lab 5 enthalpy of ice

In model 1 of the activity 'Vapor Pressure vs. Temperature and Heating Curves and Vapor Pressure', Why is the slope different between phase 1 and phase 3? the change in temperature was different between liquid water and solid water the liquid water was heated at a different rate than solid water liquid water has a different heat capacity than solid water liquid water has a greater density than solid water

Calculate the amount of heat needed to melt 128. g of solid acetic acid (HCH2CO,) and bring it to a temperature of 83.1 °C. Be sure your answer has a unit symbol and the correct number of significant digits. x10 ? Submit Assignment Terms of Use Privacy 2019 McGraw-Hill Education. All Rights Reserved. MacBook Pro DII 000 OO0 F 9 F10 F8 esc F 6 F7 F 5 F 4 F3 F2 F1 % 2 3 5 co X S4

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The following information is given for silver, Ag, at 1 atm: Boiling point = 2212.0°C   Heat of vaporization =  cal/g Melting point = 961.0°C   Heat of fusion = 26.5 cal/g How many kcal of energy must be removed from a 21.7 g sample of liquid silver in order to freeze it at its normal melting point of 961.0°C? Energy removed =  ______kcal

I need help with question 3 B,C,D,E

4. Calculate the amount of energy absorbed when 5g ice @ 0°C melts to water at 0°C. Did a phase change occur? If so, which one? Is this endothermic or exothermic?

Answer number 1-5 pls. I don't want to waste my money here

Rectangular Snip Question 5 of 18 Submit What is the quantity of heat (in kJ) associated with cooling 150.3 g of water from 25.60°C to ice at -10.70°C? kJ Cliquid = 4.184 J/g•°C Csolid = 2.092 J/g.°C 1 2 Trusion = 0.00 °C AHfusion 4 C 6.01 kJ/mol 7 8 +/- х 100 + CO LO

How much heat will it take to raise the temperature of 10 g of ice from −30°C to −20°C?   The specific heat of ice is 0.48 cal/g°C.

cntical point 218 water ice P. 1. atm triple point 0.006 water he rg dang vapor 100 374 T°C In order to sublimate completely (and not melt), water has to O increase in pressure at a temperature below the triple point decrese in pressure at the exact temperature of the triple point increase in temperature at a pressure below the triple point decrease in temperature at a pressure below the triple point

Using the data below, determine how much heat (in Joules) is required to convert 405.0 g of ice at -18.5°C to liquid water at 67.5°C Please enter your answer as a number with the correct unit and number of sig figs. Quantity c, H₂0 (s) c, H₂0 (1) c, H₂O(g) AH fus AHvap Value 2.087C 4.184 2.042 334 g-°C (per gram) 6.01. 36.03 75.37 Value (per mole) 37.60 mol - °C J mol - °C 8. mol. °C kj mol 2260 40.7 k mol

The graph below represents the heating curve of a substance that starts as a solid below its freezing point. 70 10 -20 10 15 20 25 30 35 40 Time (minutes) 1. Which letter represents the state that has definite volume but no definite shape. Which part of the curve represents a mixed solid/ liquid phase of substance? 3. What is the melting point of the substance? °C. 4. Which letter represents the state where molecules cannot move? 40 Temperature ("C) 2.

Calculate the amount of energy absorbed when 75g ice @ -4C melts to 31 C Did a phase change occur? If so, which one?    Is this endothermic or exothermic?

Please provide solution. Thank you!

= STATES OF MATTER Using a phase diagram to predict phase at a given temperature... Study the following phase diagram of Substance X. pressure (atm) 2.8- 1.4- solid 0- 0 100 liquid 200 temperature (K) Use this diagram to answer the following questions. gas 300 Suppose a small sample of pure X is held at -231. °C and 1.7 atm. What will be the state of the sample? Suppose the temperature is held constant at -231. °C but the pressure is decreased by 0.8 atm. What will happen to the sample? Suppose, on the other hand, the pressure is held constant at 1.7 atm but the temperature is increased by 121. °C. What will happen to the sample? (choose one) ✓ (choose one) (choose one) X 3 0/3

The vapor pressure of Substance X is measured at several temperatures: temperature vapor pressure -8.°C 0.103 atm 7. °C 0.142 atm 22. °C 0.189 atm Use this information to calculate the enthalpy of vaporization of X. Round your answer to 2 significant digits. Be sure your answer contains a correct unit symbol. ☐ 0.0 0|0 = × S

Calculate the amount of heat needed to melt 128. g of solld octane (C,H,) and bring it to a temperature of -44.7 °C. Be sure your answer has a unit symbol and the correct number of significant digits. x10

...elting point enthalpy of fusion temperature (°C) 80 70 60 50- 40- 30 You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at -20 °C is put into an evacuated flask and heated at a constant rate until 10.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. 20- 10- 0 -10- -20 density 0 1 2 3 30. °C 4.00 kJ/mol 3 3.00 g/cm³ (solid) 2.30 g/mL (liquid) 4 5 6 7 heat added (kJ/mol) 8 9 boiling point enthalpy of vaporization 10 heat capacity × 60. °C 34.00 kJ/mol 1 1 29. J.K¹·mol ·mol (solid) - 1 56. J.K mol (liquid) 1 44. J∙K¯¹·mol (vapor) Ś -1

Given that for liquid water, AH(fusion)=334J/g, how much is needed to melt approximately 34.2 grams of ice?

This question is not a grade question, its just a pratice problem.

= STATES OF MATTER Identifying phase transitions on a heating curve A pure solid sample of Substance X is put into an evacuated flask. The flask is heated at a steady rate and the temperature recorded as time passes. Here is a graph of the results: temperature (°C) 170. 150. 130. 110. 90 70. 0. 10. What is the melting point of X ? Use this graph to answer the following questions: heat added (kJ/mol) What phase (physical state) of X would you expect to find in the flask after 5 kJ/mol of heat has been added? *C 30. X 40. (check all that apply) solid liquid gas 0/3 50.

3. Calculate the heat required to increase the temperature of 630 grams of ice from -2℃ to 23℃ and turn it to steam with temperature of 124℃. The specific heat of ice is 2.108 J/(g∙℃).

Temperature (°C) 125 a. 100 75 C. 50 25 0 -25 Select one: 5 J b. 91 J A BC 68 J d. 10 J Ice Vaporization temperature does not change until all H₂O() becomes H₂O(g). Heat added •Calculate the enthalpy change for AB, for 1 mole of ice D Liquid water Steam. Melting temperature does not change until all H₂O(s) becomes H₂O(1). F E

Just answers label so I know

1 Intermolecular Forces Water is a polar molecule. It has an electric dipole strength of p = 6 x 10-30 C - m. This is roughly equivalent to a proton and an electron separated by a distance of d = 4 x 10-11 m (about the radius of a hydrogen atom). In this problem, we will use Coulomb's law to compare the force between two protons (H*), a proton and a water molecule, and two water molecules. Use the arrangement of the charges shown in the figure for your calculations. (a) r (b) (c) r (a) First, consider interactions at "short" distances. A chemical bond has a length on the order of r = 0.1 nm. • What is the force between two protons separated by a distance of r = 0.1 nm? • What is the force between a proton and a water molecule separated by a distance of r = 0.1 nm? What is the force between two water molecules separated by a distance of r = 0.1 nm? (b) Now consider a "long" distance: a separation of R = 1.0 nm. (This is about the length of ten hydrogen atoms lined up next to each…

Calculate the amount of heat needed to melt 180. g of solid octane (C,H,2) and bring it to a temperature of -32.8 °C. Be sure your answer has a unit symbol and the correct number of significant digits. ?