Substance X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of Xhave been determined:melting point80. °Cboiling point125. °Centhalpy of fusion7.00 kJ/molenthalpy ofvaporization21.00 kJ/mol2.20 g/cm³ (solid)density1.60 g/mL (liquid)34. J.K-1 'mol (solid)1heat capacity24. J.Kmol1(liquid)157. J.Kmol (vapor)You may also assume X behaves as an ideal gas in the vapor phase.Suppose a small sample of X at 50 °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.temperature (°c)150-140-130-120-110-100+90-80-70-60-50-034567910heat added (kJ/mol)G

Step 1: Heat required to increase the temperature up to its melting…

Answered: Substance X is known to exist at 1 atm…

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...

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The vapor pressure of liquid aluminum is 400 mm Hg at 2.59×10^3K. Assuming that its molar heat of vaporization is constant at 252kJ/mol, the vapor pressure of liquid Al is mm Hg at a temperature of 2.61×10^3 K.
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Use the phase diagram of Substance X below to find the melting point of X when the pressure above the solid is 10. atm. لالا pressure (atm) 32. Doc 16. solid 100 liquid 200 gas 300 temperature (K) Note: your answer must be within 12.5 °C of the exact answer to be graded correct.
How much heat energy is required to convert 39.6 g of solid ethanol at -114.5 °C to gaseous ethanol at 147.2 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of −114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g. °C, and that of gaseous ethanol is 1.43 J/g. °C. q= 4326.84 kJ
Calculate the amount of energy (in kJ) necessary to convert 497 g of liquid water from 0°C to water vapor at 182°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g °C, and for steam is 1.99 J/g °C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) kJ
Substance X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X have been determined: melting point 30. °C boiling point 90. °C enthalpy of vaporization enthalpy of fusion 8.00 kJ/mol 29.00 kJ/mol 1.70 g/cm (solid) 1.50 g/mL (liquid) density 35. J·K 1- •mol (solid) heat capacity 45. J'K (liquid) "mol 55. J·K •mol (vapor) You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at 0 °C is put into an evacuated flask and heated at a constant rate until 15.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment.
carbon disulfide Cs2 has a heat of vaporization of 29,200 J/mol. at 268 K it has a vapor pressure of 1.0 X 10^2 mmHg. what is its vapor pressure at 301 K
1. Calculate the amount of heat (in kJ) released when converting 150.2 g of water to ice at -23 degrees Celsius. 2. A closed vessel of volume 10.0 L initially contains 1.303 g of water and no water vapor. Please calculate the mass of liquid water remaining once the system reaches equilibrium at 30 degrees Celsius. The vapor pressure of water at that temperature is equal to 0.0418 atm. 3. A person drinks four glasses of cold water (5 degrees C) every day. The volume of each glass is 195. mL. How much heat (in kJ) does the body have to supply to raise the temperature of the water to 37 degrees C (body temperature)? 4.From these data: N2H4(l) + O2(g) à 2N2(g) + 2H2O(l) H= -622.2 kJ/mol H2(g) + ½O2 à H2O(l) H= -285.8 kJ/mol H2(g) + O2(g) à H2O2(l) H= -115 kJ/mol Find H for the reaction: N2H4(l) + 2H2O2(l) à 2N2(g) + 4H2O(l) 5. Consider the following chemical equation. CH4(g) + 2O2(g) à CO2(g) + 2H2O(l) Using the values in the table, calculate…
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How much energy would need to be added to 930.g of ice at 0.0°C to turn it into liquid water at 0.0°C ? 930. J O 3.89x103 J O 1.86x103 J O 2.10x106 J 3.12x105 J
Consider the phase diagram shown. What is the normal sublimation point at 1 atm? Pressure (not to scale) 72.9 atm 5.1 atm 1 atm O 0°C O 100°C -56.7 °C 31°C -78.5 °C SOLID LIQUID GAS -78.5 °C -56.7 °C Temperature (not to scale) 31 °C
Substance X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X have been determined: melting point enthalpy of fusion - 10. °C boiling point 4.00 kJ/mol enthalpy of vaporization 30. °C 39.00 kJ/mol 3 1.60 g/cm³ (solid) 1 1 density 44. J.K ·mol (solid) 1.30 g/mL (liquid) 1 -1 heat capacity 64. J.K ·mol (liquid) 1 1 54. J.K mol (vapor) You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at -50 °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. temperature (°C) 50- 40 30. 20 10. -10 -20 -30 -40 -50 0 1 2 3 4 5 6 7 8 9 10 heat added (kJ/mol) ☑ ? 00. 18 Ar

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