Silver metal reacts with sulfur to form silver sulfide according to the following reaction: 2Ag(s) + S(s) → Ag,S(s) w w m. Step 1. Analyze the problem. Step 2. Determine the limiting reagent.
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Please answer 1-2 sub-units thank you
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- Write the equation for the reaction, if any, that occurs when each of the following experiments is performed under standard conditions. (a) Sulfur is added to mercury. (b) Manganese dioxide in acidic solution is added to liquid mercury. (c) Aluminum metal is added to a solution of potassium ions.Balance the reaction between Fe2+ and MnO4- to form Fe3+ and Mn2+ in acidic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown. Fe2+ + MnO4- Fe3+ + Mn2+Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)How many electrons are transferred in this reaction?Calculate the theoretical yield of isopentyl acetate for the esterification reaction. If you started with 8.0 mL of isopentyl alcohol and 8.0 mL glacial acetic acid in this reaction, which substance would be your limiting reactant? isopentyl alcohol- quantity: 4.37 g molar mass (g/mol): 88.15 acetic acid- quantity: 8.0 mL molar mass: 60.05 8.0mL of isopentyl alcohol isopentyl acetate (product)- molar mass:88.15
- Upon completion of an experiment involving a reaction between copper wire, Cu(s), and aqueous silver nitrate, AgNO3(aq), to produce silver, Ag(s), some copper wire remained in the reaction vessel. What describes the role of AgNO3(aq) in the reaction? a) dehydrator. b) excess. c) limiting. d) residual.For all of the following experiments, under standard conditions, which species could be spontaneously produced? (a) A lead wire is placed in a solution containing Cu2+ No reaction. YES or NO Cu. YES or NO PbO2. YES or NO (b) Crystals of I2 are added to a solution of NaCl. No reaction. YES or NO I^-. YES or NO Na. YES or NO (c) Cl2 gas is bubbled into a solution of NaI. Cl^-. YES or NO No reaction. YES or NO Na. YES or NOBalance each chemical reaction below, the combine (add) the two balanced reactions and write an overall balance chemical reaction for the two step process obtaining copper metal from chalcocite. Hint: you may need to double one of the balanced reactions before adding them. "Roasting, extraction of copper from Chalcocite" Cu2S(s) + O2(g) --> Cu2O(s) + SO2(g) "Obtaning Copper Metal" Cu2O(s) + C(s) --> Cu(s) + 2CO(g)
- 17. Consider the reaction of 0.161 g of aluminum metal with 50.0 mL of 0.235 M Co(NO₃)₂. a. Which metal, Al or Co, is more easily oxidized? b. Write the balanced chemical equation that occurs for the oxidation reaction. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction. c. What quantity in moles of Co(NO₃)₂ do you start with? d. What quantity in moles of metal product are generated if all of the Co(NO₃)₂ is consumed? e.What quantity in moles of Al do you start with? f. What quantity in moles of metal product are generated if all of the Al is consumed? g. Which reactant is limiting? h. What mass (in grams) of metal is formed when the limiting reactant is considered?1. How many metric tons of charcoal is required to reduce 1500 kg of arsenic trioxide?AS2O3 + C = CO + As 2. The Le Blanc Process for the manufacture of soda ash encompasses the four steps:NaCl + H2SO4 = NaHSO4 + HClNaHSO4 + NaCl = Na2SO4 + HClNa2SO4 + C = Na2S + CO2Na2S + CaCO3 = Na2CO3 + CaSHow many tonnes of soda ash are produced per 5 tonnes of salt? How many kg of C are required?A student Investigated the stoichiometry of the reaction of zinc (Zn) and HCl solution and reported the following data. When 0.2158 g of Zn reacted with 10.00 ml of 1.000M HCl, 82.062 g of water was displaced. A total of 36.00 ml of 9.501 x 10-2M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. Calculate the volume of the displaced water from its mass (which will be equal to the volume of the gas collected.) 2) Calculate the pressure of the H2 collected 3) Calculate the number of moles of H2 collected using the ideal gas equation. 4)calculate the number of moles of hcl remaining in the flask at the end of the reaction 5) caluxukage the number of miles of hcl originally present in the reaction 6) calculate the number of moles hcl reacting 7) ccalculate the number of moles zn reacting 8) calculate the ratio of the number of hcl reacting to the number of…
- Balance this reaction. If a coefficient is one, enter "1" explicitly. HCl + Ca(OH)2 → H2O + CaCl2Balance this reaction HNO2 (aq) + Hg(l) ↔ NO (g) + Hg2+ (aq). What is the equilibrium constant for this reaction?Consider the chemical reaction 4 K(s) + O2(g) ──> 2 K2O(s) The molar mass of K is 39.10g/mol, and that of O2 is 32.00g/mol. Without performing any calculations, pick the conditions under which potassium is the limiting reagent and explain your reasoning. 170g K, 31g O2 36g K, 2.5g O2 365kg K, 28kg O2 1.5g K, 0.38g O2