Textbook Question
A concentration cell consists of two Sn/Sn2+ half-cells. The cell has a potential of 0.10 V at 25°C. What is the ratio of the Sn2+ concentrations in the two half-cells?
2408
views
2
rank
Ch.19 - Electrochemistry
Chapter 19, Problem 84
What mass of lead sulfate is formed in a lead–acid storage battery when 1.00 g of Pb undergoes oxidation?
Verified step by step guidance1
Identify the chemical reaction involved in the oxidation of lead (Pb) in a lead-acid battery. The reaction is: Pb + HSO4- → PbSO4 + H+ + 2e-.
Calculate the molar mass of lead (Pb) using the periodic table. This will be used to convert the mass of Pb to moles.
Using stoichiometry, determine the moles of lead sulfate (PbSO4) produced per mole of lead (Pb) oxidized. From the balanced chemical equation, the mole ratio of Pb to PbSO4 is 1:1.
Calculate the molar mass of lead sulfate (PbSO4) using the periodic table. This will be used to convert moles of PbSO4 to mass.
Multiply the moles of PbSO4 by its molar mass to find the mass of lead sulfate formed.
Verified Solution
Video duration:
2m
This video solution was recommended by our tutors as helpful for the problem above.Was this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Oxidation-Reduction Reactions
Oxidation-reduction (redox) reactions involve the transfer of electrons between substances. In this context, lead (Pb) is oxidized, meaning it loses electrons, which is essential for understanding how lead sulfate (PbSO4) is formed in the battery. Recognizing the oxidation states of the elements involved helps in determining the products of the reaction.
Recommended video:
Guided course
01:53
Oxidation and Reduction Reactions
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. To find the mass of lead sulfate produced, one must use the molar ratios from the balanced equation of the reaction between lead and sulfuric acid, which is crucial for converting grams of Pb to grams of PbSO4.
Recommended video:
Guided course
01:16Stoichiometry Concept
Molar Mass
Molar mass is the mass of one mole of a substance, expressed in grams per mole. It is necessary to calculate the mass of lead sulfate formed from the mass of lead oxidized. Knowing the molar masses of lead (Pb) and lead sulfate (PbSO4) allows for accurate conversions between the mass of reactants and products in the reaction.
Recommended video:
Guided course
02:11Molar Mass Concept
Related Practice
Textbook Question
A Cu/Cu2+ concentration cell has a voltage of 0.22 V at 25 °C. The concentration of Cu2+ in one of the half-cells is 1.5×10–3 M. What is the concentration of Cu2+ in the other half-cell? (Assume the concentration in the unknown cell is the lower of the two concentrations.)
3843
views
Textbook Question
Determine the optimum mass ratio of Zn to MnO2 in an alkaline battery.
400
views
Open Question
Refer to the tabulated values of ∆Gf° in Appendix IIB to calculate E°cell for a fuel cell that employs the reaction between methane gas (CH4) and oxygen to form carbon dioxide and gaseous water.
Textbook Question
Refer to the tabulated values of ∆G°f in Appendix IIB to calculate E°cell for the fuel-cell breathalyzer, which employs the following reaction. ((∆G° for HC2H3O2(g) = -374.2 kJ/mol.)
CH3CH2OH(g) + O2(g) → HC2H3O2(g) + H2O(g)
544
views
Textbook Question
Determine whether or not each metal, if coated onto iron, would prevent the corrosion of iron. a. Zn
299
views