Hvap 40.65 kJ/mol Hf -285.83

Ln(P2/p1)=ln(-delta Hvap/R)•(1/T1-1/t2)I have ammonia at normal boil with a temp at 39.2C find the Hvap
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2. asked by Anonymous
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How do u find the Hvap if you only know the slope is -.002 ?
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2. asked by James
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How do u find the Hvap if you only know the slope is -.002 ?
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2. asked by James
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How do you find [delta]Hvap?
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2. asked by James
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A liquid has a delta(Hvap) of 35.5 kJ/mol and a boiling point of 122 C at 1.00atm. What is its vapor pressure at 113 C?
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2. asked by Bruce
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ln 555.6/281.1 = -deltaH vap/8.314J/k mol [1/256.1K - 1/242K]. I have to solve for delta Hvap.I know that the left side would
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2. asked by Hannah
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Hvap 40.65 kJ/molHf -285.83 kJ/mol Hfusion 6.03 kJ/mol specific heat 4.186 J/gC molar mass 18.02 g How much energy is consumed
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2. asked by martin
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Hvap 40.65 kJ/molHf -285.83 kJ/mol Hfusion 6.03 kJ/mol specific heat 4.186 J/gC molar mass 18.02 g How much energy is consumed
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2. asked by martin
3. 482 views
How many kilojoules of heat are needed to completely vaporize 42.8 g of C4H10O at its boiling point? Given Hvap=26.5kj/mol
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2. asked by kim
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Calculate the molar entropy of vaporization forliquid hydrogen iodide at its boiling point, �34.55°C. HI(l)7HI(g) �Hvap � 19.76
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2. asked by philipa
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