What can be said about a reaction with H = 62.4 kJ/mol and S = 0.145 kJ/(mol·K)?
2 answers:
The answer is "It is spontaneous at 500 k"
Answer: At 430.34 K the reaction will be at equilibrium, at T > 430.34 the
reaction will be spontaneous, and at T < 430.4K the reaction will not
occur spontaneously. Explanation: 1) Variables: G = Gibbs energy H = enthalpy S = entropy 2) Formula (definition) G = H + TS => ΔG = ΔH - TΔS 3) conditionsΔG < 0 => spontaneous reaction ΔG = 0 => equilibrium ΔG > 0 non espontaneous reaction 4) Assuming the data given correspond to ΔH and ΔSΔG = ΔH - T ΔS = 62.4 kJ/mol + T 0.145 kJ / mol * K => T = [ΔH - ΔG] / ΔS ΔG = 0 => T = [ 62.4 kJ/mol - 0 ] / 0.145 kJ/mol*K = 430.34K This is, at 430.34 K the reaction will be at equilibrium, at T > 430.34 the reaction will be spontaneous, and at T < 430.4K the reaction will not occur spontaneously.
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Answer:
g CO2(g) = 264.06 g
Explanation:
∴ moles O2(g) = 6 mol
∴ mm CO2 = 44.01 g/mol
⇒ mol CO2(g) = ( 6 mol O2(g) )×( mol CO2(g) / mol O2(g) ) = 6 mol CO2(g)
⇒ mass CO2(g) = ( 6 mol CO2(g) )×( 44.01 g/mol ) = 264.06 g CO2(g)
3.25 kg in g = 3.25 * 1000 = 3250 g Molar mass C₂H₆O₂ = 62.0 g/mol Mass solvent = 7.75 kg Number of moles: n = mass solute / molar mass n = 3250 / 62.0 n = 52.419 moles Molality = moles of solute / kilograms of solvent M = 52.419 / 7.75M = 6.7637 mol/kg hope this helps!
Answer:
accretion at convergent boundaries
Explanation:
Answer:
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