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A: Let the oxidation state of S be x. The value of x can be calculated as follows-
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Q: Give the oxidation state of sulfur in (a) S₈; (b) SF₄; (c) SF₆;(d) H₂S; (e) FeS₂; (f) H₂SO₄; (g)…
A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…
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Q: How many coulomb will it take to plate out 11.2g of fe from a solution FeCl2?
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Q: Describe how to determine the oxidation number of sulfur in(a) H₂S and (b) SO₃²⁻.
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Q: 17. Which is the oxidizing agent in, 2C0 + 2NO → 2CO2 + N?
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Q: (b) A metallurgical laboratory carried out analysis of a sample in which analysis of Mn was done by…
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- Write balanced chemical equations for the following reactions: (a) zinc metal heated in a stream of oxygen gas (b) zinc carbonate heated until loss of mass stops (c) zinc carbonate added to a solution 0f acetic acid, CH3CO2H (d) zinc added to a solution of hydro-bromic acid4.22 Generally, an excess of O2 is needed for the reaction Sn+O2SnO2 . What is the minimum number of moles of oxygen required to oxidize 7.3 moles of tin?A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with excess silver nitrate. The resulting precipitate, filtered and dried, weighs 3.03707 g. What was the percent by mass of chloride ion in the original compound? What is the identity of the salt?
- Write “true” or “false” for each statement. (a) We balancechemical equations as we do because energy must be conserved.(b) If the reaction 2 O3(g)S 3 O2(g) goes to completionand all O3 is converted to O2, then the mass of O3 atthe beginning of the reaction must be the same as the massof O2 at the end of the reaction. (c) You can balance the“water-splitting” reaction H2O(l)S H2(g) + O2(g) by writingit this way: H2O2(l)S H2(g) + O2(g).1. If 30.4 g of Nal (MM=149.89g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of Nal in the resulting solution? 2. What volume (in L) of 1.1 M FeCl3 would be required to obtain 0.59 moles of Cl- ions?a) What mass of strontium nitrate (Sr(NO3)2) would be required to prepare 2.000 L of a 0.0180 M aqueous solution of this salt? (b) Calculate the mass percent of Sr(NO3)2 in this solution, assuming the density of the solution is 1.000 kg/L. c.) A 15.0 g sample of anhydrous sodium sulfate, Na2SO4, is dissolved in 4.83 L of water. The molar mass of sodium sulfate is 142.1 g/mol. Use the equation given to calculate the molality (m) of the solution, in mol/kg.For this situation, assume the density of water is 1.00 g/mL.
- (a) Write chemical equations to show what happens when each of the following substances is mixedwith water:(i) Hydride ion(ii) Glucose, C6H12O6(s)(iii) Copper(II) bromide(iv) Formic acid(b) Write chemical equations for the following processes:(i) Chemical reaction for ΔH°f for mercury(I) phosphate.(ii) Thermal dissociation of gaseous bromine.(iii) Sublimation of carbon dioxide.(iv) Reduction of VO2+ to produce VO2+.(v) Neutralization of sulfuric acid by barium hydroxide.(vi) Thermal decomposition of 1 mol of sodium bicarbonate to produce sodium carbonate, carbon dioxide and waterReacting water with magnesium nitride produces ammonia (NH3) and magnesium hydroxide. If this process is 70% efficient, what mass of ammonia (in kg) can be prepared from 19.5 kg of magnesium nitride?What mass of a 30% (w/w) hydrogen peroxide solution is required to provide the mass 3.0618 for a 25.00 mL of a solution containing 3.6 M H2O2 (a w/w solution means g solute/100 g solution)?
- The accompanying photo shows the reaction between asolution of Cd1NO322 and one of Na2S. (a) What is the identityof the precipitate? (b) What ions remain in solution?(c) Write the net ionic equation for the reaction. (d) Is this aredox reaction?How many grams of O2 will be formed from 3.76 grams of KClO3?How many ions can you get in solution from 123.1 grams of MoCl3?
