3. Make an energy diagram for the heat formation of one mole ofeach of the following substances:H2(g) + 2(9)→ 2H (9)a.b.2H2(g) + COCH₂OH (1)C.C(s) + 2H2(9)CH4(9)

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Answered: 3. Make an energy diagram for the heat…

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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8. 1.250 L of a 0.7601 mol/L Sodium Sulfide aqueous solution is mixed with 500.0 mL of a 0.7450mol/L aqueous solution of Lead (II) Nitrate. A. How much energy is absorbed or released by the reaction? B. If the reaction is carried out in a calorimeter whose constant is 14.60 kJ/°C and the solutions are initially at 21.000°C, what is the final temperature of the reaction solution on completion. Assume the heat capacity of the final solution is 4.200 J/g°C and that it has a density of 1.05 g/mL. Also assume that any solid formed does not absorb or give off heat.
1. Use standard enthalpies of formation from the equation sheets or the back of your book to calculate H°rxn for this reaction. Then draw a Reaction Energy diagram for the reaction using "Reaction Progress" on the x-axis and "Potential Energy" on the y-axis. Label H°rxn, reactants and products on each diagram. 2 H2S(g) + 3 O2(g)  2 H2O(g) + 2 SO2(g) please help me to answer this question
a. How much energy is required to decompose 850 g of PCl3, according to the reaction below? The molar mass of PCl3 is 137.32 g/mol and may be useful.4 PCl3(g) → P4(s) + 6 Cl2(g) ΔH°rxn = +1207 kJ b. The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 6.00 g of water from 22.0°C to 57.0°C? 1.99 × 10-2 J 1.98 × 103 J 65.0 J 50.2 J 878 J
What is the enthalpy change, Delta Hrxn, for the following reaction? 2 RbI (s) + Cl2 (g) --> 2 RbCl (s) + I2 (s) a. 1.33 x 103 kJ b. 656 kJ c. – 215 kJ d. 107 kJ e. 763 kJ f. none of these g. – 1.33 x 103 kJ h. 871 kJ
When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2 and liquid water are formed. The reaction absorbs 90.1 KJ of heat. a. Write a balanced thermochemical equation for the reaction. b. Calculate ∆H°f for calcium cyanamide.
c. Draw a potential energy diagram for the formation of NO₂(g): N₂(g) +20₂(g) → 2NO2(g). AHreaction = 66.2 kJ/mol. Label the graph with "Reactants," "Products," "AHreaction," and "Ea
2. The decomposition of ammonia gas into nitrogen gas and hydrogen gas is endothermic: 2 NH3 (g) → N2 (g) + 3 H2 (g) ΔH = 92 kJ/mol If 762 mL of hydrogen gas, measured at 325°C and 792 mmHg, is formed in the reaction above, how much heat will be absorbed?
The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol
An 87.9 g sample of chromium metal at 99.1°C is placed in a calorimeter containing 100.00 g of water at 21.0°C The contents of the calorimeter come to a temperature of 25.7°C. The heat capacity of water is 4.18 J/(g* °C) a. Is this process exothermic or endothermic? b. Calculate the amount of heat released by the metal (q metal) in Joules. Show your work.
Please help with question 2!

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3. Make an energy diagram for the heat formation of one mole of each of the following substances: H2(g) + 2(9) → 2H (9) a. b. 2H2(g) + CO CH₂OH (1) C. C(s) + 2H2(9) CH4(9)