What concentration of Zn^{2+} is present in solution when 5.64 g of zinc metal is used...

What concentration of Zn^{2+} is present in solution when 5.64 g of zinc metal is used to displace hydrogen from 118 mL of 0.661 M HCl(aq)?

Expert Solution

queen_honey_blossom answered 2 years ago

Consider the reaction that results from the addition of 50.0 g of Zinc metal (Zn) to...

Consider the reaction that results from the addition of 50.0 g of Zinc metal (Zn) to 60.0 g of hydrochloric acid (HCl)? Generate a balanced equation for this reaction and then answer the folling (3) questions. 1) What is the limiting reactant? A) zinc B) hydrochloric acid C) zinc chloride D) hydrogen gas E) hydrogen gas 2) How much hydrogen gas forms? A) 2.68g B) 0.77g C)0.83g D) 8.35g E) 1.55g 3) How much excess reagent is left over? A)...

Zinc (Zn) metal reacts with hydrochloric acid (HCl) according to the following reaction: Zn(s) + 2...

Zinc (Zn) metal reacts with hydrochloric acid (HCl) according to the following reaction: Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g)What volume of H2 gas would be collected over water if 6.93 g Zn metal were allowed to react with 25.0 mL of 1.0 M HCl at 25.0 oC? The vapour pressure of water at 25.0 oC is 23.8 torr, and the pressure of the laboratory is 1.00 atm

-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g of...

-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g of an unknown compound of bismuth and chlorine. The reaction results in the formation of zinc chloride and metallic bismuth. When the reaction is complete, unreacted zinc remains, and this unreacted zinc is consumed by reaction with HCl. After washing and drying, the mass of bismuth metal recovered is 0.6763g. Q. Write a balanced chemical equation for the reaction of zinc with the original unknown...

Q.-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g...

Q.-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g of an unknown compound of bismuth and chlorine. The reaction results in the formation of zinc chloride and metallic bismuth. When the reaction is complete, unreacted zinc remains, and this unreacted zinc is consumed by reaction with HCl. After washing and drying, the mass of bismuth metal recovered is 0.6763g -- Calculate the experimental % of bismuth in the original unknown compound -- If...

Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.107 g...

Zinc metal reacts with hydrochloric acid according to the following balanced equation. Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g) When 0.107 g of Zn(s) is combined with enough HCl to make 54.9 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.0 ∘C to 24.0 ∘C. Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g⋅∘C as the specific heat capacity.)

Consider the reaction between the zinc metal (Zn) and hydrochloric acid (HCl), 2HCl (aq) + Zn...

Consider the reaction between the zinc metal (Zn) and hydrochloric acid (HCl), 2HCl (aq) + Zn (s) → ZnCl2 (aq) + H2 (g). How many grams of hydrogen gas (H2) are possible when 0.500 grams of Zn is added to 250 mL of a 0.123 M HCl solution? (Answer: 0.0154 grams of H2) Please give a step by step explanation. Answer is given above

what concentration of Zn^2+ will remain when 200mL of 4.50*10^-3 M Zn(NO3)2 is combined with 200.0mL...

what concentration of Zn^2+ will remain when 200mL of 4.50*10^-3 M Zn(NO3)2 is combined with 200.0mL of .250 M NaOH? Kf of Zn(OH)4 ^2- = 2.0*10^15

11. Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn (s) +...

11. Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn (s) + 2 HCl (aq)  ZnCl2 (aq) + H2 (g) When 0.103 g of Zn (s) is combined with enough HCl to make 50.00 mL of solution in a coffee cup calorimeter, all of the zinc reacts raising the temperature of the solution from 22.50 oC to 23.70 oC. Calculate Hrxn in kJ/mol of Zn. (Assume that density of the solution = 1.00 g/mL and...

When the nickel-zinc battery, used in digital cameras, is recharged, the following cell reaction occurs: 2Ni(OH)2(s)+Zn(OH)2(s)→...

When the nickel-zinc battery, used in digital cameras, is recharged, the following cell reaction occurs: 2Ni(OH)2(s)+Zn(OH)2(s)→ 2Ni(OH)3(s)+Zn(s) How many grams of zinc are formed when 3.39×10−2 g of Ni(OH)2 are consumed? How many minutes are required to fully recharge a dead battery that contains 6.13×10−2 g of Zn with a constant current of 0.100 A? Thank You!!

A) Calculate the concentration of zinc (II) ions in a solution containing 0.20 M hexaammine zinc(II)...

A) Calculate the concentration of zinc (II) ions in a solution containing 0.20 M hexaammine zinc(II) ion and 0.0116 M ammonia at equilibrium. The Kf of [Zn(NH3)4]^2+ is 2.8*10^9. B) Calculate the solubility of lead (II) sulfate in a 0.0034 M solution of sodium sulfate. The Ksp for lead(II) sulfate is 1.83*10^-8.

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