The quantity of oxygen that can dissolve in water depends on the temperature of the water. (So thermal pollution influences the oxygen content of w water temperature T. S (mg/L) 20 16 12 8 4 0 8 16 24 32 40 T (°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)

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

just 2 and 3 and maybe 4

DATA : Mass of Magnesium (g) 0.0525 g Volume of hydrogen gas (mL) 50.0 mL Temperature of hydrogen gas (°C) 25.0°C Atmospheric Pressure (mmHg) 762 mm Hg Vapor pressure of water (mmHg) Partial pressure of hydrogen (mmHg) DATA ANALYSIS

9-2. Consider this thermochem ical equation: 4 PCh(1) → Pa(s) + 6 Ch(g) AH° = +1278.8 kJ If the chlorine gas is collected at STP, then what volume of chlorine is produced when 68 joules are absorbed in the reaction?