How do we predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each of the following reactions will be spontaneous.
(I have the correct answers to the following so I really want to understand how to solve this question or approach it - Thank you)
a) H2O(g) -->H2O(l)
b) CO2(s)-->CO2(g)
c) H2(g)-->2H(g)
d) 2NO2(g)-->2NO(g)+O2(g)(endothermic)
*Please expain how to determine the answers - I have the correct solutions*
How do we predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which...
2NO2(g)--2NO(g)+O2(g) (endothermic) H2(g)--2H(g) H2O(g)--H2O(l) CO2(s)--CO2(g) cem 15 Part A Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each of the following reactions will be spontaneous Drag the appropriate items to their respective bins. Reset Help 2NO3(e)--2NO(g) + Os(e) (endele) - 1.00 H.) - 24(e) CO.() - CO. High temperature Low temperature All temperatures No temperatures
Question 6 1.5 pts Predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any, the following reactions will be spontaneous. A. 2CO(g) + O2(g) = 2002(g), AH rxn=-566.0 kJ [ Select] B. 2NO2(g)2NO(g)+O2(g), AH rxn= +113.1 kJ [ Select ] C. 2H2(g)+O2(g)—2H2O(g), AH rxn=-483.6 kJ [ Select] D. 2H2O2(1)→2H2O(1)+O2(g), AH rxn= -196.0 kJ [Select ]
Question 5 1 pts Predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any, the reaction will be spontaneous. A. 4NO(g)+6H2O(g) 4NH3(g)+502(g) AHrxn=+906kJ [Select] B. 2N2O(g)+O2(g)-4NO(g) AH rxn=+197.1kJ [Select] C. C3H3(g)+502(g)-3CO2(g)+4H2O(g) AH rxn=-2044kJ Spontaneous at all temperatura A
Exercise 18.38-Enhanced-with Feedback 7 of 13> Part E ReviewI ConstantsI Periodic Table In addition, predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any the reaction in each part will be spontaneous. Without doing any calculations, iddentify the signs of ΔSays and ΔSsurr for each of the following chemical reactions. Drag the appropriate items to their respective bins. Reset Help Reaction is spontaneous at all temperatures Reaction is spontaneous at low temperatures Reaction is spontaneous at high...
16. For the following reactions, predict whether they will tend to be spontaneous at either high or low temperatures, or at all temperatures, or at no temperature (10.0 points) a) H2(g) + 12(g) → 2HI(g) AH = -220 kJ b) 3S2(g) → 253(g) AH = +227 kJ c) H2O(l) → H2O(g) AH = +44 kJ d) H2(g) + '/gS8(g) → H2S(1) AH = -247 kJ
Predict whether AS will be positive or negative for reactions (a) and (b): a. 2 HgO(s) → 2Hg(1) + O2(g) AS b. 2 CH (B) + 70(8) ► 4 CO2(g) + 6 H2O(1) AS Choose one of the above reactions a OR b. Calculate the AH® for your chosen reaction using information from the table below. AH = Using your answers above, predict under what temperature (temp) conditions (high temp or low temp) where this reaction will be spontaneous, or...
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Consider the reaction: 2 BsHs (I)12 02 (g) (a) Use the standard enthalpies of formation found in Appendix B of the textbook to calculate the enthalpy change of the reaction. The standard enthalpy of formation of BsH, (I) is 73.2 kl/mol. 5 B2Os (s) +9 H2O (I) (b) Predict the sign of the entropy change and provide the two reasons likely to have made the biggest impact on the entropy change (and upon which you based your prediction). (c) Based...
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20) Which statement is true concerning the stand A) The standard state for N2() is the pure gas at 1 atm. B) The standard state for N2() is the pu at a concentration of 1 mol/L. tre concerning the standard states of N2(x) and C12H22011(aq)? te for N2(8) is the pure gas at 1 atm and for C12H22011(aq) is the pure solid 20) — ndard state for N2() is the pure gas at 1 mol/L and for C12H22011(aq) is the...