Consider the reaction below
2Na(l) + FeCl2(s) ⇌ 2NaCl(s) + Fe(s)
for which E°cell = 2.25 V at 200°C. G° at this temperature is
| A. |
-520 |
|
| B. |
-453 |
|
| C. |
-414 kJ |
|
| D. |
-376 |
|
| E. |
-434 |
QUESTION 6 Consider the reaction below 2Na(l) + FeCl2(s) = 2NaCl(s) + Fe(s) for which Eºcell = 1.95 V at 200°C. Gº at this temperature is - A. -414 kJ B. -434 C-376 D. -520 E. -453
Part A. Consider the non-aqueous cell reaction 2Na(l) + FeCl2(s) --> 2NaCl(s) + Fe(s) for which E°cell= 2.35 V at 200°C. deltaG° at this temperature is what? *Do not include units in your answer. Report answer to 3 sigfigs Part B. A voltaic cell consists of an Au/Au3+electrode (E° = 1.50 V) and a Cu/Cu2+electrode (E° = 0.34 V). Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell= 1.13 V at 25°C. *Do not include units in your answer. Report...
A chemist measures the enthalpy change
ΔH
during the following reaction:
2Na
(s)
+
Cl2
(g)
→
2NaCl
(s)
=ΔH−822.kJ
Use this information to complete the table below. Round each of
your answers to the nearest
/kJmol
.
A chemist measures the enthalpy change AH during the following reaction: 2Na(s) + Cl2(g)→2 NaCl(s) NH=-822. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol reaction △H kJ NaCl(s) → Na(s) + Cl2(g)...
Consider the following reaction:2Na + Cl2(g) → 2NaCl ΔH = -821.8 kJ(a) Is the reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 5.6 g of Na reacts at constant pressure. (c) How many grams of NaCl are produced during an enthalpy change of 16.5 kJ? (d) How many kilojoules of heat are absorbed when 44.1 g of NaCl is decomposed into Na and Cl2 at constant pressure?
Which of the following reactions will have the least amount of equilibrium shift in any direction, associated with a decrease in volume? a. 3O2(g) ⇄ 2O3(g) b. 2KClO3 (g) ⇄ 2KCl(s) + 3O2 (g) c. Fe(s) + CO2(g) ⇄ FeO(s) + CO(g) d. 4NH3 (g) + 5O2 (g) ⇄ 4NO(g) + 6H2O(l) e. 2Na(s) + Cl2 (g) ⇄ 2NaCl(s)
All of the following reactions can be described as displacement reactions except: a.) Zn(s) + FeCl2(aq) → ZnCl2(aq) + Fe(s). b.) C6H6(l) + Cl2(g) → C6H5Cl(l) + HCl(g). c.) 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g). d.) Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s). e.) CuSO4(aq) + Fe(s) → Cu(s) + FeSO4(aq).
A chemist measures the enthalpy change ΔH during the following reaction: 2Na (s) + Cl2 (g) → 2NaCl (s) =ΔH−822.kJ Use this information to complete the table below. Round each of your answers to the nearest /kJmol . reaction H →+6Nas3Cl2g6NaCls kJ →12NaCls+12Nas14Cl2g kJ →2NaCls+2NasCl2g kJ
B. Calculate the standard entropy change for the reaction
2Na(s)+Cl2(g)?2NaCl(s)
using the data from the following table:
Substance
?H?f (kJ/mol)
?G?f (kJ/mol)
S? [J/(K?mol)]
Na(s)
0.00
0.00
51.30
Cl2(g)
0.00
0.00
223.1
NaCl(s)
-411.0
-384.0
72.10
Express your answer to four significant figures and include the
appropriate units.
Part A Predict the sign of the entropy change, AS°,for each of the reaction displayed. Drag the appropriate items to their respective bins. Ag+(aq) + Cl-(aq) → AgCl(s) | | Ca(OH)2(s) →...
1. For the reaction 2SO2(g) + O2(g) ----->2SO3(g) ΔG° = -148.8 kJ and ΔS° = -187.9 J/K at 261 K and 1 atm. The maximum amount of work that could be done by this reaction when 1.98 moles of SO2(g) react at standard conditions at this temperature is _______ kJ. 2. For the reaction 2Na(s) + 2H2O(l) ---->2NaOH(aq) + H2(g) ΔH° = -368.6 kJ and ΔS° = -15.3 J/K The maximum amount of work that could be done when 2.25...
please helpppp!!!
7) The standard cell potential (E cell) f for the reaction below i ls -0 43 V. The cell potential for this at best cong (6 polnts) Ag Acid 6 natch the H idding 6e e cancel e, pposite pposite (e) e ancel is the he por Poten 8) The standard cell potential (E-cell) of the reaction below is .0.126 V. The value of ΔG" for the reaction is Pb (o) 2H (aq)Pb2+ (aq) H2 (g) vith (6...