The quantity of oxygen that can dissolve in water depends on the temperature of the water. (So thermal pollution influences the oxygen content of wwater temperature T.S (mg/L)201612840816 243240T (°C)0(a) What is the meaning of the derivative S'(7)? What are its units?S'(T) is the rate at which temperature changes with respect to time. The units are °C/s.S(T) is the rate at which oxygen solubility changes with respect to the water temperature. The units are (mg/L)/°C.O S'(T) is the rate at which temperature changes with respect to the oxygen solubility. The units are °C/(mg/L).OS'(T) is the current level of oxygen solubility for a given temperature. The units are mg/L.OS'(T) is the rate at which oxygen solubility changes with respect to the time. The units are (mg/L)/s.(b) Estimate the value of S'(32) and interpret it. (Round your answer to three decimal places.)S(32)

Answered: The quantity of oxygen that can…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of C, H₁g (g) consumed, under standard conditions. 25 Cg H18 (8) + O₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) What is the standard enthalpy of formation of this isomer of Cg H₁g (g)? AH; = $ V T B MacBook Air Y H & 7 8 AH-5108.7 kJ/mol 18 N M K 1 38 kJ/mol
We want to convert 18 g of solid water at -22 °C to vapor at 116 °C. The energy need for this process is supplied by combustion of CH/C,H, gas mixture which is composed of 60% CH,(g) by mass. What is the volume of required amount of the mixture at 25 °C and under 745 mmHg pressure? For water c(solid) = 2.11 JgK", c(liquid) = 4.18 Jg" K", c(gas) = 2.00 J g K". AH"(fusion) = 6.00 kJ mol", AH (vapor.) = 40.7 kJ mol". %3D %3D %3D For CH, AH"(combustion) = -891 kJ mol %3D For C,He AH"(combustion) -1560 kJ mol O a. 1.38 L O b. 1.58 L Oc. 1.43 L O d. 1.47 L O e. 1.30 L
Suppose that 13.93 grams of X (MW = 52.41) undergo combustion. The heat from this reaction is then transferred to 266 mL of water, and the water temperature changes from 26.37°C to 79.01°C. Assume the specific heat of water is 4.2 J/(g.°C) and the density of water is 1.0 g/mL. %3D Calculate the enthalpy of combustion of X in kJ/mol. Report your answer to three decimal places.
Ery 1 3 M (M) 2req The production capacity for acrylonitrile (C3H3N) in the United States is over 2 billion pounds per year. Acrylonitrile, the building block for polyacrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: 2C3H6(g) + 2NH3(g) + 30₂(g) → 2C3H3N(g) + 6H₂O(g) Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: Mass 7.28x102 g 5.00 x 102 g 1.00 x 103 g In progress Reactant oxygen propylene ammonia oxygen What mass of water is formed from your mixture? mass of water formed = g Calculate the mass (in grams) of each reactant after the reaction is complete: Submit g = mass of acrylonitrile produced Reactant Mass remaining propylene ammonia Show Hints ס ס ס g g Cengage Learning Cengage Technical Support Previous Next Save and Exit
A propane tank with 8.17 liters is purchased while the temperature was at 14.4 ∘∘C, you decided to use it the following day to bbq due to the nice sunny hot day. The tank was placed in direct sunlight causing an increase in the temperature of the gas to 37.8 ∘∘C. Calculate the new volume of the gas due to the change in temperature. The gas tank's release valve maintains the pressure constant.
Consider these reactions, where M represents a generic metal. 2 M(s) + 6HCl(aq) 2 MC13(aq) + 3H₂(g) HCl(g) HCl(aq) H₂(g) + Cl₂ (g) - MC13 (s) →→→ MC1₂ (aq) Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl₂(g) → 2 MC1₂ (s) 1. 2. 3. 4. AH = 2 HCl(g) AH₁ = -553.0 kJ ΔΗ, = −74.8 kJ AH3 = -1845.0 kJ AH4 = -337.0 kJ kJ
2H,O1) = H3O+(aq) + OH (aq) Kw = 1.0x 1014 at 25 °C Kw=5.5x 1014 at 50 °C Based on this data, which statements are true? You may check any combination of statements. 2H20(1) = H3O*(aq) + OH(aq) is an exothermic reaction 0.10 M NAOH solution at 50°C has pH = 12.26 Pure water at 50°C contains more ions than pure water at 25 °C.
Some commercial drain cleaners use a mixture of sodium hydroxide and aluminum powder. When the solid mixture is poured into the drain and dissolves, a reaction ensues that produces hydrogen gas: 2N2OH(aq) + 2Al(s) + 6H2O() – 2NAAI(OH)4(aq) + 3H2(g) Determine the temperature (in °C) of hydrogen gas produced when 31.58 g of aluminum reacts with excess sodium hydroxide and water if the pressure is 103.10 kPa and the volume is 36.23 L. Provide your answer with TWO decimals. Your Answer: Answer units
CaCO3(s)⇄CaO(s)+CO2(g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0mol sample of CaCO3(s) is placed in a rigid 100.L reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00atm, while some CaCO3(s) remains in the vessel. (a) Calculate the number of moles of CO2(g) present in the vessel at equilibrium. (b) Write the expression for Kp, the equilibrium constant for the reaction, and determine its value at 898°C. (c) The experiment was repeated, but this time starting with a 4.0mol sample of CaCO3(s). On the following graph, draw a curve showing how the pressure of CO2(g) would change over time as the vessel is heated to 898°C and equilibrium is established.
An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g); ∆H = -1124 kJ. The density of sulfur dioxide at 25 °C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/mol °C. a) How much heat would be evolved in producing 1.00 L of SO2 at 25 °C and 1.00 atm? b) Suppose heat from this reaction is used to heat 1.00 L of SO2 from 25 °C to 500 °C for its use in the next step of the process. What percentage of the heat evolved is required for this?
Some commercial drain cleaners use a mixture of sodium hydroxide and aluminum powder. When the solid mixture is poured into the drain and dissolves, a reaction ensues that produces hydrogen gas: 2NAOH(aq) + 2AI(s) + 6H2O() → 2NAAI(OH)4(aq) + 3H2{g) Determine the temperature (in C) of hydrogen gas produced when 17.08 g of aluminum reacts with excess sodium hydroxide and water if the pressure is 107.37 kPa and the volume is 40.29 L. Provide your answer with TWO decimals.
Oxygen gas can be generated by heating potassium chlorate: heat 2KCIO, (s) 2KCI(s) + 30, (g) What volume of oxygen gas, collected by displacement of water and measured at 750.1 torr and 80.0 °C (vapor pressure of water 80.0 °C -355.63 torr), will be formed by the decomposition of 19.3 g of potassium chlorate? Be sure your answer has the correct number of significant figures. Note: Reference the Conversion factors for non-SI units and Fundamental constants tables for additional information. L D-P X S

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