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for subparts a, c, d, e, f
![13.39. Complete the following equations:
||
(a) CH,CH,CHËBr +
-CO;¯
-
CH,
(b)
CO,H + PBr,
-CO,H +
H,SO,
heat
(c)
(1) LIAIH,
(d)
o,CH,CH,
(2) H,0
(e) CH,CH;CH,CO,H + SOCI,
D'
(f) CH,CH,OČOCH,CH, + D,O
(g) CH,CH,CCI + (CH;=CHCH2),Cd
(h) CH,CH,CI + LiCu[CH(CH3),:]2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8538c8bf-746e-4715-909a-c76d8ddcd05a%2F8faa929c-7eae-4269-b784-c1c15ff0a15e%2Fandt3ed_processed.png&w=3840&q=75)
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- 13.3p. If you allow one pound of carbon dioxide to sublime (change from CO2(s) to CO2(g)) at room conditions of roughly 1atm and 25C, what volume would it occupy?What is the Gibbs free energy, in kJ/mol, of a reaction that has an equilibrium constant of K = 4.44 × 1014 at 400 oC?Estimate the temperature at which the equilibrium constant for CuSO4 ⋅ 5 H2O(s) → CuSO4(s) + 5 H2O(g) becomes 1; assume pH2O = 1 bar.
- At 4000C and 350 bar, a 1:3 mixture of nitrogen and hydrogen gases react to form an equilibrium a mixture containing ammonia at a mole fraction of 0.75. Assuming perfect gas behavior, calculate the equilibrium constant K for: N2(g) + 3 H2(g) ⇄ 2 NH3(g)You have a calorimeter with a heat capacity of 0.426 kJ/ºC. You combine 50.0 mL 1.50 M NaA (A- = conjugate base of weak acid HA) with an equal volume of HCl of higher molarilty. The temperature changes from 18.6 ºC to 21.1 ºC. What is ΔHºdissoc for the dissociation reaction of HA, in kJ?For a C <->2D equilibrium reaction, if the enthalpy change at standard condition is 60 kJ/mol, if there is 20% decomposition at 1 bar and 1000⁰C, what is the K value at room temperature (25⁰C), the Gibbs energy change of the reaction under standard conditions, and the K value at 1200K?
- Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.Molecular bromine is 24 per cent dissociated at 1600 K and 1.00 bar in the equilibrium Br2(g) = 2 Br(g). Calculate (a) K at 25°C, (b) ∆r G0 , (c) K at 2000°C given that ∆r H o = +112 kJ mol−1 over the temperature range.A student conducted an experiment to determine the Ksp of Ca(OH)2 at T = 298 K. The value he calculated was 5.4 x 10-6 and when he looked the theoretical value, he found that it is 5.1 x 10-6. Give the possible sources of error why the calculated value was higher than the theoretical value