15. How aralisi disebut....................................................... E) 5.87 g in an acidic solution? of NO_(3)^-(aq) and N((s) when the following redox equation is balanced A) 2,6 B) 3,6 NO_(3)^(1)/(3)(aq)+Ni(s)arrow NO(g)+Ni^2+(aq) C)3,4 D)2,3 17. Give the net ionic cquation for the reaction (if any) that Na_(2)CO_(3) and HCl 1.2 2Na^2(aq)+CO_(3)^2(aq)+2H^+(aq)+2Cl(aq)arrow H_(2)CO_(3))_(2)+CO_(2)(aq)+2Na^+(aq)+2Cr(aq) 2Na^{2 B) C) D) E)No reaction occurs. 18. The titration of 1000 mL of HCl solution of unknown concentration requires 12.54 mL of a0.100M NaOH solution to reach the equivalenc A) 0.278 M B) 0.125 M HCl(aq)+NaOH(aq)arrow H2O(l)+NaCl(aq) 5M ()0.354M D)0.143M 19. How many milliliters of 0.260MNa_(2)S are needed to react with 35.00 mL of 0.315MAgNO_(3) according to the following unbalanced precipitation reaction? E) 0.0125 M A) 21.2 mL Na_(2)S(aq)+AgNO_(3)(aq)arrow NaNO_(3)(aq)+Ag_(2)S(s) B)57.8mL D) 84.8 mL E) 35.6 mL 20. Determine the theoretical yield of H_(2)S (in moles) if 32 mol Al_(2)S_(3) and 32molH_(2)O are reacted according to the following balanced reaction. A possibly useful molar mass is Al_(2)S_(3)=150.17g/mol Al_(2)S_(3)(s)+6H_(2)O(l)arrow 2Al(OH)_(3)(s)+3H_(2)S(g) A) 16molH_(2)S B) 96molH_(2)S C) 48molH_(2)S D) 32molH_(2)S E) 64molH_(2)S 21. How many grams of NaCl are required to make 250.00 mL of 3.000 M solution? (Na:22.99g/mol,Cl: 35.45g/mol) A)58.40 g B) 43.83 g C) 175.3 g D) 14.60 g E) 1288 22. What is the concentration of a solution prepared by diluting 20.0 mL of a 0.200MLiCl to 250.0 mL A) 0.0160 M B) 0.160 M C) 2.50 M D) 0.00800 M E) 0.0320 m 23. What is the oxidation. "tate of H in H_(2)(g) in th; following belanced reaction? Mg(s)+2HBr(aq)arrow MgBr_(2)(aq)+H_(2)(g) D) A) +1 B) +2 C) 0 -1 E) -2 4. What is the oxidizing reaction? 2Al^3(aq)+2Fe(s)arrow 2Al(s)+3Fe^2+(aq) C) Al D) Fe^2+ A) Al^3+ B) Fe E) none 5. Determine the limiting reactant (LR) and the mass (ing) of nitrogen that can be formed from 50.0g below. Some possibly useful atomic a. masyarakat dangkat dan A E) No LR,45.0gN_(2) formed

15. How many moles of and are involved in the redox reaction?A) 2,6B) 3,6C) 3,4D) 2,3E) 5,87 gTo balance the redox equation, we need to determine the number of moles of and involved in the reaction. From the given equation, we can see that the oxidation state of nitrogen changes from 0 in to +5 in . Therefore, the number of moles of involved in the reaction is 5.Similarly, the oxidation state of nitrogen changes from +5 in to 0 in . Therefore, the number of moles of involved in the reaction is 3.Therefore, the correct answer is B) 3,6.17. Give the net ionic equation for the reaction between and .A) B)C)D)E) No reaction occurs.The net ionic equation for the reaction between and is: This equation represents the formation of carbonic acid and carbon dioxide gas from the reaction of carbonate ions and hydrogen ions.18. The titration of 10.00 mL of solution of unknown concentration requires 12.54 mL of solution to reach the equivalence point. What is the concentration of the solution?A) 0.278 MB) 0.125 MC) 0.354 MD) 0.143 MTo find the concentration of the solution, we can use the formula: where and are the molarity and volume of the solution, and and are the molarity and volume of the solution.Substituting the given values, we have: Solving for , we get: Therefore, the concentration of the solution is B) 0.125 M.19. How many milliliters of are needed to react with 35.00 mL of according to the following unbalanced precipitation reaction? A) 21.2 mLB) 57.8 mLC) 84.8 mLD) 35.6 mLTo find the volume of needed, we can use the formula: where and are the molarity and volume of the solution, and and are the molarity and volume of the solution.Substituting the given values, we have: Solving for , we get: Therefore, the correct answer is D) 35.6 mL.20. Determine the theoretical yield of in moles if 32 mol and 32 mol are reacted according to the following balanced reaction: