Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can.ChangeDuring an endothermic chemical reaction, four moles of gaseous reactantsare turned into two moles of gaseous products.A solid precipitates from a solution, releasing heat as it does so.Is this change spontaneous?Yes.No.Can't decide with information given.○ Yes.○ No.Can't decide with information given.A solid substance dissolves in water, releasing heat as it does so.Yes.No.○ Can't decide with information given.

Q1. Since the reaction is endothermic, that means you have to provide heat during the reaction,…

Answered: Read the descriptions of physical or…

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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In the past, scientists were surprised that an endothermic process like the one in this lab, could be spontaneous. Which statement correctly describes why it seems like an endothermic process should not be spontaneous? Group of answer choices All endothermic processes create order in both the system and surroundings. Endothermic processes cause heat to flow from a cold object to a hot object. A process that spontaneously takes in energy seems to be analogous to a rock rolling up a hill. Endothermic processes become so cold that molecular motion stops.
What is the change in enthalpy (∆H) for a chemical reaction?How is ∆H different from ∆E?
1.Consider the complete combustion of methane gas, CH4(g): Which of the following BEST describes the relationship between ΔH and ΔU? a.ΔH > ΔU b.ΔH = ΔU = 0 c.ΔH = ΔU d.ΔH < ΔU 2.Which of the following reactions would you expect to have the lowest ΔSo? a.CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) b.C2H4(g) + 2O2(g) → 2CO2(g) + 2H2O(g) c.C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(g) d.C2H6(g) + 7/2O2(g) → 2CO2(g) + 3H2O(g) 3.Which species would you expect to have the lowest standard entropy (So)? a.Cl2(g) b.I2(s) c.F2(g) d.Br2(l)
15.A sample of 125 g of cold water and 283 g of hot water are mixed in an ideal thermos and thermal equilibrium is reached. If the initial temperature of the cold water is 3°C and the initial temperature of the hot water is 91 °C, what will be the final temperature? Justify your answer
Explain Enthalpy and Entropy ? Show the Difference between them ?
Consider the following reactions at 298 K. 2 03(g) → 3 O₂(g) O₂(g) → 2 0(g) NO(g) + O3(g) → NO₂(g) + O₂(g) ΔΗΘ Aat H ᎪᎻᎾ = -427.0 kJ/mol = 495.0 kJ/mol = -199.0 kJ/mol Apply Hess's law to calculate the standard reaction enthalpy for the reaction NO(g) + O(g) → NO₂(g)
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change A gas condenses to a liquid, neither absorbing nor releasing heat. An exothermic chemical reaction between a solid and a liquid results in gaseous products. Two liquids mix, neither absorbing nor releasing heat. Is this change spontaneous? Yes. No. Can't decide with information given. ○ Yes. ○ No. Can't decide with information given. Yes. No. ○ Can't decide with information given.
Which one of the following reactions cannot proceed spontaneously as written at any temperature? Assume that ΔH°rxn does not depend on temperature. A. 2Cl2O(g) → 2Cl2(g) + O2(g) ΔH°rxn = –151 kJ B. 3O2(g) → 2O3(g) ΔH°rxn = +284 kJ C. COCl2(g) → CO(g) + Cl2(g) ΔH°rxn = +112 kJ D. 2C(s) + 2S(s) + O2(g) → 2COS(g) ΔH°rxn = –137 kJ E. N2O4(g) → 2NO2(g) ΔH°rxn = +171 kJ
State the First Law of Thermodynamics in your own words. Cite at least one example that applies to the First Law of Thermodynamics.
Strontium carbonate is responsible for the red color in fireworks. It is generated in the reaction given below. Sr(s) + C(graphite) + 3/2 O2(g) → SrCO3(s) Use these reactions to determine ∆H for the formation of 1 mole of SrCO3. Sr(s) + ½ O2(g) → SrO(s) ∆H = -592 kJSrCO3(s) → SrO(s) + CO2(g) ∆H = 234 kJC(graphite) + O2(g) → CO2(g) ∆H = -394 kJ
None
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 24.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 24.0 L. w = J Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.50 atm to a volume of 16.0 L. 2. From the end point of step 1, let the gas expand to 24.0 L against a constant external pressure of 1.00 atm. w = J

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