Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Battery manufacturers often assess batteries in terms of their specific energy (or energy
capacity). The weight capacity of a battery is defined as q 3 V/mass. Why would a battery
manufacturer be interested in this quantity?
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- 3. What mass of lead is needed to create 2.50g of PbSO4 in a lead acid battery? The overall balanced reaction that occur in the lead - acid storage battery is Pb(s)+PbO, (s)+2 HSO, (aq)+2H* (aq) → 2 PbSO, (s) +2H,0(I)arrow_forward6. As we will discuss when we get to the chapter on electrochemistry, the AGO for a reaction can very easily be determined by incorporating the reaction into an electrochemical cell (battery). AGO is directly proportional to the potential (voltage) of the cell. Using this technique, it was found that the AG° = -1370.8 kJ for the following reaction. 2 CH₂OH(1) + 3 0₂(g) → 2 CO₂(g) + 4H₂O(1) 0. The standard entropy change (AST) for this reaction is ?163.6 J/K at 25.0 °C. A. B. C. What is the standard enthalpy of reaction, AHxn at 25.0 °C?. Please provider your answer below. ☐☐ → 0 0 0 If AHrxn and ASrxn do NOT change with temperature, what is the AGxn at 171.58 °C? Please provider your answer below. 0² 0₂ 010 H 0² 0₂ Above Please provider your answer below. °C, the reaction will become non-spontaneous? kJ kJarrow_forwardBalance this equation: _UO2(s) + _ HF(£) → _ UF4(s) +_ H20(E) -> Though you would not normally do so, enter the coefficient of "1" if needed.arrow_forward
- Given the reaction: Fe+2 + Cr2O7 -2 → Fe+3 + Cr+3 How many mole/s of Fe+2 is/are used involved in a balanced reaction ? 7 5 3 4 6arrow_forwardComplete and balance the following redox equations using the smallest whole-number coefficients. The reaction takes place in a BASIC solution. Fe(OH)2 (s) + MnO4−(aq) → MnO2 (s) + Fe(OH)2 (s) In the balanced equation, 3 OH- are present on the product side. In the balanced equation, 5 molecules of water are present on the reagent side. In the balanced equation, 4 molecules of water are present on the product side. In the balanced equation, 5 molecules of water are present on the product side. In the balanced equation, 3 OH- are present on the reagent side. In the balanced equation, 4 molecules of water are present on the reagent side.arrow_forwardConsider the following equation in aqueous solution: PO₃³⁻(aq) + SO₂(g) → PO₄³⁻(aq) + S²⁻(aq) The oxidation half-reaction is PO₃³⁻(aq) + H₂O(l) → PO₄³⁻(aq) + 2 H⁺(aq) + 2 e⁻ and the reduction half-reaction is SO₂ (g) + 4 H⁺(aq) + 6 e⁻ → S²⁻ (aq) + 2 H₂O(l). How many moles of electrons must be transferred in the overall reaction?arrow_forward
- Balance the reaction between NO and Cd2+ to form NO3 and Cd in acidic solution. When you have balanced the equation using the smallest integers possible, enter the coefficients of the species shown. NO + Cd2+ NO3 Cd (reactant, (Enter 0 for neither.) Water appears in the balanced equation as a product, neither) with a coefficient of How many electrons are transferred in this reaction?arrow_forwardBalance the following redox reaction in the gas phase. Note that this reaction cannot be balanced with the half-reaction method and must be done by inspection. In the gas phase, H2 O (1) is used to balance oxygen atoms and H3 O+ and OH are not available for balancing purposes. ONLY integers should be used in your answer. NH3 (aq) + O2 (g) –→ NO2 (g) Enter your chemical notation herearrow_forwardBe sure to answer all parts. Over a period of time, the concentration of sulfuric acid in the lead storage battery of an automobile has decreased from 38.0 percent by mass (density = 1.29 g/mL) to 26.0 percent by mass (1.19 g/mL). Assume the volume of the acid remains constant at 709 mL. (a) Calculate the total charge in coulombs supplied by the battery. x 10 с Enter your answer in scientific notation. (b) How long (in hours) will it take to recharge the battery back to the original sulfuric acid using a current of 23.4 A? harrow_forward
- A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+8H(aq) +5e Cl₂(g) +2e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Answer the following questions about this cell. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. + Do you have enough information to calculate the cell voltage under standard conditions? half-reaction 0 0 Yes Mn²+ (aq) + 4H₂O(1) →Mn²+, 2 C1 (aq) No standard reduction potential Eº 'red = +1.51 V E=+1.359 V red ロ→ロ X 0x19 Sarrow_forwardIs the reaction a redox reaction; "yes" or "no".arrow_forwardWrite a balanced net ionic equation for a redox reaction that results in the formation of potassium chloride. (Assume that potassium chloride is not a starting material, and assume the reaction takes place in aqueous solution.) X, Не (aq), 2K(ag)+Cl, (aq) KCI(aq)arrow_forward
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