Question

In: Chemistry

Consider these reactions, where M represents a generic metal 1. 2M(s)+6HCl(aq)------>2MCl3(aq)+3H2(g) Delta H1=-749.0 KJ 2. HCl(g)------->HCl(aq)...

Consider these reactions, where M represents a generic metal

1. 2M(s)+6HCl(aq)------>2MCl3(aq)+3H2(g) Delta H1=-749.0 KJ

2. HCl(g)------->HCl(aq) Delta H2=-74.8 KJ

3. H2(g)+Cl2(g)------->2HCl(g) Delta H3=-1845.0 KJ

4. MCl3(s)-------->MCl3(aq) Delta H4=-298.0 KJ

Use the information above to determine the enthalpy of the following reaction.

2M(s)+3Cl2(g)----->2MCl3(s) Delta H=???

Expert Solution

2M(s)+6HCl(aq) -----> 2MCl₃(aq)+3H₂(g) : ΔH₁ = -749.0 KJ ----(1)

HCl(g) -----> HCl(aq) ; ΔH₂ = -74.8 KJ ----(2)

H₂(g)+Cl₂(g) -----> 2HCl(g) ; ΔH₃ = -1845.0 KJ ----(3)

MCl₃(s) ------> MCl₃(aq) : ΔH₄ = -298.0 KJ ----(4)

Use the information above to determine the enthalpy of the following reaction.

2M(s)+3Cl₂(g) -----> 2MCl₃(s) ΔH= ? ----(5)

Equ(5) can be obtained from remaining four equations as follows:

Eqn(5) = Eqn(1) + [6xEqn(2)]+[3xEqn(3) ] + [2xreverse of Eqn(4)]

ΔH= ΔH₁ +(6xΔH₂ ) + (3xΔH₃ ) + (2x(-ΔH₄ )

= -749 + (6x(-74.8)) + (3x(-1845)) + (2x(-(-298))) kJ

= -6136.8 kJ

queen_honey_blossom answered 5 months ago

Consider these reactions where M represents a generic metal: 2M(s) + 6HCl(aq) ---->2MCl3(aq) + 3H2(g) Delta...

Consider these reactions where M represents a generic metal: 2M(s) + 6HCl(aq) ---->2MCl3(aq) + 3H2(g) Delta H1 = -569kj HCl(g) ----> HCl(aq) DeltaH2 = -74.8 H2(g) + Cl2(g) ----> 2HCl(g) Delta H3 = -1845kj MCl3(s) ----> MCl3(aq) Delta H4 = -405kj Use the above information to determine the enthalpy of the following reaction: 2M(s) + 3Cl2(g) ----> 2MCl3(s) What is Delta H for this reaction?

2. Consider the following three reactions: 2 Fe (s) + 6HCl (aq) → 2 FeCl3 (aq)...

2. Consider the following three reactions: 2 Fe (s) + 6HCl (aq) → 2 FeCl3 (aq) + 3 H2 (g) ΔHA Fe2O3 (s) + 6HCl (aq) → 2 FeCl3 (aq) + 3 H2O (l) ΔHB 2H2 (g) + O2 (g) → 2 H2O (l) ΔHC a. Show how these equations must be summed together according to Hess’s Law to determine ∆H for the combustion of iron (target equation shown below). Also show clearly how the ∆H values of each of...

Consider the equilibrium CH4(g) + H2O(g) <--> CO(g) + 3H2(g), where delta h= 206 KJ. Which...

Consider the equilibrium CH4(g) + H2O(g) <--> CO(g) + 3H2(g), where delta h= 206 KJ. Which of the following disturbances will NOT cause the system to shift to the right to reestablish equilibrium? A.) The partial pressure of CH4 increases. B.) The partial pressure of CO decreases. C.) The volume decreases. D.) The temperature increases. E.) All of these will cause the system to shift to the right.

Given these reactions, X(s) + 1/2 O2(g) -----> XO(s) Delta H = -699.3 kJ/mol XCO3(s) ------->...

Given these reactions, X(s) + 1/2 O2(g) -----> XO(s) Delta H = -699.3 kJ/mol XCO3(s) -------> XO(s) + CO2(g) Delta H = +328.3 kJ/mol what is Delta Hrxn for this reaction? X(s) + 1/2 O2(g) + CO2(g) -------> XCO3(s) Delta H = kJ/mol

2X(s) + 6HCl (aq) ----> 2 XCl3 (aq) + 3 H2(g) a. Which reactant is oxidized...

2X(s) + 6HCl (aq) ----> 2 XCl3 (aq) + 3 H2(g) a. Which reactant is oxidized and which reactant is reduced? (Please explain) b. To prepare a HCl solution, 12.0 M concentrated HCl was diluted with water to make 250 mL of a 4.00 M HCl solution. How much, in mL, of concetrated acid was used? c. In an experiment, it was found that 25 mL of the diluted acid was required to react completely with the 4.80 g of...

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.

Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. M(0H)2 yields M+2OH M(OH)2 +2OH...

Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. M(0H)2 yields M+2OH M(OH)2 +2OH yields (M(OH4)2- Ksp=3x10^-16 Kf= .05 Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0.

What are the reactions for the following? Using (molecular, ionic, net-ionic) 1. Ca(s)+HCl(aq) 2. Mg(s)+HCl(aq) 3....

What are the reactions for the following? Using (molecular, ionic, net-ionic) 1. Ca(s)+HCl(aq) 2. Mg(s)+HCl(aq) 3. Fe(s)+HCl(aq) 4. Cu(s)+HCl(aq) 5. Zn(s)+HCl(aq) 6. Sn(s)+HCl(aq)

Consider the given reaction. MgCO3(s) + 2 HCl(aq) — MgCl2(aq) + H2O(l) + CO2(g)

Consider the given reaction. MgCO3(s) + 2 HCl(aq) — MgCl2(aq) + H2O(l) + CO2(g) Calculate the atom economy of this reaction to form carbon dioxide assuming that no other reactions are occurring. atom economy = _______ %

Suppose you are investigating the reaction: M(s) + 2 HCl(aq) → MCl2(aq) + H2(g). You weigh...

Suppose you are investigating the reaction: M(s) + 2 HCl(aq) → MCl2(aq) + H2(g). You weigh out a 0.250 gram piece of metal and combine it with 72.9 mL of 1.00 M HCl in a coffee-cup calorimeter. If the molar mass of the metal is 42.29 g/mol, and you measure that the reaction absorbed 155 J of heat, what is the enthalpy of this reaction in kJ per mole of limiting reactant? Enter your answer numerically to three significant figures...