Liquid ammonia (boiling point = -33.4°C) can be use as a refrigerant and heat transfer fluid. How much energy is needed to heat 25.0 g of NH3(1) from - 65.0°C to -12.0°C? (Show work) Specific heat capacity, NH3(): 4.7 J/(gxK) Specific heat capacity, NH3(g): 2.2 J/(gxK) Heat of vaporization: 23.5 kJ/mol Molar mass, : 17.0 g/mol 6.3 kJ 340 kJ 5.5 kJ 590 kJ

Liquid ammonia (boiling point = -33.4°C) can be use as a refrigerant and heat transfer fluid. How much energy is needed to heat 25.0 g of NH3(1) from - 65.0°C to -12.0°C? (Show work) Specific heat capacity, NH3(): 4.7 J/(gxK) Specific heat capacity, NH3(g): 2.2 J/(gxK) Heat of vaporization: 23.5 kJ/mol Molar mass, : 17.0 g/mol 6.3 kJ 340 kJ 5.5 kJ 590 kJ

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

Similar questions

Need solution to all parts urgently
ator%=Dassignment-take Not syncing The combustion of 0.1557 g benzoic acid increases the temperature of a bomb calorimeter by 2.50°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) [References) Heat capacity = kJ/°C A 0.2155-g sample of vanillin (Cg Hg O3) is then burned in the same calorimeter, and the temperature increases by 3.20°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol Submit Answer Try Another Version 5 item attempts remaining (Previous Next Save and Exit Email Instructor Technical Support
The AH value for the reaction 2Hg(1) + 02(g) heat (kJ) is released when 43.4 g Hg is reacted with oxygen? - 2H9O(s) is -181.6 kJ. How much
The heat capacity of a bomb calorimeter was determined by burning 6.85 g of methane (energy of combustion = -803 kJ/mol CH4) in the bomb. The temperature changed by 11.1°C. (a) What is the heat capacity of the bomb? kJ/°C (b) A 14.7-g sample of ethanol (C₂H5OH) produced a temperature increase of 12.8°C in the same calorimeter. What is the energy of combustion of ethanol (in kJ/mol)? kJ/mol
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
ab The enthalpy of solution (AH) of NaNO3 is 20.4 kJ/mol. If 8.50 g NaNO3 is dissolved in enough water to make a 100.0 mL solution, what is the change in temperature (°C) of the solution? (The specific heat capacity of the solution is 4.184 J/g °C and the density of the solution is 1.02 g/mL). Tap here or pull up for additional resources 1 Q @ 2 W # 3 E $ 4 R % 5 T Question 1 of 10 6 Y & 7 U 8 1 9 1 4 7 +/- 0
20.0 g of ice cubes at 0.0°C are combined with 150. g of liquid water at 70.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (Data: specific heat capacity of H20(), c = 4.18 J/g.°C; H 20( s) – H20() A H= 6.02 kJ/mol)Hint: When you equate heat lost to heat gained the heat capacity is cancelled since it si found on both sides of the equation and this simplifies your calculation. O 0.0 O 10.6 O 30.7 O 56.4 O61.8
5(a)
How much did our sodium-in-water demonstration raise the temperature of water in the dessicator jar? The reaction we performed was: Na(s) + H2O(l) NaOH(aq) + 1/2H2(g) qreaction = rHo = -184 kJ/mol-rxn Assuming the dessicator jar is well insulated (like our coffee-cup calorimeter), the energy balance is: 0 = qsystem = qreaction + qwater qreaction = -qwater qreaction = -mwater*Cwater*Twater The data from the demonstration was: (a) 1.0 kg water, (b) 22.0oC, (d) Cwater = 4.18 J/g-K, (e) mNa = 0.21 g How many moles of sodium were added to the water (in moles)?
5a