This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Let's knock this out. Problem 1: Step 1: Determine the charge required to liberate 1.98 g of copper. From the given information, 1 C of charge liberates 0.0033 g of copper. We can set up a proportion: Mass liberatedCharge = constant 0.0033 g1 C = 1.98 gQ Solving for Q: Q = 1.98 g × 1 C0.0033 g Q = 600 C Step 2: Calculate the time taken. The relationship between charge (Q), current (I), and time (t) is Q = I × t. We are given I = 2 A and we calculated Q = 600 C. t = (Q)/(I) t = 600 C2 A t = 300 s Step 3: Convert the time from seconds to minutes. t = 300 s × 1 minute60 s t = 5 minutes The correct option is 5 minutes. 5 minutes Problem 2: Step 1: Calculate the mass of the substance deposited. The mass deposited (m) is the difference between the final and initial mass of the cathode. m = m_final - m_initial m = 5.01 g - 5 g m = 0.01 g Step 2: Calculate the electrochemical equivalent (Z). According to Faraday's First Law of Electrolysis, the mass deposited (m) is given by the formula: m = ZIt Where: m = 0.01 g I = 5 A t = 50 s Rearrange the formula to solve for Z: Z = (m)/(It) Substitute the values: Z = 0.01 g(5 A) × (50 s) Z = 0.01 g250 A s Z = 0.00004 g/C The electrochemical equivalent of the deposited substance is 0.00004 g/C. 0.00004 g/C Send me the next one 📸