4. Answer the following questions for the reaction below Mg (s) + HCl (aq)MgCl2 (aq) + H2(g) Balance the equation (SHOW...
What species is the reducing agent in the following equation? Mg(s) + 2HCl (aq) --> MgCl2(aq) + H2(g) (assume Cl has an Oxidation number =-1) a)H^+(aq) b) Mg^2+(aq) c)Cl^-(aq) d)Mg(s) e) H2(g)
Consider the following reaction: Mg (s) + 2 HCl (aq) → MgCl2 (aq) + H2 (g) ΔHrxn = –4.6 × 102 kJ a. Is this reaction endothermic or exothermic? Circle one. [1] b. How much heat is evolved when 1.37 g of Mg are dissolved in excess HCl? [5] c. If 1.37 g of Mg are dissolved in enough HCl to make 250.0 mL of solution in a coffee-cup calorimeter, what is the final temperature of the solution? (Assume density...
Which of the following is true concerning the following reaction? 2CI+(aq) + F2(g) + Cl2(g) + 2F"(aq) O CI+(aq) is reduced and is the oxidizing agent and F2(g) is oxidized and is the reducing agent. O Cl2(g) is oxidized and is the reducing agent and F2(g) is reduced and is the oxidizing agent. O Cl(aq) is oxidized and is the reducing agent and F2(g) is reduced and is the oxidizing agent. O None of these choices is correct O Cl(aq)...
Consider the following reaction: 2 HCl(aq) + 1 Mg(s) → 1 MgCl2(aq) + 1 H2(g) ΔH°rx = -465.8 kJ Determine the amount of heat released, in kJ, of each of the following scenarios. Give each answer to 2 decimal places. (a) 10.69 g of Mg(s) is reacted with excess HCl(aq)· (c) 1.17 g of H2(g) is produced from the reaction after completion. (b) Excess Mg(s) is added to 440 mL of 0.996 M of HCl(aq)· (d) 580 mL of a...
HNO3 (aq) + Cu (s) + H2(g) + CuNO3 (aq) •Identify what type of reaction it is: precipitation, redox or acid-base. •Balance the above equation. •Write the balanced net ionic equation. d. Indicate the element that has been oxidized and the one that has been reduced. You should also identify the oxidation number (ox #) of each before and after the process. Identify the reducing agent and the oxidizing agent. Element Oxidized: Ox # Reactant: Ox # Product: Element Reduced:...
7) In the following reaction, Mg(s) + Cu²+ (aq) → Mg2+ (aq) + Cu (s): A) Mg is the reducing agent and Cu is the oxidizing agent. B) Mg²+ is the reducing agent and Cu is the oxidizing agent. C) Cu is the reducing agent and Mg?is the oxidizing agent. D) Cu²+ is the reducing agent and Mg is the oxidizing agent. E) Mg is the reducing agent and Cuis the oxidizing agent. 8) In the following reaction, Zn (s)...
Complete and balance the reaction below: Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (s) How many moles of H2 gas will be produced from 2 mol of HCl ? 2HCl ---à H2 + Cl2 1 mol of H2 gas will be produced from 2 moles HCl. How would you determine the volume of a 125mL Erlenmeyer flask that you will use for the experiment? (a 125 mL flask does not have a total volume of 125 mL)...
QUESTION 4 In the following reaction, Mg(s) + + Cu2+ (aq) → Mg2+ *(aq) + Cu(3) Mg is the reducing agent and Cu is the oxidizing agent. O Cu is the reducing agent and Mg2+ is the oxidizing agent. Mg2+ is the reducing agent and Cu is the oxidizing agent. O Mg is the reducing agent and Cu2+ is the oxidizing agent. is the reducing agent and Mg is the oxidizing agent. O QUESTION 5 Which of the following diatomic...
4) Consider the following balanced conventional equation. (21 pts) Zn(s) + H2SO, (aq) → Znso. (aq) + H2 (9) Individual oxidation numbers: a. Assign oxidation numbers to each element as indicated by the boxes in H SO, Zn in ZnSOS in Znso. O in ZnSO, and H in H2) (6 pts) b. Write the total ionic equation for the reaction above. (9 pts) ndicated by the boxes above. (i.e. Zn in Zn(s), H c. Write the net ionic equation for...
Consider the following balanced chemical equation. Mg(s) + 2 HCl(aq) → MgCl2 (aq) + H2 (8) When 61.42 mL of 1.44 M HCl reacts at 1.14 atm and 315 K, what volume (in L) of H2 forms?