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Volume of gas evolved in electrolysis

This type of question, asked 2 times: 29 Jun 2022, 24 Jan 2026 S1. All 2 questions below, oldest first.

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  1. Question 1

    29 Jun 2022

    54
    A dilute solution of sulphuric acid is electrolysed using a current of 0.10 A0.10\text{ }A for 2 hours to produce hydrogen and oxygen gas. The total volume of gases produced at STP is ____ cm3\_\_\_\_\ cm^{3}. (Nearest integer) [Given: Faraday constant F=96500CF = 96500C mol−1mol^{- 1} at STP, molar volume of an ideal gas is 22.7 L mol−122.7\text{ }L{\text{ }mol}^{- 1} ]

  2. Question 2

    24 Jan 2026 S1

    46
    Electricity is passed through an acidic solution of Cu2+{Cu}^{2 +} till all the cu2+{cu}^{2 +} was exhausted, leading to the deposition of 300 mg of Cu metal. However, a current of 600 mA was continued to pass through the same solution for another 28 minutes by keeping the total volume of the solution fixed at 200 mL . The total volume of oxygen evolved at STP during the entire process is ____\_\_\_\_ mL. (Nearest integer) [Given : Cu2+(aq)+2e−→Cu(s)Ered 0=+0.34 V{Cu}^{2 +}(aq) + 2e^{-} \rightarrow Cu(s)E_{\text{red~}}^{0} = + 0.34\text{ }V O2( g)+4H++4e−→2H2OEred 0=+1.23 VO_{2}(\text{ }g) + 4H^{+} + 4e^{-} \rightarrow 2H_{2}OE_{\text{red~}}^{0} = + 1.23\text{ }V Molar mass of Cu=63.54 g mol−1Cu = 63.54\text{ }g{\text{ }mol}^{- 1} Molar mass of O2=32 g mol−1O_{2} = 32\text{ }g{\text{ }mol}^{- 1} Faraday Constant =96500Cmol−1= 96500C{mol}^{- 1} Molar volume at STP=22.4 LSTP = 22.4\text{ }L ]