(a)
Interpretation:
The closed-system energy balance equation for the given process is to be written and simplified. The sign of non-zero heat and work terms are to be predicted.
Concept introduction:
The closed-energy balance equation for a closed system is expressed as,
Net energy transferred to the system
(b)
Interpretation:
The closed-system energy balance equation for the given process is to be written and simplified. The sign of non-zero heat and work terms are to be predicted.
Concept introduction:
The closed-energy balance equation for a closed system is expressed as,
Net energy transferred to the system
(c)
Interpretation:
The closed-system energy balance equation for the given process is to be written and simplified. The sign of non-zero heat and work terms are to be predicted.
Concept introduction:
The closed-energy balance equation for a closed system is expressed as,
Net energy transferred to the system
(d)
Interpretation:
The closed-system energy balance equation for the given process is to be written and to be simplified. The sign of non-zero heat and work terms are to be predicted.
Concept introduction:
The closed-energy balance equation for a closed system is expressed as,
Net energy transferred to the system
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EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.arrow_forwardThe dissolution process is represented by the following equation: CaCl₂ (s) Ca²+ (aq) + 2C1¯ (aq) The value for AHis 81.8 kJ for the reaction as written. (No sign has been included, as you are asked for that in Part 1.) When 0.0261 mol CaCl₂ is used in a hot pack, kJ of heat is produced by the hot pack.arrow_forwardA dilute solution of hydrochloric acid with a mass of 608.62 g and containing 0.38547 mol of HCI was exactly neutralized in a calorimeter by the sodium hydroxide in 616.25 g of a comparably dilute solution. The temperature increased from 16.621 to 20.626°C. The specific heat of the HCl solution was 4.031 J-g1.°C-1; that of the NaOH solution was 4.046 J-g1.°C1. The heat capacity of the calorimeter was 77.99 J.°C 1. Incorrect. Enter the balanced equation for the reaction. Include states in your answer. NaOH + HC1 →NACI, (aq) +H,O (1) (aq) (aq) eTextbook and Media Assistance Used 2 Incorrect. Use the data above to calculate the heat evolved. What is the heat of neutralization per mole of HCI? Assume that the original solutions made independent contributions to the total heat capacity of the system following their mixing. ΔΗ - kJ/molarrow_forward
- In a calorimetry experiment 3.2 g of potassium hydroxide is dissolved in 400 mL water in a thermos flask. The temperature increase in the solution is 7 \deg C. The effective mass of the glass in the thermos flask ( mcal) is 0.040 kg. The heat capacity of the solution (Cs) is 4.04 kJkg-1K-1. The heat capacity of the calorimeter (Ccal) is 0.387 kJkg-1K-1. Remember to enter your answer using the specified number of significant figures, but keep the entire number in your calculator for use in further calculations. Part B - Calculating qsolution Calculate the heat absorbed by the solution (qsolution) Give your answer to four significant figures. Part C- Calculating qcalorimeter Calculate the heat absorbed by the glass in the calorimeter (qcalorimeter). Give your answer to four significant figures. Part D - Calculating qtotal Calculate the total heat transferred for the reaction (qtotal) Give your answer to four significant figures. Calculate the number of moles of KOH used in the experiment…arrow_forwardA) A sample of Ammonium chloride,NH4Cl(s) is completely dissolved in 50.0mL of water in a calorimetee. determinr the molar enthalpy of dissolution (dissolving) of NH4ck(s). show all steps and proper units. when the mass of NH4Cl(s) is 3.96, the T initial is 20.2 degrees celsius and the Tfinal is 13.5 degrees celsius b) write a balanced chemical equation to represent process including the states and the delta H value.arrow_forwardThe vaporization of 1 mole of liquid water (the system) at 100.9°C, 1.00 atm, is endothermic. $$H2O(l)+40.7kJH2O(g)Assume that at exactly 100.0°C and 1.00 atm total pressure, 1.00 mole of liquid water and 1.00 mole of water vapor occupy 18.80 mL and 30.62 L, respectively. a. Calculate the work done on or by the system when 1.25 mol of liquid H2O vaporizes. answer in J. b. Calculate the water's change in internal energy. answer in kJ.arrow_forward
- 50.0mL of 0.300M CuSO4 is mixed with equal volume of 0.400M. The reaction temperature raised by 3.20oC. a) Determine the molar enthalpy of reaction. 2 NaOH + CuSO4 à Cu(OH)2 + Na2SO4 b) Write a thermochemical equation (with enthalpy value embedded in the equation) to represent the reaction:arrow_forward17D.4. Pondering the concept ofspecific heat while walking homefrom chemistry class, you find an oldpenny on the ground and begin towonder what the specific heat ofcopper is. You rush home and put5.00 g of water at 18.00 °C in astyrofoam cup. You heat the 2.45 gpenny to 50.00 °C and drop it in thewater. The final temperature of themetal and water is 19.38 °C.Assuming the penny is pure copper(which modern pennies are not),what is the specific heat of copper?The specific heat of water is 4.18J/g·°C.arrow_forward11. From the data in Table 4–1 calculate the heat of combustion of C,H,OH(g) at 25°C. 12. From the data in Table 4-3 determine at 25°C: (a) The amount of heat which will be liberated when 2 moles of H,SO.(1) are dissolved in 30 moles of H,0(1) (b) The differential heats of solution of the acid and the water for the given solution.arrow_forward
- Suppose that 4.92 grams of X (MW = 35.78) are dissolved in 647 mL of water, and the water temperature changes from 27.08°C to 28.24°C. Assume that the mass of X is negligible compared to the mass of the water. Assume the specific heat of water is 4.2 J/(g.°C) and the density of water is 1.0 g/mL. Calculate the enthalpy of dissolution of X in kJ/mol. Report your answer to three decimal places.arrow_forward50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution temperature rises by 3.0 °C. Calculate the enthalpy of neutralization per mole of HCl. The specific heat capacity of the solution is 4.18 J g-1 mol-1 and the density of the solution is 1.0 g ml-1.arrow_forwardFor the reaction P4010(s) + 6 H20(1) 4 H3PO4(aq) AG° = -447.6 kJ and AS° = -16.3 J/K at 345 K and 1 atm. favored under standard conditions at 345 K. This reaction is (reactant, product) The standard enthalpy change for the reaction of 2.34 moles of P4010(s) at this temperature would be kJ.arrow_forward
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