Answer 8b please simple and clear please N 17%11:34OCR A Chemistry .kerboodle.comOCR A Ch© Oxford University Press | Help8.Chlorinegasis prepared by the electrolysisof brine, a concentrated solution of sodiumchloride in water.2NaCl + 2H,O2NaOH + Cl, + H,The concentration of brine can be assumed tobe 4.00 mol dm-3.aCalculate the mass of sodium chloridedissolved in 250 cm3 of brine.(1 mark)b Each day, the UK produces 2.5 x 10° dm3of chlorine gas, at RTP, from brine.Calculate the volume of brine required forchlorine production each day in the UK.(3 marks)An organic compound X, contains carbon,hydrogen and oxygen only. Compound Xhas the following percentage compositionby mass: 54.55%, C; 9.09% H.9.a(i) Calculate the empirical formula of X.(2 marks)(ii) In an experiment, 0.2103g of avaporised sample of X was shownto occupy 72.0 cm³ at 100°C and103.0kPa.Calculate the relative molecular.Resources

Concentration of brine solution = 4.0 mol .dm-3 Volume of Cl2 used = 2.5 × 109 dm3

Chlorine gas is prepared by the electrolysis of brine, a concentrated solution of sodium chloride in water. 2NaCl + 2H,0 2NAOH + CI, + H, The concentration of brine can be assumed to be 4.00 mol dm-3. a Calculate the mass of sodium chloride dissolved in 250 cm3 of brine. (1 mark) b Each day, the UK produces 2.5 x 10° dm3 of chlorine gas, at RTP, from brine.

Chlorine gas is prepared by the electrolysis of brine, a concentrated solution of sodium chloride in water. 2NaCl + 2H,0 2NAOH + CI, + H, The concentration of brine can be assumed to be 4.00 mol dm-3. a Calculate the mass of sodium chloride dissolved in 250 cm3 of brine. (1 mark) b Each day, the UK produces 2.5 x 10° dm3 of chlorine gas, at RTP, from brine.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 8RQ

See similar textbooks

Similar questions

An active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Consider the electrolysis of NiCl2 to Ni(s) and Cl2(g). (a) What is the minimum voltage required to carry out this reaction at standard conditions? (b) If a voltage of 3.0 V is actually used, and 10.00 kJ of energy are consumed, how many grams of Ni(s) are obtained? (1J=1volt-coulomb)
Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 C. Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s) a. Write a balanced equation for the reaction that occurs at the cathode. b. Write a balanced equation for the reaction that occurs at the anode. c. Write a balanced chemical equation for the overall reaction. d. Determine the potential (in volts) of the cell.
13.106 Hydrazine, N2H4 , has been proposed as the fuel in a fuel cell in which oxygen is the oxidizing agent. The reactions are N2H4(aq)+4OH-(aq)N2(g)+4H2O(l)+4eO2(g)+2H2O(l)+4e4OH-(aq) (a) Which reaction occurs at the anode and which at the cathode? (b) What is the net cell reaction? (C) If the cell is to produce 0.50 A of current for 50.0 h, what mass in grams of hydrazine must be present? (d) What mass in grams of O2 must be available to react with the mass of N2H4 determined in part (c)?
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?