A 1.3kg metallic mass increase 2°c for every 1000J of heat applied to it. The simple shows some impurities that can alter the temperature reading a bit. Identify the metal.

A model for the compound 2,2- dimethylbutane is shown. Write a balanced chemical equation that shows the formation of 2,2-dimethylbutane from the elements carbon (C) and hydrogen). (Use the smallest integer coefficients possible and do not include states.) A model for the compound 2,2-dimethylbutane is shown Write a balanced chemical equation that shows the formation of 2,2-dimethylbutane from the elements carbon (C) and hydrogen (H₂) (Use the smallest integer coefficients possible ond do not include states.)

Consider the following data. 2 H₂0 (1) 2 H₂(g) + O₂(g) 2 HNO3(1) = N₂05(9) + H₂O(1) 2 HNO30 (1) ⇒ N₂(g) + 3 O₂(g) + H₂(g) Use Hess's law to calculate AH for the reaction below. ΔΗ= |1083.8 AH = +571.7 kJ AH = +92.0 kJ AH = +348.2 kJ x kJ 2 N₂05(9) 2 N₂(g) + 5 O₂(g)

a.) Image 1 b.) Image 2

You may want to reference (Pages 323 - 325) Section 9.6 while completing this problem. Part A How much energy in kilojoules is required to convert 511 mL of water at its boiling point from liquid to vapor? Recall that AHvan (H20) = +40.7 kJ/mol. Express the energy to three significant figures with the appropriate units. 圖]? heat = Value Units Submit Request Answer Part B Complete previous part(s) < Return to Assignment Provide Feedback MacBook Pro esc @ 23 % & 2 3 4 5 6 8 9 Q W E Y P R

The thermogram in the figure below shows the change in mass for a sample of calcium oxalate monohydrate, CaC2O4 × H2O. The original sample weighed 42.50 mg and was heated from room temperature to1500 °C at a rate of 5 °C min. The following changes in mass and corresponding temperature ranges were observed: • Loss of 4.03 mg from 100–250 °C• Loss of 5.72 mg from 400–500 °C• Loss of 8.41 mg from 700–850 °CDetermine the identities of the volatilization products and the solid residue at each step of the thermal decomposition.

4. (i) Identify the different enthalpy changes and construct the Born-Haber cycle for the formation of sodium choride (NaCl) using the information below. Calculate the missing enthalpy change value Na*(g) + Cl(g) → NaCI (s) AH° = ? Cl2 (g) → CI (g) AH° = +121 kJmol1 CI (g) + e¨ → Cl(g) AH° = -364 kJmol1 Na (s) → Na (g) AH° = +108 kJmol1 Na (g) → Na*(g) + e` AH° = +500 kJmol1 Na (s) + Cl2 (g) → NaCI (s) AH°= -411 kJmol1

Given the following processes and their enthalpy values::            Reaction/Process                   Delta_H (enthalpy)             Li(s)  -->  Li(g)                             159 kJ             Li(g)  -->  Li+(g)  +  e–                 520. kJ             Cl2(g)  -->  2Cl–(g)                      242 kJ             Cl(g)  +  e–  -->  Cl(g)                  -349 kJ             LiCl(s)  -->  Li+(g) +  Cl–(g)           853 kJ          ----------------------------------------------------------------------------------          Calculate the enthalpy of formation of LiCl(s) (in kJ/mol) according to the following equation:             Li(s)  +  ½ Cl2(g)  -->  LiCl(s)  (C 4)          (A)  1425          (B)  1204          (C) -402          (D) -281

Consider the balanced reaction 7 A + 6 B → 3 C + 6 D. Consider the balanced reaction 9 A + 6 B → 3 C + 8 D. If 4.384 moles of D (MW = 34.59) are produced, how many grams of A (MW = 23.38) are consumed?

Given these reactions, where X represents a generic metal or metalloid 1) H, (g) + 0,(g) → H,0(g) AH1 = -241.8 kJ 2) X(s) + 2 Cl,(g) → XCl,(s) AH2 = +475.9 kJ 3) H,(g) + CL,(g) HCl(g) АНз 3 —92.3 kJ → 4) X(s) + O,(g) –→ XO,(s) AH4 = -748.7 kJ 5) Н, О(2) — н,00) AH5 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI, (8) + 2H,О() — ХО,(8) + 4 HCI(g)