What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of 2.58 A in 16.8 min? H₂(g) 0₂(9) L

Q: How many moles of oxygen, O2, will be produced by the electrolysis of water with a current of 1.5…

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Q: What volumes of H2 (g) and O2 (g) at STP are produced from the electrolysis of water by a current of…

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Q: How many hours are required to produce 115 g of Iron metal from the electrolysis of molten FeCl3…

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Q: An electrolytic cell contans 50.0 mL of a 0.152 M solution of FeCl3. A current of 0.775 A is passed…

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Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: Amount of charge (Q) = I . t  where I = current and t = time

Q: A 5.77 g of zinc is deposited at the cathode when a current of 7.1 amperes passes through an…

A: Given : Current = 7.1 A And time = 40 min = 40 X 60 = 2400 s…

Q: An electrolysis cell is set up with the cathode producing H₂ gas and with an unknown metal at the…

A: Electrolysis Electrolysis involves passing an electric current through either a molten salt or an…

Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

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Q: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: Aluminum metal can be made from aluminum ions by electrolysis. What is the half-reaction at the…

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Q: Electrolysis of an NaCl solution with a current of 2.00 A for a period of 200 s produced 59.6 mL of…

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Q: In the commercial preparation of aluminum, aluminum oxide, Al,O3, is electrolyzed at 1000°C. (The…

A: Since from the above reaction we can see that 1 mole of Al is produced when 3 moles of electrons is…

Q: A steady current was passed through molten CoSO. until 2.35 g of metallic cobalt was produced.…

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Q: Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold…

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Q: Rhodium is a bright, hard, and highly reflective metal. It is most commonly used to plate white gold…

A: To find out the oxidation state, first find out the moles of e- and the moles of the rhodium. Then…

Q: Calcium metal can be obtained by the direct electrolysis of molten , at a voltage of 3.2 volts. How…

A: Given voltage = 3.2 V Atomic weight of Calcium = 40.078 g/mol

Q: What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given ,

Q: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

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Q: Aluminum metal can be made from aluminum(III) ions by electrolysis. What is the half-reaction at the…

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Q: A solution containing vanadium (chemical symbol V) in an unknown oxcidation state was electrolyzed…

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Q: Chlorine gas is used in the production of many other chemicals, including carbon tetrachloride,…

A: Given: Volume of chlorine gas produced at STP = 5.9 ✕ 105 L Known: Molar mass of NaCl = 58.44 g/mol

Q: Calculate the number of grams of aluminum produced in one hour by the electrolysis of molten…

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Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: According to Faraday's 1st law weight of the substance from in each electrolyte  W = ZIt where , W…

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A: From Faradays First law of electrolysis,  the amount of the substance deposited(W) at the given…

Q: What is the time required to produce 45.0 g of Cl2 gas from Cl- using 50.0 A of current?

A: The oxidation reaction taking place will be  2 Cl- -------> Cl2 + 2 e-  Given : mass of Cl2 to…

Q: Aluminum is produced commercially by the electrolysis of Al203 in the presence of a molten salt. If…

A: Total current, I = 1.09 million Ampere                           = 1.09×106 Ampere Time, t = 3 hr…

Q: Chemistry Question

A: 1. Select the principle carbon chain 2. Numbering 3. Naming (prefix + word root + suffix)

Q: How many moles of hydroxide ion will be produced at the cathode during the electrolysis of water…

A: The given cathode reaction is: 2H2O + 2e- → H2 + 2OH- The balanced equation shows that for every 2…

Q: Calculate the mass of chlorine in grams that can be produced by the electrolysis of 50.0 kg of…

A: The electrolysis of sodium chloride takes place as follows: 2NaCl(aq) + 2H2O(l) → 2NaOH(aq)+ Cl2(g)+…

Q: Mass =

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Q: A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper II)…

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Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: Using farday's law of electrolysis we can solve this problem.

Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: A numerical problem based on Faraday's law, which is to be accomplished.

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

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Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.