b) NaOH, H₂O 2 H₁C H 100°C

(f) The student finds the following particulate model of AgCl(s). Assuming the crystal structures are similar, how should the student modify the model to represent AgBr(s)? Justify your answer in terms of the radius and arrangement of electrons in the ions. CI- Ag+ CIF Ag* 口 Ag+ CI- Ag* CIT CI- Ag+ CI- Ag+ Ag+ CI- Ag+ CIT

For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of Cg H₁ (g) consumed, under standard conditions. C8H18 (g) + -25 0₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) AH; = ΔΗ What is the standard enthalpy of formation of this isomer of Cg H₁8 (g)? 18 -208.5 Incorrect ▲Hixn = -5108.7 kJ/mol kJ/mol

H B H cat HCI H₂O

[References] Given the following data СэНа (9) + 302(9) — 2 СО2(9) + 2Н,0() 2C2 H6 (g) + 702(9) → 4 CO2(g) + 6H2O(1) 2H2 (g) + O2 (g) → 2H2 O(1) ΔΗ -1411.0 kJ AH = -3119.8 kJ AH=-571.7 kJ calculate A H for the reaction C2H4 (9) + H2 (g) → C2H6 (9) ΔΗΞ kJ Submit Answer Try Another Version 3 item attempts remaining

You are given the following data: 2H(g) > H₂(g) - 2Br(g) - Br₂ (g) 2HBr(g) → H₂(g) + Br₂ (g) kJ mol → x10 ΔΗ° = -436.4 Calculate AH° for the reaction. H(g) + Br(g) HBr (g) Be sure your answer has the correct number of significant digits. X ΔΗ° = -192.5 ΔΗ° = 72.4 kJ mol kJ mol kJ mol

500.0 mL of 0.100 mol·L HCl(aq) was added to a high quality insulated calorimeter containing 500.0 mL of 0.100 mol·LNaOH(aq). Both solutions had a density of 1.000 g·mL and a specific heat of 4.184 J·g ·K . The calorimeter had a heatcapacity of 850.0 J·K . The temperature of the entire system rose from 25.50 C to 26.05 C.Calculate the heat of reaction.   Thank you!

2 CO (g) O2 (g) → 2 CO, (g) Exothermic or endothermic

Q2 (a) Given that the enthalpy values for the following reactions are: AH = -1049.0 kJ 2 Al (5) + 6HCI (ад) — 2 ALCI3 (аg) + 3 Н2 (9) AH = -74.8 kJ HCl (g) → HCl (aq) + Cl2 (g) → 2HCI AH = -185.0 kJ H2 (9) + AlCl3 (s) → AlCl3 (aq) (g) AH = -323.0 kJ ΔΗ Manipulate the reactions above to determine AH for: 2 Al(s) + 3 Cl2 (9) → 2 AlCl3 (s) In one experiment, a 25 g sample of an alloy was heated to a certain temperature. (b) The heated alloy was then dropped into a beaker containing 90 g of water at 25.32 °C. The temperature of the water rose to a final value of 27.18 °C. Predict the final temperature that the alloy is being heated at the beginning of the experiment. Given that the heat capacity of water and alloy are 4.184 Jgl°C-' and 0.3847 Jg l°C' respectively.

Calculate the standard enthalpy for the reaction: 4NH3(g) + 502(g) - 4NO(g) + 6H2O(g), given the following data: N2(g) + O2(g) - 2NO(g) AH,xn = -43.1 kcal mol %3D N2(g) + 3H2(g) - 2NH3(g) AHxn = -21.9 kcal mol 2H2(g) + O2(g) - 2H,0(g) AHxn = -115.6 kcal mol1 Round your answer to 2 decimal places.