5) Will this reaction occur spontaneously as written? (3 points) why 3Pb(s) + NO3 (aq) +...
1. Lead(II) sulfide dissolves in excess nitric acid according to the equation below. Calculate the volume of NO(g) at 27 °C and 1.10 atm produced from 4.7 g of PbS(s). M24.71 3Pb (s) + 2NO3(aq) + 8H(aq) 3Pb2+ (aq) + 3S(s) + 2NO(g) + 4H2O(1) 3x106.42432.065) a) 0.29 L b) 0.44 L c) 0.66 L d) 30. L 2x 4,057 + 16 - 44,014
For the following cell, at 25 ° C, Cr (s) | Cr (NO3) 3 (0.200 M) || Pb (NO3) 2 (0.060 M) | Pb (s) the cell potential was 0.589 V. Calculate the equilibrium constant for the following reaction at this temperature : 2Cr (s) + 3Pb2 + (aq) --- 2 Cr3 + (aq) + 3Pb (s)
For the reaction below: (5 points) 3Cu(s) + 2NO3– (aq) + 8 H+(aq) 3Cu2+(aq) + 2NO(g) + 4H2O(퓁)What is Gº at 25 ºC?(a) −361 kJ(b) 180. kJ(c) 361 kJ(d) −120 kJ(e) none of these
3. (24 points) Consider the following reaction: Au(s) + NO3(aq) + 4H+ (aq) → NO(g) + 2 H20() + Aul(aq) SHOW ALL WORK: Equations written in symbols first. All conversions. Units on every number. a. (4 points) What is the standard cell potential? b. (5 points) What is the standard free energy change for this cell? (Be sure your answer is in the appropriate units for free energy) c. (2 points) As written would this reaction be the basis for...
1. Consider the reaction below: 3Ag2S(s) + 8H+(aq) + 2NO3-(aq) ? 6Ag+(aq) + 3S(s) + 2NO(g) + 4H2O(l) In this reaction, which species is reduced? 2. Calculate Ecell for the following electrochemical cell which is operating under nonstandard conditions: Cr | Cr3+(0.010 M) || Ag+(0.00010 M) | Ag The relevant standard reduction potentials are: Cr3+(aq) + 3e- ? Cr(s) Eº = ?0.74 V Ag+(aq) + e- ? Ag(s) Eº = +0.80 V
Determine whether or not the reaction indicated will occur spontaneously. 2Cu+(aq) + Ni(s) Ú 2Cu(s) + Ni2+(aq)
. AT&T 8:47 PM 67% Exit In the reaction 3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(aq) + 4H2O(l) + 2NO(g) 6.3 g of Cu and 100.0 mL of 1.0 M HNO3 are combined. Which of the following statements is true? O 0.080 mol H2O is produced O Cu and HNO3 are present in stoichiometric amounts; neither is in excess. O Cu is the limiting reagent, and 0.062 mol HNO3 does not react. O HNO3 is the limiting reagent, and 0.062 mol Cu...
Cu(s) + 8HNO3(aq) → 2NO(g) + 3Cu(NO3)2(aq) + 4H2O(l) If 15 g of copper metal was added to an aqueous solution containing 6.0 moles of HNO3, how many moles of NO(g) would be produced, assuming a 75 % yield.
Calculate Ho for the following equations: a. Zn(s) + 2H+(aq) Zn2+(aq) + H2(g) b. 2H2S(g) + 3O2(g) 2SO2(g) + 2H2O(g) c. 3Ni(s) + 2NO3-(aq) + 8H+(aq) 3Ni2+(aq) + 2NO(g) + 4H2O(l)
Given the following list of half-reaction reduction potentials, identify the reaction that will occur spontaneously as written: Half-reaction E° (V) -0.74 Cr3+ (aq) + 3 e ---> Cr (s) Sn4+ (aq) + 2 e ---> Sn2+ (aq) +0.154 -0.440 Fe2+ (aq) + 2 e ---> Fe(s) Fe3+ (aq) + e ---> Fe2+ (aq) +0.771 2 Cr (s) + 3 Fe2+ (aq) ---> 3 Fe (s) + 2 Cr3+ (aq) 2 Cr3+ (aq) + 3 Sn2+ (aq) ---> 3 Sn4+ (aq)...