Answer question “B” MULTI-STEP HEAT PROBLEMSThe data below refers to an unknown substance, X.BoilingHeat ofPointFusionMeltingpoint14.0°C86.0°CHeat ofVaporization150 J/g550 J/g4.3 J/g °C5.2 J/g °C1.1 J/gºC1. Draw a heating curve for substance X, going from 2°C to 120°C on the axis below. Write in allformulas used to calculate heat.(vapor)(solid) melting (q'heatingng (Fusim)T2=120°CTi=86.0°C(liquid)heatingSH Capacity SH(solid)zbhaving your taste buds rocked, here's $10 off your order of92=mxAH fus(liquid)heating25q1=mxsh (solid) (T₂-T₁) T2=14.0°CT₁ -2°CVaporization vapor (gas)24-Μ. ΔΗναρ2¹92= mxsHliqui djx (T₂-T₁).SH (vapor)Alvap->heat ofc. How much heat will be released when 25g of X cools from 110°C to 50°C?VaporizationT2=86.0°CT₁=14.0°CAttrur->heat of fusionM-mass of X2°CSolidb. Determine the amount of heat necessary to change 30g of X from solid at 4°C to liquid at 14°C.10EnterShiftPgDn

Answered: Image /qna-images/answer/1727cd0d-98bd-4b2f-8dc0-971d148eca8c.jpg

MULTI-STEP HEAT PROBLEMS The data below refers to an unknown substance. X. Boiling Heat of Point Fusion Melting point 14.0°C Heat of Vaporization 150 J/g 550 J/g 4.3 J/gºC 5.2 J/gºC 1.1 J/gºC 1. Draw a heating curve for substance X, going from 2°C to 120°C on the axis below. Write in all formulas used to calculate heat. qs=mXSH (vapor (T2-T.) 86.0°C (solid) melting (Fusim) qº heating SH Capacity SH (solid) T2=120°C Ti=86.0°( heating (liquid) vaporization 2¹ (liquid) 92: mxAH fus q1=myst (solid) (T₂-T₁) I2=14.0°C T₁-2°C heating q4=mx Alvap SH (vapor) 25 vapor (gas) 92= mxsHliqui djx (T₂-T₁).- Alvap->heat of Vaporization T2=86.0°C 7₁=14.0°C Atrus->heat of fusion M-mass of x 2°C Solid b. Determine the amount of heat necessary to change 30g of X from solid at 4°C to liquid at 14°C.

MULTI-STEP HEAT PROBLEMS The data below refers to an unknown substance. X. Boiling Heat of Point Fusion Melting point 14.0°C Heat of Vaporization 150 J/g 550 J/g 4.3 J/gºC 5.2 J/gºC 1.1 J/gºC 1. Draw a heating curve for substance X, going from 2°C to 120°C on the axis below. Write in all formulas used to calculate heat. qs=mXSH (vapor (T2-T.) 86.0°C (solid) melting (Fusim) qº heating SH Capacity SH (solid) T2=120°C Ti=86.0°( heating (liquid) vaporization 2¹ (liquid) 92: mxAH fus q1=myst (solid) (T₂-T₁) I2=14.0°C T₁-2°C heating q4=mx Alvap SH (vapor) 25 vapor (gas) 92= mxsHliqui djx (T₂-T₁).- Alvap->heat of Vaporization T2=86.0°C 7₁=14.0°C Atrus->heat of fusion M-mass of x 2°C Solid b. Determine the amount of heat necessary to change 30g of X from solid at 4°C to liquid at 14°C.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter6: Equilibria In Single-component Systems

Section: Chapter Questions

Problem 6.26E

See similar textbooks

Similar questions

A 2.00-L box initially contains 234 g of ice at -10 oC. The system absorbs 140. kJ of heat. cice = 2.0 J/g×oC; c.liquid = 4.2 J/g×oC; ΔHfus = 6.0 kJ/mol; ΔHvap = 42.5 kJ/mol; Pvap = 24 torr at 25 oC Determine the final temperature (oC) of the H2O.
vapor pressure of water is given by lnP= A-4880/T the heat of vaporization of water at 100c is 538cal/g please calculate the volume of 1g of water vapor at 1 atm and 100c
Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? The nitrogen released heat and the flask absorbed it.
Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? The nitrogen gas will first condense to liquid at -196oC then the liquid will decrease its temperature to -210oC.
4.How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point, if its ΔHvap is 31.6 kJ/mol? Group of answer choices 31.2 kJ 6.49 kJ 55.1 kJ 15.4 kJ 18.1 kJ
Ammonia has a normal (1.00atm) boiling point of -33.3*C. Under a pressure of 2.11 atm, what is ammonia's boiling point in *C? For ammonia delta vaporization= 23.3kJ/mol.
Under normal atmospheric pressure, nitrogen boils (and condenses) at -196oC. When 7.7 g of nitrogen gas at -196oC was put into a dewar flask initially at -260oC, their temperatures reach -210oC. The specific heat capacity and heat of vaporization of nitrogen are 1.04 J/g-oC and 200 J/g. Based on the system described above, is the following statement true or false? The magnitude of the heat effect on the flask can be evaluated using the formula C·ΔT.
Nitrogen is liquified from an air sample at -200oC. This is an example of what kind of process? a. sublimation b. freezing c. endothermic d. exothermic e. vaporization
Find ΔHrxn, ΔSrxn, and ΔGrxn for this phase change CCl4 (l) <- -> CCl4 (g) and then, what is ΔGrxn, when you use ΔGrxn = ΔHrxn – TΔSrxn, at the temperatures… a) -95.0°C b) 495.0°C
. How much energy does it take to heat a 45.0 g sample of substance X from-10.0 0C to 70 0C? Draw a heating curve for the process and show yourcalculations.Given the following information for substance X:Specific Heat (c) of solid phase: 2.0 J/g°CHeat of Fusion (Lf): 100 J/gSpecific Heat (c) of liquid phase: 5.0 J/g°CHeat of Vaporization (Lv): 1000 J/gSpecific Heat (c) of vapor phase: 1.0 J/g°CBoiling point: 55 0CMelting point: 5 0C
1955 Robert Wentorf. Graphite to diamond at 2000°C and 106 atm. Even though graphite is more stable than diamond at 25°C and atmospheric pressure, the conversion is very slow. A process called chemical vapor deposition uses Carbon sources like methane to release carbon atoms in presence of hydrogen gas and deposit it as diamond at low pressure and temperature (600°C) Reference: Chemistry: An atoms first approach, Zumdahl & Zumdahl, Cengage Learning, 2012. Question: Based on the above phase diagram: Comparing graphite and diamond, which one is denser? How many triple points? Explain
A 154.1 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C. (heat capacity of liquid = 1.62 J/g･°C; heat capacity of gas = 1.04 J/g･°C; ∆Hvap = 78.11 kJ/mol; Tb = 160.3 °C) a) How much energy (in kJ) is absorbed/released to cool the gas? b) How much energy (in kJ) is absorbed/released to condense the gas? c) How much energy (in kJ) is absorbed/released to cool the liquid? d) How much energy (in kJ) is absorbed/released for the entire process?