 705 kJ How many…

Q: The number of Calories in food items were originally determined by combusting the food, and…

A: Mass of banana used = 115 g Volume of water taken = 850.0 mL Increase in temperature of water =…

Q: The temperature of a 5.0 g sample of Aluminum increases from 25°C to 30°C. How many joules of heat…

Q: How much would the temperature of 295 g of water increase if 17.4 kJ of heat were added? (the…

Q: A gas in a closed container is heated, causing the lid of the container to rise. The gas performs 3J…

A: Given: work done ( w) = - 3 J Internal energy change ( ∆U ) = + 15 J Heat absorbed ( q ) = ? By…

Q: A substance increases in temperature by 255°C when a 983g sample of it absorbs 83,200J of heat.…

Q: The complete combustion of a small wooden match produces approximately 512 cal of heat. How many…

A: Given, The approximate amount of heat produced by the combustion of a small wooden match = 512 cal…

Q: = 378g d. The specific heat of the resulting solution is 3.87 J/g °C. If the temperature change was…

A: Heat absorbed by the solution = mass × temperature change × Specific heat capacity

Q: A sample of 23.2 g of ammonium nitrate, NH¼NO3, was dissolved in 137.5 g of water in a coffee cup…

Q: Determine the heat capacity of 20.0 g of water. The specific heat of water is 4.184 J/g °C

A: Given Mass of water m=20g Specific heat capacity S= 4.184 Jg-1 °C-1

Q: How much heat is required to raise the temperature of a sample of copper from 0°C to 55° C, if the…

A: Given that : Mass (m) = 67 g Change in temperature ∆T = 55°C - 0°C = 55°C Specific heat of copper…

Q: How much heat is needed to raise the temperature of 100.0 g of water from 30.0°C to 100.0°C?

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

Q: If 75.0 grams of water is heated from 32.6°C to 78.9°C, how many kilojoules of heat does the water…

A: Given - - > Mass, m = 75 g Initial temperature, T1 = 32.6°C Final temperature, T2 = 78.9°C…

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: What is heat? How does heat differ from thermal energy? Under what conditions is heat transferred…

Q: From the given chemical equation, solve for the heat evolved (in kJ) when 78.96 g of carbon dioxide…

A: Number of mols = weight/ molecular weight

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: How much heat is released when 4.50 g of methane gas is burned in a constant-pressure system?

A: Given: Mass of methane = 4.50g To find: The amount of heat released

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: How much heat is evolved when 453.5 g of ammonia (NH3) is produced according to the following…

A: Given Reaction is - N2 (g) + 3H2 (g) → 2NH3 (g) ΔH= -91.8 kJ

Q: If two objects, A and B, of different temperature come into direct contact, what is the relationship…

Q: When a 1.25 kg sample of water was heated in a kettle, its temperature increased from 16.4°C to…

A: Given: Mass of water = 1.25 Kg = 1250 g. (Since 1 Kg = 1000…

Q: How much heat is needed to raise the temperature of 13.0g of iron from 19.00C to 100.00 °C? The…

A: Please note- As per our company guidelines we are supposed to answer only one question. Kindly…

Q: 2. In order to produce 972 kJ of heat, how many grams of H2 must react? 2 H2 (g) + 02 (g) → 2 H20…

Q: 4. A 17.1-gram sample of Iron increases temperature from 25.0 °C to 110.0 °C. How much heat is…

A: The amount of Heat absorbed by the Iron can be calculated as -

Q: Quantity Mass of can (g) 12.695 mass of can and water (g) 125.129 Initial mass of food sample (g)…

Q: A metal object with a mass of 19 g is heated to 96°C and is transferred to a calorimeter containing…

A: Given data: The mass of metal = 19 g. The temperature of the metal = 96°C. The mass of water = 75…

Q: 1. How much work was done when 46 kJ of energy was spent on compressing a gas as it released 28 kJ…

Q: Consider the following reaction: N2(g)+O2(g)⟶2NO(g) ΔH∘=182.6kJ How…

Q: N2(g) + 3 H2(g) → 2 NH3(g); ΔH = −91.8 kJ How much heat is released when 1.521 ✕ 104 grams of…

A: Step 1: Here, for the given process, the heat released in formation of 2 moles of ammonia is given…

Q: Aluminum has a specific heat of 0.902 J/goC. How much heat is gained when a piece of aluminum with a…

Q: What is the specific heat of a 75.01 g piece of an unknown metal that exhibits a 45.2°C temperature…

A: Given : Mass of metal = 75.01 g Change in temperature of metal = 45.2 °C And the total heat absorbed…

Q: A 534.2 g sample of water is subjected to a temperature change of -67.86 °C. The specific heat…

A: Given, Mass of water in g = 534.2 g Change in temperature = ΔT = -67.86 0C Specific heat capacity…

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: Given that 154.81 g of solution increased in temperature by 4.82 °C, how much heat, in J, was gained…

Q: What is the specific heat of a 72.01 g piece of an unknown metal that exhibits a 45.2°C temperature…

A: Given data is mass of sample = 72.01 g Temperature = 45.2 oC Heat absorbed = 1870 J Formula used…

Q: Iron reacts with oxygen to form one mole iron (III) oxide releasing 826 kJ of heat. How much heat is…

Q: A 120 gram sample of gold absorbs absorbs 1.2 kJ of heat. How many much does the temperature of the…

A: Given: Mass of the sample= 120 g Heat absorbed= 1.2 kJ Specific heat capacity of gold= 0.129 To…

Q: A system receives 525 J of heat from its surroundings and delivers 465 J of work to its…

Q: How much heat (J) can be absorbed by 1.500 kg of water and have the temperature of the water…

A: Given Mass of water = 1.500 kg temperature increase ΔT = 2.0°C

Q: When 1.75 g of CaCl2 dissolves in 125 g of water in a coffee-cup calorimeter, the temperature…

Q: How much heat is required to raise the temperature of 25g of water from 25.0°C to 30.0°C? The…

A: Mass of water, m = 25 g Specific heat of water, Cs = 4.184 J/g °C Initial Temperature, Ti = 25 °C…

Q: A 1.00g sample of octane is burned in a calorimeter that contains 1.20kg of water. The temperature…

Q: How much heat (kJ) is released by a 200-gram piece of silver as it cools from 1023°C to 300°C?

A: Given :- Mass of piece of silver (m) = 200 g Initial temperature (T1) = 1023°C Final temperature…

Q: The air in an inflated balloon (defined as the system) is warmed over a toaster and absorbs 110 J of…

A: Given that : Heat absorbed by the balloon = 110 J Work done by the balloon = 79 kJ We have to…

Q: 11) q of combustion of the food sample equals a) q absorbed by the calorimeter -q absorbed by the…

A: We have given that 11) q of combustion of the food sample equals a) q absorbed by the calorimeter…

Q: 1.What is the specific heat of a metal whose mass is 94.5 g if the temperature changes from 250° to…

A: The heat required to raise the temperature of a sample of mass 'm' having specific heat 'c' from T1…

Q: What is the specific heat of a 91.51 g piece of an unknown metal that exhibits a 45.2°C temperature…

A: Given temperature of the piece of metal (T) = 45.2°C Given mass of the piece of the metal (m) =…

Q: A piece of copper alloy with a mass of 85.0g is heated from 30.0°C to 45.0°C. In the process, it…

A: To solve this problem we will use the formula Q = m • C • ∆T Where, Q = heat absorbed m = mass…

Q: A 8.17 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

A: Mass of salt sample = 8.17 g Mass of water = 150 g Total mass of solution ( m ) = 8.17 g + 150 g =…

Question

Copy of Spe
ent/d/1x04x_GDcrqdfD6R-r8-Pxn3rXs2vicUh-H7MN4NWds0/edit?pli.
100%
Normal text
Arlal Narrow
1.
Specific Heat/Calorimetry/Reaction Energy
q = m-C-AT
Calculating Heat Evolved or Absorbed
1. The temperature of 13.5g of water increased from 15.0°C to 37.0°C.
How much heat was absorbed by the water?
2. The temperature of 15.5g of ethanol decreased from 27.5°C to 15.5°C
How much heat was released from the ethanol?
3. A7.5g mass of pure silver absorbed 175J of heat.
What was the final temperature of the silver if the initial temperature wa
4. A nugget of pure gold absorbed 276 J of heat. Its temperature rose from
What was the mass of the gold nugget?

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

Trending now

This is a popular solution!

Step by step

Solved in 2 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

The specific heat of an unknown liquid is determined using a sample of molybdenum (Mo) with a mass of 35.12g. The Mo is heated to 99.2OC in boiling water, and then transferred to 52.16g of unknown liquid whose temperature is 23.4OC. The final temperature of the Mo-unknown liquid system is 28.9OC. Calculate the specific heat of the unknown liquid. CMo = 0.251 J•g-1•OC-1
The specific heat of compound AB(s) was determined using coffee-cup calorimeter. When 1.750 g of AB(s) was mixed with 15.00 mL deionized distilled water at room temperature, only 0.850 grams of the compound was dissolved. The temperature of the heterogenous mixture was decreased by 1.70K.Prior to this, the calorimeter was calibrated using a 15mL aqueous reaction mixture that initially contains 0.070 moles each of HBr and KOH. The recorded ΔT is +5.75K. Note: H+(aq) + OH -(aq) → H2O(l) ΔH = -55.85 kJ/molAB(s) ⇌ A+(aq) + B-(aq) ΔH = 88.75 kJ/molspecific heat (H2O) = 4.184 J/g°CMM of AB = 65 g/mol What is the specific heat of solid AB compound (in J/g°C)?
4.38 g of a gas (28.1 g mol–1) was dissolved in liquid water in a calorimeter with a calorimeter constant of 76.0 J K–1. Prior to mixing everything was equilibrated to 21.2 °C. The resulting solution with a mass of 23.4 g was observed to be at a temperature of -6.8 °C and have a specific heat capacity of 4.61 J g–1 K–1. Determine q per mole for this dissolution process. a. -5150 J/mol b. -1.94 × 104 J/mol c. 2.89 × 105 J/mol d. -3.39 × 105 J/mol e. 3.30 × 104 J/mol
Determination of enthalpy of neutalisation Ccal=20 J/°C Volume of HCl = 150 ml Initial temperature of HCl = 30 °C Volume of NaOH = 149 ml Initial temperature of NaOH = 30 ° C Final Solution Temperature = 45 °C Moles of H+ = .220 mol Moles of OH- = .221 mol Limitng reagent = OH- Heat transfer of solution = ___________|Kj Enthalpy of neutralisation per mole of limiting reagent = _____________________|kj/ mol
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 68.5 mL water (where X is a hypothetical metal): X + 2 HCI ---> XCI2 + H2 In this process, the water temperature rose from 25.0 °C to 33.3 °C. If 0.00629 mol of "X" was consumed during the reaction, what is ?rH of this reaction in kJ mol^-1with respect to "X"? The specific heat of water is 4.184 J g-¹ °C-¹
1. Calculate the standard enthalpy of formation of C10H10. Its standard enthalpy of combustion is shown by the equation: 2C10H10 (l) + 25O2 (g) → 20CO2 (g) + 10H2O (l) ∆H = 10,314 KJ/mol The standard heat of formation (KJ/mol) at 298.15oC : CO2 = -393.5 ; H2O(l) = -285.8 2. Determine ΔG° at 298.15K for the reaction: 4Fe (s) + 3O2 (g) → 2Fe2O3 (s) Given that ΔH° = -1648 kJ ; ΔS° = -549.3 J/K 3. In the picture, Find the the ∆H°rxn if ∆G°rxn is 420 kJ/mol and ∆S°rxn is -143 J/mol*k
A student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = J
A student was asked to determine the enthalpy of solution of KclO3 in water using Styrofoam calorimetry. Calibration was performed by mixing 8.00 mL 0.050 M HCI with 2.00 mL 0.200 M NaOH. The neutralization reaction (AH = -55.85 kJ/mol) was accompanied by a temperature change from 25.0 to 28.3°C. Using the same calorimeter, 0.300 g KCIO3 (MW: 122.55) was dissolved in water and the temperature was observed to change from 23.6 to 17.3°C. (Assume that the total volume of the mixture in calibration is the same in the enthalpy measurement) What is the calorimeter constant in kJ/°C? What is the enthalpy of dissolution of KCIO3 in kJ/mol?
To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of the material was supplied with 35.548 J of heat causing the temperature of the material to rise from 297.05 K to 461.4 K. What is the specific heat of this material? Report your answer in units of J/(ºC · g) to 4 sig figs, but do NOT include units in your answer.
Estimate the thermal properties of a food with the following composition: carbohydrate 0.3%, protein 27.6%, fat 17.5%, ash 4.7%, moisture 49.9%. a. Specific heat is based on the Siebel equation = kJ / kg ° C. b. Specific heat is based on the Charm equation = kJ / kg ° C. c. Specific heat is based on the Heldman & Singh equation = kJ / kg ° C. d. Specific heat is based on the Choi & Okos equation = kJ / kg ° C. e. Heat conductivity is based on the equation Sweat = W / m ° C. f. Heat conductivity is based on the Choi & Okos equation = W / m ° C. g. Heat diffusivity based on the Choi & Okos equation = m² / s.
At constant pressure and 25^C, What is delta H for the following reaction. 2C2H6(g) + 7O2(g) = 4CO2(g) + H2O(l) if the complete consumption of 38.2 g of C2H6 libraties 1981 KJ of heat energy?
A pellet of benzoic acid standard was combusted in a bomb calorimeter to determine the experimental calorimeter constant. After 6 mins of monitoring the temperature, the bomb was fired. The following data were obtained. mole of benzoic acid: 0.0049 mol mass of burnt fuse wire: 0.0125 g qwire,surr: 5858 J/g ΔHcombustion of benzoic acid: -3228.0 kJ/mol Δng (combustion of benzoic acid): -0.5 mol R: 8.314 J/mol•K r1: 0ºC/min r2: 0ºC/min Tf: 30.4ºC Ti: 28.4ºC Determine the calorimeter constant (in J/ºC). Report your answer in 2 decimal places.