The enthalpy change for the dissolution of sulphuric acid in water is -75.0kJ/mol. Concentrated sulphuric acid is an 18.1M solution. Calculate how much the temperature of the solution would change if you were making 1.38L of pH -0.56 H2SO4. Assume the solution has the same heat of solution as water, 4.186 kJ/Kg °C and the density of concentrated H2SO4 is 1.840 kg/L. Only your final answer is required to three sig figs.
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- A small amount of acetonitrile (CH,CN) is dissolved in a large amount of water. Imagine separating this process into the four stages sketched below. (These sketches show only a portion of the substances, so you can see the density and distribution of atoms and molecules in them.) D CH;CN H20 solution Use these sketches to answer the questions in the table below. The enthalpy of solution AH is negative when soln CH3CN dissolves in water. Use this information to list the stages in order of increasing enthalpy. O absorbed Would heat be absorbed or released if the system moved from Stage A to B? O released O neither absorbed nor released O none O ionic bonding force O covalent bonding force O metal bonding force O hydrogen-bonding force What force would oppose or favor the system moving from Stage A to B? Check all that apply. O dipole force O ion-dipole force O dispersion forceDetermine the enthalpy of neutralization in Joules/mmol for a solution resulting from 19 mL of 0.8 M NAOH solution and 19 mL of a HCl with the same molarity. If separately, each had a temperature of 29 degrees Celsius, and upEn addition, the highest temperature reached by the solution was graphically determined to be 38 degrees Celsius, Round to the nearest whole number.A typical coal-fired electric generating plant will burn about 3 metric tons of coal per hour. Most of the coal burned in the United States contains 1 to 4 % by weight sulfur in the form of pyrite, which is oxidized as the coal burns: 4FeS2(s) + 11 O₂(g) 2 Fe2O3(s) + 8 SO2(9) Once in the atmosphere, the SO2 is oxidized to SO3, which then reacts with water in the atmosphere to form sulfuric acid: SO3(9) + H₂O(1)→→→→→→→ H₂SO4(aq) If 42.4 metric tons of coal that contains 1.44 % by weight S is burned and all of the sulfuric acid that is formed rains down into a pond of dimensions 397 m x 256 m x 4.96 m, what is the pH of the pond? (OK to assume 2 mol H30+ per mole H₂SO4.) Hint: 1 metric ton = 1000 kg
- 1. Henry’s Law constant for most gases decreases with increased temperature. Given that KH for O2 is 2.20 x 10-3 M atm-1 at 5oC, calculate the percent O2(aq) saturation if a lake water sample at 5oC and sea-level is found to contain, 9.20 mg/L of O2(aq). (Recall: partial pressure of O2 at sea-level = 0.2095 atm).4 of 15 > Calculate the standard enthalpy of reaction, AHxn, of each of the given acid-base neutralization reactions involving the strong base KOH. The standard enthalpy of formation data are provided. $ = R Compound or Ion Standard Enthalpy of Formation (kJ/mol) -482.4 -285.8 -98.4 -349.5 -121.0 -372.1 -132.5 -80.3 -251.2 AHixn = F KOH(aq) H₂O(1) HCIO3(aq) KCIO₂ (aq) V HBr(aq) KBr(aq) NH(aq) HCIO3(aq) + KOH(aq) → KCIO3(aq) + H₂O(1) NH, (aq) K+ (aq) G Search or type URL % 5 T G B MacBook Pro 6 Y H & ve 7 N U J 00 8 M I ( 9 K O < H O L command A P Δ' 1 - ; 3 Question option [ + 11 + 21 = ? kJ/mol 11Water is added to a flask containing solid NH₄Cl. As the salt dissolves, the solution becomes colder.(a) Is the dissolving of NH₄Cl exothermic or endothermic?(b) Is the magnitude of ΔH(lattice) of NH₄Cl larger or smaller than the combined ΔH(hydr) of the ions? Explain.(c) Given the answer to (a), why does NH₄Cl dissolve in water?