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What is the value for G at 700 K if H -92 kj mol and S -0.199 kj mol-k?
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What is the accepted value for the heat of solution NH4Cl?
The accepted value for the heat of solution of NaOH is -44.2 kJ/mol
What is the standard thermodynamic value of liquid butane C4H10?
C4H10(g) is about -126 kJ/mol C4H10(l) is about -147 kJ/mol
Is actinium has a low ionization energy?
The value is not so low: 499 kJ/mol.
What is the value and units of the molar gas constant?
R = 0.082 ATM L/mol K
What is the value of specific heat of 2-propanol at 130c?
82 degrees Celsius
What is the value for G at 100 K if H 27 kJ mol and S 0.09 kJ molK?
G=18 kJ/mol
What is the value for G at 100 K if H equals 27 kJ mol and S equals 0.09 kJ molK?
G = 18 kJ/mol
What is the value for G at 100 K if H 27 kJmol and S 0.09 kJ(molK)?
18 kJ/Mol
What is the value for g at 5000 k if h -220 kj mol and s equals -0.05 kj molk?
-18 kj/mol
What form a spontaneous reaction at 298 K?
H = 28 kJ/mol, S = 0.109 kJ/(molK)
Which statement describes a reaction at 298 K if H 31 kJ mol S 0.093 kJ molK?
It is not spontaneous.
What can be said about a reaction with H equals -890 kJ mol and S equals -0.24 kJ molK?
It is spontaneous at 2000 K.
If a reaction has an enthalpy of -54.32 kJ/mol and an entropy of -354.2 J/(K*mol), what is the Gibbs free Energy at 54.3(degrees c)?
DeltaG = DeltaH - TDeltaS dG = -54.32 kJ/mol - (54'32+273)K(-354.2J/molK) NB Thevtemperature is quoted in Kelvin(K) and the Entropy must be converted to kJ by dividing by '1000'/ Hence dG = - 54.32kJ/mol - (327.32K)(-0.3542 kJ/molK) NB The 'K' cancels out. Then maker the multiplication dG = -54/32 kJ/mol - - 115.94 kJ/mol Note the double minus; it becomes plus(+). Hence dG = -54.32kj/mol + 115.94 kJ/mol dG = (+)61.61 kJ/mol Since dG is positive, the reaction is NOT thermodynamically feasible.
Use the reaction I2(s) I2(g), H = 62.4 kJ/mol, S = 0.145 kJ/(molK), for this question What can be said about the reaction at 500 K?
It is spontaneous.
How do you calculate the volume in liters of 1.50 mol Cl2 at stp?
Use PV =nRT ( pressure at STP is 1 atmosphere and temp. is 298.15 Kelvin ) (1 atm)(volume) = (1.50 mole)(0.08206 Latm/molK)(298.15 K) = 36.7 Liters
What is the heat of formation of NaCl?
The standard enthalpy of formation for sodium chloride is -411,12 kJ/mol.
What is the enthalpy of formation value for nh4cl?
Approximately -82kJ/mol
