8) If the heat of fusion for water is 80. cal/g, how many calories are needed to melt 45.0 g of ice at 0 °C? A) 0.56 cal B) 80. cal C) 3.6 cal D) 1.8 cal 81 Insimal olgmootesd ir moils ono nimuis E) 3.6 x 103 cal os6.0 (8

8) If the heat of fusion for water is 80. cal/g, how many calories are needed to melt 45.0 g of ice at 0 °C? A) 0.56 cal B) 80. cal C) 3.6 cal D) 1.8 cal 81 Insimal olgmootesd ir moils ono nimuis E) 3.6 x 103 cal os6.0 (8

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: Energy Constants for H2O 334 J/g = Heat of Fusion (Hf) 2260 J/g = Heat of Vaporization (Hv) 2.11…

A: Heat absorbed by the sample is calculated as follows: Heat = Heat required to convert ice to water…

Q: Two 20.0 g ice cubes at -20.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is…

A: In the given question we have to calculate the final temperature in the given conditions.The heat of…

Q: 2. How much heat must be added to 110.0 g of ice at -18.0°C to change it to water at 47.5°C ? (Cice…

A: The following formula is used to calculate the required heat.

Q: 15. Calorimetry a. How much heat needs to be taken from 0.5 kg of ethyl alcohol as a gas at its…

A: Q = mc∆T Q = heat energy (Joules, J), m = mass of a substance (g) c = specific heat (units…

Q: Calculate the heat required to vaporize 102 g of water at a temperature of 100oC if the Heat of…

A: The process of conversion of a substance in its liquid state into its gaseous state is called…

Q: Two 20.0 g ice cubes at -20.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is…

A: Mass of each ice cube = 20.0 gTemperature of each ice cube = -20.0 °CMass of water = 245…

Q: The specific heat of ice is 2.100 kJ/kg °C, the heat of fusion for ice at 0°C is 333.7 kJ/kg, the…

Q: Based on the thermodynamic properties provided for water, determine the energy change when the…

A: Mass of water = 0.350 kg = 350 g Molar mass of water = 18 g/mol Moles of water = 350 g / 18 g/mol =…

Q: The specific heat of ice is 2.10 kJ/kg∙°C, the heat of fusion for ice at 0°C is 333.7 kJ/kg, the…

A: Given : Specific heat of ice = 2.10 KJ /Kg°c Heat of fusion for ice at 0°C = 333.7 kJ/kg specific…

Q: What is the enthalpy change in units of kJ for converting 27.9 grams of water vapor at 112.1 Celsius…

A: Molar mass of water = 18 g/mol Calculation of no. of mol of water:

Q: 5. The normal melting point of water is 0°C the normal boiling point is 100°C. The heat of…

A: Scientists describe heat as thermal energy transmitted between two systems at different temperatures…

Q: What is the enthalpy change during the process in which 100 g of liquid water at 50.0°C is cooled to…

A: Cooling of water from 50°C to 0°C Given: m = 100g ∆t = 0°C - 50°C = -50°C cH2O(l) = 4.184…

Q: How much heat in kilojoules is required to (a) melt and (b) boil 1.50 mol ofisopropanol (rubbing…

A: First convert moles to mass in grams by multiplying with molar mass of isopropyl alcohol 1.5 mol x…

Q: A0 682 mol sample of liquid propanol (60.09 g/mol) is heated from 25.6°C to 322.7°C. The boiling…

Q: ow much heat is required to convert 32.48 g of ice at -7.05 °C into liquid water at 19.36 °C?…

A: Heat involved in a process on increasing temperature = mass of the substance×specific heat…

Q: 12. How much energy is needed to change a 47 g cube of ice from -29 °C to liquid water, at 29 °C?…

Q: How much heat is required to change 256.0 g of water at 58.1 ° C to steam at 100.0 ° C?

A: Given that: Mass of water, mwater = 256.0 g Initial temperature = 58.1⁰C Final temperature = 100.0⁰C…

Q: How much heat is required to change 266.4 g of ice at 0 ° C to water at 0 ° C?

A: The mass of ice is = 266.4 g The temperature of ice is = 0oC The temperature of the water is = 0oC…

Q: the vapor pressure of water at 25 C is 3.13 x 10^-2 atm, and the heat of vaporization of water is 25…

Q: Suppose that 117.2 J of heat energy is required to completely vaporize 4.3 g of a pure liquid. If…

Q: What amount of heat (in kJ) is required to convert 29.9 g of an unknown solid (MM = 67.44 g/mol) at…

A: The objective of the question is to calculate the total amount of heat required to convert a solid…

Q: What is quantity of heat (in KJ) associated with cooling 212.7 g of water from 25.60 C to ice at…

Q: When 4.61 grams of ice at – 20°C have absorbed 2500 calories of heat, what is the temperature of the…

A: Latent heat is the amount of energy that is required by a phase to convert itself from solid to…

Q: What does not correspond to the molar heat of fusion? O AHfus O the heat absorbed by one mole of a…

Q: Ammonia has a normal (1.00 atm) boiling point of -33.3 °C. Under a pressure of 2.00 atm, what is…

A: Clausius-Clapeyron Equation: The Clausius-Clapeyron Equation is used to calculate the vapor pressure…

Q: How much heat energy is required to boil 18.4 g of ammonia, NH3? The molar heat of vaporization of…

A: mass of 1 mol of ammonia = mass of 1 mol of N + mass of 3 mol of H atommass of 1 mol of ammonia =…

Q: Niobium is a transition metal used for making airplane propellers stronger as well as making…

A: Given Heat of fusion (ΔHfus) = 26.8 kJ mol-1 Mass of niobium metal = 25.4 g To Calculate: Heat…

Q: How much heat is needed to convert 35.6g of ice at 0°C to water at 27°C? AHfus of ice = 6.01 kJ/mol…

A: Heat required = Raise the temperature from 0 oC to 27 oC Q = mc delta T

Q: Calculate the total amount of heat needed to convert 22.50 g of solid carbon tetrachloride, CC14, at…

Q: 20. How much heat is required to convert 5.0 g of ice at -10.0 C to liquid water at 15.0 C? (Assume…

A: To calculate the amount of heat required to convert 5.0 g of ice at -10°C to liquid water at 15°C,…

Q: How much heat is required to vaporize 54.9g of acetone at its boiling point? The heat of…

Q: How much energy is required to vaporize 158 g of butane (C4H10) at its boiling point if its AHvap is…

Q: If 100 grams of ice at -10.0 degrees C is placed in 200 grams of water at 90 degrees C in an…

A: Specific heat is defined as the quantity of heat required to raise the temperature of one gram of a…

Q: The standard heat of vaporization for water is 40,700J/mol. What is the boiling point of water at a…

A: By Clausius-Clayperon equation lnP2P1= △HR(1T1- 1T2) △H=Heat of vaporizationP2 = Final pressureP1=…

Q: What is the enthalpy change for converting 10.0 g of ice at -15.0 °C to water at 55.0 °C in kJ. The…

A: Mass of ice = 10 g Initial temperature = - 15°C Final temperature = 50°C Specific heat of ice = 2.09…

Q: -20.9 °C to water at 38.3 °C. becfic heat capacities: ce = 2.108 J/g.°C water = 4.184 J/g.º℃ eat of…

Q: 7. How many calories of energy are released to the surroundings when 275g of mercury freezes? The…

Q: a. Calculate the heat required to melt 7.64 g of benzerie at jts normal melting point. Heat of…

A: Given: Mass of benzene = 7.64 g. Heat of fusion of benzene = 9.92 KJ/mol. And heat of vaporization…

Q: If 100.0 g of ice at -10.0°C is placed in 200. g of water at 90.0°C in an insulated container, what…

A: Given : Mass of ice = 100.0 g Initial temperature of ice = -10.0 oC Mass of hot water = 200 g And…

Question

8) If the heat of fusion for water is 80. cal/g, how many calories are needed to melt 45.0 g of ice at 0 °C?
A) 0.56 cal
B) 80. cal
C) 3.6 cal
D) 1.8 cal
81
Insimal
olgmootesd ir
moils ono
nimuis
E) 3.6 x 103 cal
os6.0 (8

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 with 1 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Two 20.0 g ice cubes at -18.0 C are placed into 225 g of water at 25.0 C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tr, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/(mol-K) Tr = °C heat capacity of H O1) 75.3 J/(mol-K) enthalpy of fusion of H,0 6.01 kJ/mol
How much heat (in calories) is absorbed when a 2.60 kg block of ice melts into a liquid? For water, ΔΔHfus = 80.0 cal/g ΔΔHvap = 540.0 cal/g
Please answer question 3.
What amount of heat (in kJ) is required to convert 19.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g-°C; specific heat capacity of liquid = 1.58 J/g-°C; AHfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)
Suppose 1.0 x 102 grams of ice absorbs 1255 J of heat, reaching a final temperature of -2.0°C.What was the initial temperature change of the ice? The specific heat capacity of H 2 O(s) = 2.1J/(g·ºC)
Based on the thermodynamic properties provided for water, determine the amount of energy released for 130.0 g of water to go from 89.0 °C to -12.0 °C. Property Value Units Melting point 0.0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C
What is the enthalpy (in J) required to melt a 4.77g block of Ice? H fusion= 6.00) kJ/mol
Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro
How much heat is required to raise the temperature of 4.5g of ice from -15.0ºC to 106ºC?
What quantity of heat (in KJ) would be required to convert 11.1 g of ice to water 0.00 C ? (Hfus=6.01 KJ/ mol for water)
6. Carbon disulfide has Pvap = 94 mm Hg at -3.5 °C and a normal boiling point of 46.5 °C. What is AHvap in kJ/mol?
Calculate the energy (in kcal) required to convert one ice cube that was made by freezing 72 mL of water (density = 1.000 g/L) an an initial temperature of -36.0 C, to liquid water at a final temperature of 37.0 CH2O(s) --> H2O(l) ΔH = +6.02 kj/mol Cpm H2O(s) = 37.7 J/mol x K Cpm H2O(l) = 75.4 J/mol x K 1 kcal = 4.18 kJ