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At which temperature would a reaction with h-92 kjmol s-0.199 kj(molk) be spontaneous?
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What statement describes a reaction at 298 K if H 31 kJmol S 0.093 kJ(molK)?
It is not spontaneous.
What temperature would a reaction with H -220 kJmol and S -0.05 kJ(molK) be spontaneous?
3600 K
What can be said about a reaction with H 620 kJmol and S -0.46 kJ(molK)?
it can never be spontanious
How many kJ of energy are required to melt 30.7 g of ice The heat of fusion of water is 6.02 kJmol. The temperature remains constant at 0 and degC. kJ?
10,267 kJ are needed
What is the standard enthalpy of hydrogenation of 1-butene?
-127 KJmol-1
Which direction of the reaction equilibrium is favored at 298 K room temperature use the reaction I2 solid to I2 gas when H 62.4 kJmol and S 0.145 kJmolK?
I2(s) --> I2(g); dH=62.4kJ/mol; dS=0.145kJ/mol. The reaction will favor the product at this temperature. Your entropy is positive and your enthalpy is also positive, so this reaction will not be spontaneous at all temperatures. But at room temperature, which is 298K, it will be spontaneous and proceed left to right. (this is the sublimation of iodine)
At which temperature would a reaction with H -92 kJmol S -0.199 kJ(molK) be spontaneous?
400 K
What statement describes a reaction at 298 K if H 31 kJmol S 0.093 kJ(molK)?
It is not spontaneous.
What can be said about a reaction with triangle H 620 kJmol and triangle S -046 kJ(mol.K)?
it is never spontaneous
What can be said about a reaction with H 620 kJmol and S -0.46 kJ molK?
it can never be spontanious
What temperature would a reaction with H -220 kJmol and S -0.05 kJ(molK) be spontaneous?
3600 K
What is the value for G at 300 K if H 27 kJmol and S 0.09 kJmolK?
G = 0 kJ/mol
Ask us anythingUse the reaction I2(s) I2(g) H 62.4 kJmol S 0.145 kJ(molK) for question 10. What can be said about the reaction at 500 K?
It is spontaneous
What is the value for g at 300 k if h 27 kjmol and s09 kjmolk?
G= 0 kJ/mol
What can be said about a reaction with H -890 kJmol and S -0.24 kJ(mol K)?
It can be said to be exothermic since H is negative. Also below a temp of 3708ºC, the reaction will be spontaneous because ∆G will be negative. This is from ∆G = ∆H - T∆S.
What can be said about a reaction with H 620 kJmol and S -0.46 kJ(molK)?
it can never be spontanious
Which reaction shows that the enthalpy of formation of H2S is Hf -20.6 kJmol?
H2(g) + S(s) —> H2S + 20.6 kJ
