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determine the ∆H°f for one mole of HBr(g)
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- 4. Write a complete stepwise mechanism for any TWO of the following. You need to use curved arrows to show electron flow.Write a net ionic equation for the neutralization reaction of HCN(aq) with NaOH(aq). A) HCN(aq) + OH¨(aq) CN (aq) + H20(A B) H*(aq) + OH´(aq) H20() C) HCN(aq) + Na*(aq) + OH"(aq) Na*(aq) + CN"(aq) + H20() O D) HCN(aq) + NaOH(aq) → NACN(aq) + H20(0LUsing Table 1, calculate AH for each of the following reactions. Tell if each is exothermic or endothermic. & 2 CO(g) + 0:(g) → 2 CO:(g) h. N;(g) + 0:(R) → 2 NO(g) II. Calculate AH, for each of the following (using Table 1). i CCHae from the reaction 2 C;H:(g) + 50:(g) - 4 CO:(g) + 2 H;0(g) + 600kcal
- At 768 oC, Keq = 0.0725 for the reaction: NO(g) + 1/2 Cl2(g) NOCl(g) (a) What is the value of Keq for the reaction NOCl(g) NO(g) + 1/2 Cl2(g)?Keq = .(b) What is the value of Keq for the reaction 2 NO(g) + Cl2(g) 2 NOCl(g)?Keq = .(c) What is the value of Keq for the reaction 2 NOCl(g) 2 NO(g) + Cl2(g)?Keq = .L. Using Table 1, calculate AH; for each of the following reactions. Tell if each is exothermic or endothermic. a. 2 NO(g) + 0:(8) → 2 NO:(g) b. 2 C,Hlg) + 70:(g) → 4 CO.(g) + 6 H;0(g) c. N:(g) + 3 H:(g) - 2 NH:(g) d. 2 CH;OH(1) + 3 0:(g) → 2 CO:(g) + 4 H;0(g) e. 2 SO:(g) + 0:(8) + 2 S0,(g) f. 2 CH«(g) + 30:(8) → 2 CO:(g) + 2 H;0(g) & 2 CO(g) + O:(8) → 2 CO:(g) h. N;(8) + O:[g) → 2 NO(8) II. Calculate AH, for each of the following (using Table 1). i CHxo from the reaction 2 C;H:(B) + 5 0:(g) → 4 CO:(g) + 2 H;0(g) + 600kcal i CHo from the reaction CH«(g) • 2 0:(g) CO:(g) + 2 H;0(g) + 192 kcal III. Given the following reactions k S+ 0: - So: 71.0 kcal 2 so, + 0: - 2 s0, + 47.0 kcal Calculate AH, for 2 S + 3 0: - 2 SO, L 2C + 0, - 2 co + 52.8 kcal 2 co + 0; - 2 CO; + 125 kcal Calculate AlH, for C + 0z - co: IV. Calculate AH, AS and AG at 25 C, and tell if the reaction will go spontaneously (use Table 1 and 2) m. N:(g) + 3 H:(R) → 2 NH:(8) n. 2 CO(g) + 0:(g) - 2 CO:(8) a 2 CH:(g) + 5 0:(8)…At 714 oC, Keq = 1.78 for the reaction: SO2(g) + 1/2 O2(g) SO3(g) (a) What is the value of Keq for the reaction SO3(g) SO2(g) + 1/2 O2(g)?Keq = .(b) What is the value of Keq for the reaction 2 SO2(g) + O2(g) 2 SO3(g)?Keq = .(c) What is the value of Keq for the reaction 2 SO3(g) 2 SO2(g) + O2(g)?Keq = .
- This question has multiple parts A chemical reaction is written as: H2(g)+Br2(g)->2 HBr(s); Delta*H = - 72.6kJ Based on this information ... (a) Is the reaction endothermic or exothermic? How do you know? (b) If we add Br 2 (g) to the reaction at equilibrium will the reaction shift to the right to the left, or not change? How do you know? () Write its equilibrium constant expression (Keg )(aq) (aq) BeSO, (aq) + H,O(1) ↑ 4.reaction Mg(s) + Cl₂(g) → MgCl₂ (s) CH₂(g) + 20₂ (g) K Br(aq) + AgNO₂ (aq) KNO₂ (aq) + Ag Br(s) HBr(aq) + NaOH(aq) → NaBr(aq) + H,O (1) CO₂(g) + 2H₂O(g) → K 10 0 0 0 0 ОС 00000000 type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition X precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base Ś ? 0 000 000
- 1 (a) Does doubling the volumes of acid and base double the amount of heat? 1 (b) Does doubling the concentrations of acid and base double the amount of heat? 2 (a) What happens when different amounts of acid and base are used? What happens when sulfuric acid is substitutted for hydrochloric acid?What is the value of q in kJ?3. _Ba(OH)2(e) + heat