This question has multiple parts. Work all the parts to get the mnost points. a Calculate AH for the reaction 2K(s) + 2H,O(1) → 2KOH(ag) + H, (g) Substance and State AH (kJ/mol) K(3) KOH(aq) H2(9) H,O(1) -481 -286 AH kJ
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- Calculate Ksp for the salt NaCl at 25°C. Substance ΔGf°(in kJ/mol) Na+(aq) –262.0 Cl–(aq) –131.0 NaCl(s) -383.6Given the following data: 4C(s) + 4H2(g) + O2(g) → CH3CH2OCOCH3(l) ΔH°=-480.0 kJ CH3CH2OH(l) + O2(g) → CH3COOH(l) + H2O(l) ΔH°=-492.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the reaction:CH3COOH(l) + CH3CH2OH(l) → CH3CH2OCOCH3(l) + H2O(l)1. Use the following reactions to determine the Delta Hrxn for P4O10(s) + 6H2O(l) 4H3PO4(l) 4P(s) + 5O2(g)---> P4O10(s). Delta H = -2984kJ 2H2(g) + O2(g)---> 2H2O(l) Delta H = -570kJ 2P(s) + 4O2(g) + 3H2(g)---> 2H3PO4(l). Delta H = -2534kJ B. Is the reaction exothermic or endothermic? C. Given Sof P4O10(s) = 228.9 J mol-1 K-1; Sof H2O(l) = 69.9 J mol-1 K-1; Sof H3PO4(l) = 241.98 J mol-1 K-1 calculate the DGrxn at 28.0oC. D. Is this reaction spontaneous or nonspontaneous?
- Hydrogen gas reacts with oxygen gas to release 286.0 kJ per one mole of liquid water product. Liquid water reacts with more oxygen gas to form one mole of liquid hydrogen peroxide absorbing 98.1 kJ. Calculate ΔHrxn for hydrogen gas reacting with oxygen gas to form one mole of liquid hydrogen peroxide.my approach was using q = I∆φ∆t and i got 1980J, converted it to kj -> q=1.98kj. using ∆U = qV , ∆U =1.98kj. is my attempt correct???For the reaction C(s,graphite) + O2-> CO2 Delta G° = -394.3kj and delta S°= 2.9J/K and 1 atm The standard enthalpy change for tje reaction of 2.35moles of C(s,graphite) at this temperature would be....kJ This reaction is reactant/product-favored under standard conditions at 266 K. Assume that Delta H and delta S are independent of temperature. Fill in the blank and choose what type of reaction this is.
- A pellet of benzoic acid standard was combusted in a bomb calorimeter to determine the experimental calorimeter constant. After 6 mins of monitoring the temperature, the bomb was fired. The following data were obtained. mole of benzoic acid: 0.0049 mol mass of burnt fuse wire: 0.0117 g qwire,surr: 5858 J/g ΔHcombustion of benzoic acid: -3228.0 kJ/mol Δng (combustion of benzoic acid): -0.5 mol R: 8.314 J/mol•K r1: 0ºC/min r2: 0ºC/min Tf: 30.5ºC Ti: 28.4ºC Determine the calorimeter constant (in J/ºC). Report your answer in 2 decimal places.Consider the problem below: (Equation 1) 4 CO(g) + 4 H2O(l) ---> C4H8(l) + 4 O2(g) ΔH = 890.6 kJ/mol (Equation 2) CO2(g) ---> CO(g) + 1/2 O2(g) ΔH = 90.6 kJ/mol (Equation 3) C4H8(l) + 6 O2(g) ---> 4 CO2(g) + 4 H2O(l) ΔH = ??????? The ΔH for equation 3 is:______(express in kJ) Screen Reader Version Consider the problem below: (Equation 1) 4 CO(g) + 4 H2O(l) arrow C4H8(l) + 4 O2(g) ΔH = 890.6 kJ/mol (Equation 2) CO2(g) arrow C O(g) + 1/2 O2(g) ΔH = 90.6 kJ/mol (Equation 3) C4H8(l) + 6 O2(g) arrow 4 CO2(g) + 4 H2O(l) ΔH = ??????? The ΔH for equation 3 is:______(express in kJ)How logn would it take to convert 100 g Na(s) at 20oC to sodium vapor at 1000oC if heating rate at a pressure of 1 atm is 8 kj/min? Tmelt = 97.8oC Tboil - 883oC CNa(s) = 28.2 J/mol K CNa (l) = 30.8 J/mol K C Na(g) = 20.2 J/mol K Solve by adding all the qs and showing work please, need step by step, and solve on paper!
- Calculate the heat reaction in Mg given: Mass of Mg: 1.07786g Volume HCl: 50mL of 3M HCl Heat capacity of the solution: 4.184J/gx°C Trial 1 initial temperature: 26°C Trial 1 final temperature: 47°C Trial 2 Initial Temperature: 27°C Trial 2 final temperature: 47°C Note: please give detailed solutions. Thank you!1. CaCO3(s) <--> CaO(s) + CO2(g) ΔH° = +178 kJ exo or endo - thermic remove mass(CaO) --> shift: __ (increase) P(CO2) shift? __ ... two ways to lose mass(CaCO3)? __________ higher T shift? __ 2. SO2(g) <--> (1/8)S8(s) + O2(g) ΔH° = +297 kJ exo or endo - thermic Δν(gas)= _, (increase)Vtot --> P(gas)_ > on _hs shift? __ (decrease)P(SO2) shift? __ ... two ways to make mass(S8)? ___________ lower T shift? __ 3. C(s) + 2H2(g) <--> CH4(g) ΔH° = –75 kJ exo or endo - thermic Δν(gas) = _, (decrease)Vtot -->P(gas)_ > on _hs shift? __ (increase)P(CH4) shift? __ ...two ways to to lose mass(C)? ___________ higher T shift? __Calculate the enthalpy change for the reaction C(s) + 2H2 (g)--->CH4(g) from the following data. C(s) + O2 (g) ---> CO2(g). ΔH = – 393.5 kJ/mol H2(g) + 0.5 O2 (g) ---> H2O(l). ΔH = – 285.8 kJ/mol CH4(g) + 2 O2 (g)---> CO2(g) + 2 H2O(l). ΔH = – 890.2 kJ/mol