For the reaction CH4 (g) + N2 (g) + 164 kJ 6 HCN(g) + NH3 (g) at 25degrees C and 1 atm of pressure ÄGo = 159 kJ. Calculate ÄSo at 25degrees C. ÄHfo for CH4 (g) = -74.77 kJ/mol and ÄHfo for NH3 (g) = -46.09 kJ/mol. What is ÄHfo for HCN(g) ?
Delta S (standard conditions) for the following reaction is favorable even though delta H (standard conditions) is not: C2H5OH (l) <-> C2H5OH (g) Assume that ethanol boils at the temperature where delta G (standard conditions) for this reaction becomes zero. Use the values of delta H and delta S for this reaction to estimate
1) Calculate the heat of combustion for C2H6 from the following information: C2H4+3O2-> 2CO2+2H2O C2H4+H2->C2H6 H2+1/2O2->H2O 2) Discuss the idea that the standard of living in society might be measured in units of kJ/person available in that society. The unit itself is called energy in chemical reactions if that helps
Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction 2 NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) Given that delta G^o = -13.6 kJ, calculate delta G at 25 oC for the following sets of conditions. (a) 10 atm NH3, 10 atm CO2, 1.0 M NH2CONH2 (b) 0.1 atm NH3, 0.1 atm CO2, 1.0 M NH2CON
The Enthalpy Change of a Chemical Reaction Procedure #1: 1. Take a calorimeter from the Glassware shelf and place it on the workbench. 2. Take a balance from the Tools shelf and drop it on the calorimeter. Record the mass of the empty calorimeter. 3. Take a thermometer from the Tools shelf and drop it onto the calo
1. A sample of N2 gas occupies 2.40 L at 20oC. If the gas is in a container that can contract or expand at constant pressure, at what temperature will the N2 occupy 4.80 L? 10oC 40oC 146oC 313oC 685oC 2. When 0.56 g of Na(s) reacts with excess F2(g) to form NaF(s), 13.8 kJ of heat is evolved at standard-state cond
I just need the calculation part done. The mass of the solutes is as follows: .502g Tris and .4999g KNO3 and .4995g Pb(NO3)2 Solution Calorimetry: Heat of Ionic Reaction Solution Calorimetry is a convenient way of experimentally determining the heat of reaction in a liquid medium. Measurements in this lab will be made
1. Consider this data for compound X: ΔHf 505.4 J/g ΔHvap= 3489J/g Specific heat: X (s) = 0.96 J/g °C, X (1) = 3.88 J/g °C, X (g) = 1.21 J/g °C Normal boiling point: 46.8 °C Normal freezing point: - 29.8 °C a. Calculate the total energy change if 10.0 grams of X is changed from 11.0 °C to 88.9 °C. b. Write
A) The pressure of a monoatomic ideal gas in a closed system is reversibly and isochorically (constant volume) increased. Determine whether each of the following quantities is less than, equal to, or greater than zero. ΔT ΔV w q ΔP ΔU ΔH ΔS b) A real gas is found to have a molar volume that is 90% of the
Suppose that the enthalpy of some substance over a large temperature range can be expressed as a function of the temperature (where alpha, beta and gamma are constants): H =alpha*ln(T) + ln(gamma) + beta/T^2 a) What is the heat capacity of this substance at constant pressure? b) You begin with two samples each contai
A process run infinitesimally slowly at equilibrium and reversed to its original state Motion of a frictionless pendulum Evaporation of water from a cup Solid and liquid water combined together at STP Ice melting to water above the melting point Isothermal expansion of a real gas Please see the attache
I completed part A and the second part asks: What can be said about the spontaneity of this reaction? C diamond to C graphite The reaction (as written) is spontaneous. The reverse reaction is spontaneous. the system is in equilibrium at 298 K.
From the values given for delta H* and delta S*, calculate delta G* for each of the following reactions at 298 K. If the reaction is not spontaneous under standard conditions at 298 K, at what temperature (if any) would the reaction become spontaneous? a) 2 PbS (s) + 3 O2 (g) ---> 2 PbO (s) + 2 SO2 (gO
Methods of Finding DeltaG and K (Gibb's Free Energy and Equilibrium Constant) from Standard Tabulated Thermodynamic Quantities.
Write the equilibrium -constant expression and calculate the value of the equilibrium constant for each of the follow reactions at 298 K, using data from Appendix C. ** Appendix C is in the Chemistry: The Central Science 11e textbook. It is a chemistry 100 (first year book). The Appendix contains delta Hf, delta Gf and S at
A body generates 5900kJ of energy/h during heavy exercise. How many grams of C6H12O6 is needed for 22 minutes of exercise? C6H12O6 burns at 4.00 kcal/g. Find the mass of potato chipes needed to eat to not lose weight. Full solution please thank you
For the reaction: H2 + C2H4 -> C2H6 In gaseous phase, the pre-exponential factor is 1.24*10^6 [M-1s-1] and the activation energy is 180 kJ/mol. find the entropy, the enthalpy and the gibbs free energy. see attachment
Calculate the enthalpy for the combustion of pentane. Please see the attached file for the fully formatted problems. Part B The combustion of pentane, , occurs via the reaction with heat of formation values given by the following table: Substance ( ) 35.1 393.5 241.8 Calculate the enthalpy for th
2 moles of a compound are allowed to react in a foam coffee cup that contains 160 grams of water. The reaction caused the temperature of the water to rise from 21 to 24.7 degrees Celsius. What is the enthalpy of this reaction? Assume that no heat is lost to the surrounding or to the coffee cup itself. Please answer in kilojou
A 1.00-L bulb of methane at a pressure of 10.0 kPa is connected to a 3.00-L bulb of hydrogen at 20.0 kPa; both bulbs are at the same temperature. (a) After the gases mix, what is the total pressure? (b) What is the mole fraction of each component in the mixture? Every time I start to answer this question I always end up wit
For a certain ideal gas, Cv = 2.5R for all temperatures. Calculate q, w, ΔU and ΔH when 2.00 mol of this gas undergoes each of the following processes: (a) a reversible expansion at a constant pressure of 1 bar from a volume of 20.0 dm3 to 40.0 dm3. (b) a reversible isothermal compression from (0.50 bar, 40.0 dm3)
1.) Use the values of ∆Hof given below to calculate (in kJ) ∆Horxn for the following reaction: C2H5OH (l)+ 3O2(g) → 2CO2(g) + 3H2O(g) Given: ∆Hof (kJ/mol) C2H5OH (l) -278 O2(g) 0 CO2(g) -394 H2O(g) -242 2.) The graph below shows the heating curve of water. Use this graph to answer the fol
In a combustion cylinder, the total internal energy change (delta E) from the burning of a fuel is -174 kJ. The cooling system that surrounds the cylinder absorbs 47 kJ as heat. a.) How much work can be done by the fuel in the cylinder? b.) Assuming an initial volume of 100.0 L and an external pressure of 1.00 atm, what is the
These are questions that relate to kinetics calculations from absorbance data. Please see the attached file for the fully formatted problems. Please provide a full explanation of what is right and wrong.
Please see the attached file for the fully formatted problem(s). Heat, Energy, and Changes of State Part A How much energy in joules would be absorbed by 3.0 L of liquid oxygen as it vaporized? The density of liquid oxygen at its boiling point is 1.14 kg/L , and its heat of vaporization is 213 kJ/kL . Express yo
Question 5 Consider the equilibrium reaction: NO2(g) + CO(g) ----> NO(g) + CO2(g) DHrxn = -226.4 kJ Which one of the following factors would cause the equilibrium constant value to increase? Please explain. a. ) Addition of a catalyst. b. ) Removal of O2 gas. c. ) Addition of SO2 gas. d. ) Decrease the
How do I figure out the quantity of heat produced when 6.20g of butane is completely combusted in air under standard conditions?
Please see the attached file for full problem descriptions: 1. A quantity of 0.20 mol of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C (s) + CO2 (g) <--> 2CO (g) Under these conditions, the average molar mass of the gas was
Please see the attached file and show work. The following reaction, which takes place just before the citric acid cycle, is catalyzed by the enzyme lactate dehydrogenase CH3COCOO- + NADH + H+ <----> CH3CH(OH)COO- + NAD+ From the data listed in Table 7.2, calculate the value of Gibb's free energy change deltaG and the equ
Please see the attached file. (a) 4Fe (s) + 3O2 (g) --> 2Fe2O3 (s) (b) O(g) + O (g) --> O2 (g) (c) NH4Cl (s) --> NH3(g) + HCl (g) (d) H2 (g) + Cl2 (g) --> 2HCl (g)
How much heat (energy) is required to convert 52.0 g of ice at -10.0 degree C to steam at 100 degree C? specific heat of ice: 2.09 J/g degree Celsius Delta H fus specific heat of water: 4.18 J/g Celsius Delta H vap= 40.7 kJ/mol specific heat of steam: 1.84 J/g Celsius