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What is the value for G at 100 K if H 27 kJ mol and S 0.09 kJ molK?
TDIXON123
Verified answer
G=18 kJ/mol
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∙ 9y ago
Anonymous
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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 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.
What is the Activation energy value for the decompositition of benzenediazonium chloride in water?
From a university lab result (made by me, the student) the activation energy value for benzenediazonium chloride is supposed to around 100 kJ/mol (100 000 J/mol).
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.
What volume will 1.44 kg of oxygen gas occupy at the planet's aatmospheric pressure?
PV=nRT P=Pressure V=Volume n=mols R=Ideal gas constant (8.3145 m3·Pa/(mol·K)) T=Temperature Atmospheric pressure is highly variable, based upon weather and altitude. Temperature fluctuates as well. Assuming: Pressure 100 KPa Temperature 25 C 100 KPa x V = (1.44kg/32g/mol)(8.3145m3Pa/(molK))(25+273) 100 KPa x V = 45 mol x 8.3145 m3Pa/(molK) x (298) V = 45 x 8.3145 x 298 / 100000 V = 1.115 m3
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
How do you find molarity of NaCl in a saturated solution?
Saturated is 36 - 40 g / 100 mL : Divide grams by the molar mass 58.5 g/mol NaCl and you'll find mol/100 mL Multiplying this value by 10 (= dL/L) and you find mol/L. Doing an estimation gives me approx. 7 mol/L, my calculator is tilted, so I hope your's doing better.
