Use Hess's law to calculate the standard heat of the water-gas shift reaction, CO(8) + H20(g) → CO2(8) + H2(g) using the two data sets given below. $1: CO(8) + H20(1) → CO2(g)+H2(8): AH, = 1226 But /lbmol H20(1) → H20(g) : AHvap = 18935 But /lbmol $2: CO(g) +1/202(g) →CO2(g): AH, =-121740 But /lbmol H2(g)+1/202(8) → H20(g) : AH, =- 104040 But /lbmol

2) Copper reacts with iodine in a similar reaction from what was done in lab to produce copper(I) iodide, CuI. The balanced equation for this reaction is 2Cu(s) + I2(s) ⟶2CuI(s) For this reaction, students obtain the following data: Mass I2: 0.5713 g Moles I2: 0.002251 mol Mass Cu: 0.3517 g Moles Cu: 0.005535 mol   Which is the limiting reactant? Group of answer choices Cu I2 No answer text provided. No answer text provided.

Solve correctly please need all parts.

8. Consider the following chemical reaction: 7 4 HBr(g) + O2(g) → 2 H20(g) + 2 Br2(g) Identify the substance oxidized (SO), the substance reduced (SR), the oxidizing agent (OA) and the reducing agent (RA). SO: SR: OA: RA:

The free energy change for the following reaction at 25 °C, when [Co²+] = 1.15 M and [Cd²+] = 6.07×10 3 M, is -36.7 kJ: Co²+(1.15 M) + Cd(s)— Co(s) + Cd²+(6.07×10-³ M) AG = -36.7 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction? forward ✓

P4(g) + 6 Cl2(g) →4 PCI3(g) If 0.680 moles of P4 is mixed with 2.99 moles of Cl2 in a 1.58-L rigid reaction vessel, what is the final pressure in the vessel after the reaction goes to completion? The final temperature is 454. °C. Assume 100% yield. 47.0 atm 82.1 atm 51.3 atm 103. atm O 75.2 atm

2. Consider the following reaction: CO) +=O=COz) s) Find AH (kJ/mol) of the reaction at 298 K and 1 bar (b) ›) Determine the spontaneity of the reaction in a furnace operating at 2000 K where the partial pressures of the compounds are: Compound iP (bar) CO(R) O₂(g) CO2(g) Consider that for this reaction AG2000k = -111 kJ/mol 0.05 2.00 2.50

From the standard enthalpy of formation of atomic hydrogen (h). from the standard enthalpies of formation, calculate the delta H rxn for the reaction. C6H12(l) + 9O2(g) = 6CO2(g) + 6H2O(l) For C6H12(l), delta H degrees farenheight= -151.9 kJ/mol

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|For the reaction at 25.0 °C: 2 SO3(g) 2 SO2 (g) + Q, (g) www. K, = 1.4 x 10-25 and G° = 141 kJ/mol At 25.0 °C, the partial pressure of So, = 10.0 atm, that of SO, is 0.00120 atm, and that of 0, is 0.00180 atm. Calculate G (in kJ) for this process. G= G° + RTINQ