Enthalpy of solution = deltaH solution = m × Cs × deltaT
where m is mass , Cs is specific heat capacity and deltaT is change in temperature
Here deltaH solution = 113958 J , m = 5.5 g , Cs = 4.18 J / g °C
So , deltaT = deltaH solution / ( m × Cs )
= 113958 J / ( 5.5 g × 4.18 J / g °C )
= 113958 J / ( 22.99 J / °C )
= 4956.85 °C
Ionic Compound Mass (g) T i (°C ) Tf (°C) ∆T (°C) q (J) ∆H (J/mol) Calcium chloride 5g 22°C 34°C +12°C -251J Ammonium nitrate 5g 22°C 16°C -6°C +125J Magnesium Carbonate 2g 21°C 21°C 0°C 0 Sodium chloride 5g 21°C 20°C -1 +21J Cs (water) = 4.18 J/g-°C , Density of water = 1g/mL Q) Calculate: ∆H (J/mol), for the four ionic compounds?
Calculate the enthalpy change, Delta H process in which 32.5 g water is converted from liquid at 18.9 C to vapor 25.0 degrees C. For water Delta H vap =44.0 kJ/mol at 25.0 °C and Cs=4.18 J/(g*^ C) for H2O (l)
Assuming that the specific heat of the solution is 4.18
J/(g⋅∘C) and that the calorimeter itself absorbs a negligible
amount of heat, calculate ΔH in kilojoules for the reaction.
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8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol
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Using the values of Delta H and Delta S given, calculate Delta G for each of the reactions at 25 degree C and indicate whether the reactions are spontaneous or non-spontaneous. Explain. Delta H = 10.5 kJ/mol and Delta S = 30.0 J/K-mol Delta H = -10.5 kJ/mol and Delta S = 105. J/K-mol
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A) For the reaction 4HCl(g) + O2(g)---->2H2O(g) + 2Cl2(g) Delta H° = -114.4 kJ and Delta S° = -128.9 J/K The equilibrium constant for this reaction at 306.0 K is _______? Assume that Delta H° and DeltaS° are independent of temperature. B) For the reaction N2(g) + 3H2(g)---->2NH3(g) Delta H° = -92.2 kJ and Delta S° = -198.7 J/K The equilibrium constant for this reaction at 333.0 K is ___? Assume that Delta H° and Delta S° are independent of...
What are the signs (+ or -) for delta H, delta S, and -T(delta S) which are required to produce the following signs (+ or -) of delta G. Think about the equation delta G = delta H - T(delta S). 1. If delta G is negative 2. If delta G is either positive or negative (there are 2 solutions) 3. If delta G is negative
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