Galena is the ore from which elemental lead is extracted. In the first step of the extraction process, galena (PbS) is heated in air to form lead(II) oxide.\[ 2 \text{PbS (s)} + 3 \text{O}_2\text{(g)} \rightarrow 2 \text{PbO (s)} + 2 \text{SO}_2\text{(g)} \quad \Delta H = -827.4 \, \text{kJ} \]What mass of galena (PbS) is converted to lead (II) oxide if 200 kJ of heat are produced?

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Answered: What mass of galena (PbS) is converted…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 40QRT

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One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na,(CO,),(HCO,) 2H,0, Na,(Co,),(HCO,) 2H,0(s) → 5Na,cO,(s) + CO,(g) 3H,0(g) + When 1.00 metric ton (1 × 10° kg) of trona is decomposed, 0.74 metric ton of Na,co, is recovered. What is the percent yield of this reaction? Select one: a. 93% 19 b. 22% С. 83% d. 43% е. 17%
Write the balanced molecular chemical equation for the reaction in aqueous solution for cesium carbonate and magnesium nitrate. If no reaction occurs, write NR. CS2CO3 + Mg(NO3)2 →2 CSNO3 + M9CO3 04 02+03+ 4+ 3 6. 7 8. 6. 0. 口3||□4 Os 19 10 (s) (1) (g) (aq) Mg Mn N NR Cs 69°F O pe here to search 4- 2.
The nitrogen content of organic compounds can be determined by the Dumas method.The compound in question is first passed over hot CuO(s): Compound ----> N2(g) + CO2(g) + H2O(g) The gaseous products are then passed through a concentrated aqueous KOH solution to remove the CO2.The remaining gas contains N2 and water vapor.A 0.185-g sample of a compound was treated as above, producing 82.2 mL of N2 saturated with water vapor at 25 °C and 775.0 torr.What is the mass percent of nitrogen in the compound? (The vapor pressure of water at 25 °C is 23.8 torr.)
Suppose the reaction system UO2 (s) + 4 HF (g) ↔ UF4 (g) + 2H2O (g) has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. Tell whether the equilibrium will shift to the right, shift to the left, or will not be affected. Additional UO2 (s) is added to the system. The reaction is performed in a glass reaction vessel; HF (g) attacks and reacts with glass. Water vapor (H2O (g)) is removed.
Write the balanced net ionic equation for the reaction that occurs in the following case: Fe(NO3)2(aq)+KOH(aq)→ Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.
To further investigate the reactivity of silver, the student submerges a piece of metallic scandium, Sc (s), in a solution of AgNO3 (aq) and observes that the following reaction occurs. Sc(s) + 3 AGNO3 (ag) →3 Ag(s) + Sc(NO3); (aq) (k) Write the balanced net-ionic equation for the reaction. B IU x² X, 3 Ĉ Ω 0/10000 Word Limit
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Sodium nitrate contains 0.3% iodine in the form of calcium iodate, Ca(IO3)2. After the sodium nitrate in the niter is dissolved and recrystallized, the remaining solution contains 9 g/Lsodium iodate, NaIO3(aq). The NaIO3 is converted to iodine when it reactswith sulfur dioxide and water.2NaIO3 + 5SO2 + 4H2O → Na2SO4 + 4H2SO4 + I2a. How many liters of sodium iodate solution that contains 9 g of NaIO3 perliter would be necessary to form 127.23 kg of iodine, I2?
Hydroxyapatite, Ca,(PO)(OH)₂, has a solubility constant of K-2.34 x 10-59, and dissociates according to Cao (PO)(OH)₂ (s) = 10 Ca² (aq) + 6PO (aq) + 2OH(aq) Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca²+ in this solution if JOH is fixed at 8.30 x 10M? |Ca²1 M
Copper(I) ions in aqueous solution react with NH3 (aq) according to Cu+ (aq) + 2 NH3 (aq) · → Cu(NH3)2(aq) K₁ = 6.3 × 1010 Calculate the solubility (in g·L-¹) of CuBr(s) (Ksp = : 6.3 × 109) in 0.74 M NH3(aq). solubility of CuBr(s): g/L
Co(H2O)62* (ag) +CF(ag) = CoCl42-(ag) + H2O (1) a) Balance this equation and write the expression for the equilibrium constant for this reaction. Write the expression for the equilibrium constant for this reaction. b) If the concentrations of all species are 2.50M at 25°C and the equilibrium constant of the reaction at 25°C is Keq = 2.85 102, how will the reaction shift? Show calculations and explanation. c) Explain the effect of adding silver nitrate to the solution. How does it shift the reaction? Provide the ionic equation.

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