Consider the reaction Fe(s) + 2HCl(aq)FeCl2(s) + H2(g) for which H° = -7.400 kJ and S°...

Consider the reaction

Fe(s) + 2HCl(aq)FeCl₂(s) + H₂(g)

for which H° = -7.400 kJ and S° = 107.9 J/K at 298.15 K.

(1) Calculate the entropy change of the UNIVERSE when 2.097 moles of Fe(s) react under standard conditions at 298.15 K.

S_universe = J/K

(2) Is this reaction reactant or product favored under standard conditions?

_________reactantproduct

(3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'.

Expert Solution

Amanda K answered 7 months ago

Hydrochloric acid can dissolve solid iron according to the following reaction. Fe(s)+2HCl(aq)→FeCl2(aq)+H2(g) What minimum mass of...

Hydrochloric acid can dissolve solid iron according to the following reaction. Fe(s)+2HCl(aq)→FeCl2(aq)+H2(g) What minimum mass of HCl in grams would you need to dissolve a 2.5 g iron bar on a padlock? How much H2 would be produced by the complete reaction of the iron bar?

Consider the reaction: FeS(s) + 2HCl (aq) --> FeCl2(aq) + 2H2S(g). A 4.00g sample of FeS...

Consider the reaction: FeS(s) + 2HCl (aq) --> FeCl2(aq) + 2H2S(g). A 4.00g sample of FeS containing nonsulfuide impurities reacted with HCl to give 896mL of H2S at 14C and 782 mmHg.Calculate mass percent purity of the sample. State your final answer using 3 Sig figs

The reaction is: Mg(s) + 2HCl(aq) --> MgCl2 (aq) + H2(g) 1. If 2.016 g of...

The reaction is: Mg(s) + 2HCl(aq) --> MgCl2 (aq) + H2(g) 1. If 2.016 g of hydrogen (H2) was released, how many moles of magnesium reacted? How many grams of magnesium would this be? 2. How many moles of magnesium would replace one mole of hydrogen (H) in the hydrochloric acid? How many grams? (This is the equivalent weight) 3. Compare the mass calculated above in question 2 to your experimental equivalent weight and calculate the percent difference. What would...

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚...

Consider the reaction: Zn(s) + 2 H+(aq) = Zn2+(aq) + H2(g) At 25C, calculate: a) ∆G˚ for the reaction, given that: ∆Gf Zn(s) = 0, ∆Gf(H+) = 0, ∆Gf(H2) = 0, ∆Gf(Zn2+) = -147.1 kj/mol b) ∆G, when P(h2) = 750 mmHg, [Zn2+ aq] = 0.10 M, [H+] = 1.0 x 10^-4 M c) The pH when ∆G - -100 kJ, P(h2) = 0.922 atm, [Zn2+] = 0.200 M and the mass of Zn is 155 g.

Using the balanced equation Mg(s)+2HCl(aq)>MgCl2(aq)+H2(g), what volume of hydrogen would be produced by the reaction of...

Using the balanced equation Mg(s)+2HCl(aq)>MgCl2(aq)+H2(g), what volume of hydrogen would be produced by the reaction of 2.00 g of magnesium with an excess of hydrochloric acid at 746 torr and 26.2°C?

Given : 2HCl(aq) + Mg(s) -> MgCl2(aq) +H2(g) Mg(s) + 1/2 O2(g) -> MgO(s) Mass of...

Given : 2HCl(aq) + Mg(s) -> MgCl2(aq) +H2(g) Mg(s) + 1/2 O2(g) -> MgO(s) Mass of 3.00M HCl (diluted in water) : 88.4g Vol of 3.00M HCl : 87.5mL Mass of Mg : 0.599g Total mass: 88.999g --------------------------------------------------------------------------------------- Find mole of product IF: (show calculations) A. HCl is the limiting reactant: ______ B. Mg is the limiting reactant: ______

Consider the following cell reaction: Fe(s) + 2 H+(? M) Fe2+(1.00 M) + H2(g)(1.00 atm) If...

Consider the following cell reaction: Fe(s) + 2 H+(? M) Fe2+(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.236 volts, what is the pH of the hydrogen electrode? A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ()= 1atm) immersed in a solution of unknown [H+]. If the cell potential is 0.202 V, what is the pH of the unknown solution at 298...

1)For the reaction NH4Cl(aq)--->NH3(g) + HCl(aq) H° = 86.4 kJ and S° = 79.1 J/K The...

1)For the reaction NH4Cl(aq)--->NH3(g) + HCl(aq) H° = 86.4 kJ and S° = 79.1 J/K The equilibrium constant for this reaction at 325.0 K is . Assume that H° and S° are independent of temperature. 2)For the reaction Fe(s) + 2HCl(aq)--->FeCl2(s) + H2(g) H° = -7.4 kJ and S° = 107.9 J/K The equilibrium constant for this reaction at 279.0 K is ____ Assume that H° and S° are independent of temperature.

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) How many...

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl: Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) How many liters of H2 would be formed at 636 mm Hg and 17 ∘C if 27.0 g of zinc was allowed to react? How many grams of zinc would you start with if you wanted to prepare 6.85 L of H2 at 284 mm Hg and 28.5 ∘C?

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl : Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) 1)How...

Hydrogen gas can be prepared by reaction of zinc metal with aqueous HCl : Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) 1)How many liters of H2 would be formed at 592 mm Hg and 17 ∘C if 25.5 g of zinc was allowed to react? 2)How many grams of zinc would you start with if you wanted to prepare 4.60 L of H2 at 294 mm Hg and 34.5 ∘C ?

Question