State the First Law of Thermodynamics.

Use this information to complete the table below.

A student dissolves 11.0 g of ammonium chloride (NH, CI) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water fall from 20.0 °C to 16.8 °C over the course of 6 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH,CI(s) NH (aq) + Cl (aq) db You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ kJ…

also, Change in Gibbs Free energy Reaction Spontaneity

Calculate the standard change in Gibbs free energy, AGixn, for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. KCI(s) K+ (aq) + Cl(aq) AGxn= Determine the concentration of K+ (aq) if the change in Gibbs free energy, AGran, for the reaction is -8.21 kJ/mol. [K+] = kJ/mol M

Give correct detailed Solution

2. Please calculate the standard enthalpy of reaction (AHrxn, in kJ/mol) for the preparation of nitrous acid, HNO2, using the thermodynamic data given below. Preparation of nitrous acid: HCl(g) + NaNO2(s) → HNO2(1) + NaCl(s) 2NaCl(s) + H₂O(l) → 2HCl(g) + Na₂O(s) NO(g) + NO₂(g) + Na2O(s) → 2NaNO2 (s) NO(g) + NO₂(g) → N₂O(g) + O₂(g) 2HNO2(1)→ N₂O(g) + O2(g) + H₂O(g) H₂O(1)→ H₂O(g) ΔΗ = 507.31 kJ/mol AH = -427.14 kJ/mol AH = - 42.68 kJ/mol 34.35 kJ/mol ΔΗ ΔΗ = 44.012 kJ/mol =

Use the following information to calculate the standard free energy change (AG°) and equilibrium constant (K) for the following system: CaCO3(s) = CaO(s) + CO2(g) T= 900.0 °C AH;° values (kJ/mol): CaO(s) = -634.9, CO2(g) = -393.51, CaCO3(s) =–1220.0 %3D S° values (J/mol K): CaO(s) = 110.0, CO2(g) = 213.8, CACO3(s) = 38.1 %3D %3D %3D

Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation of NH3 (g) is -104 kJ/mol at 298 K, calculate the equilibrium constant, K, at this temperature. To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.

At constant pressure and 25°C, the ΔrH° for the following reaction is –1560 kJ/mol C2H6(g) + 3.5O2(g) → 2CO2(g) +0.5 H2O(l) What is the enthalpy change for the oxidation of 5 g of C2H6?