For items 1-4, consider the isothermal expansion of a 1.5 mole of monoatomic gas gas from a pressure of 1 atm to 0.45 atm at 333 K. 1.) What is the work done for the process? A.) -3.32 kJ B.) + 3.32 kJ C.) -2.28 kJ D.) +2.28 kJ E.) 0 kJ 2.) What is the heat transferred for the process? A.) -3.32 kJ B.) +3.32 kJ C.) -2.28 kJ D.) +2.28 kJ E.) 0 kJ 3.) What is the change in internal energy for the process? A.) +7.61 kJ B.) -7.61 kJ C.) +12.6 kJ D.) -12.6 kJ E.) 0 kJ 4.) What is the change in enthalpy for the process? A.) +12.6 kJ B.) -12.6 kJ C.) +17.8 kJ D.) -17.8 kJ E.) 0 kJ

For items 1-4, consider the isothermal expansion of a 1.5 mole of monoatomic gas gas from a pressure of 1 atm to 0.45 atm at 333 K. 1.) What is the work done for the process? A.) -3.32 kJ B.) + 3.32 kJ C.) -2.28 kJ D.) +2.28 kJ E.) 0 kJ 2.) What is the heat transferred for the process? A.) -3.32 kJ B.) +3.32 kJ C.) -2.28 kJ D.) +2.28 kJ E.) 0 kJ 3.) What is the change in internal energy for the process? A.) +7.61 kJ B.) -7.61 kJ C.) +12.6 kJ D.) -12.6 kJ E.) 0 kJ 4.) What is the change in enthalpy for the process? A.) +12.6 kJ B.) -12.6 kJ C.) +17.8 kJ D.) -17.8 kJ E.) 0 kJ

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.88E: The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500...

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The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
My working out is given Heat of capacity is 4.68 J g–1 K–1 and M (mass)= 41.9g-21.2g = 63.1g then temperature, delta T= 43.7 °C- 29.8 °C = 13.9 °C. After you have the delta H or Q = MC(delta)T equation = 63.1 x 4.68 x 13.9 = 4104.7812, but what do you do with the calorimeter constant of 34.7 J K–1 (is that there to trick students or do I use it in conjunction to the Heat of capacity of 4.68 J g–1 K–1 ? I have a second image of a example of a tutor working out but it has two issue of accidently forgetting a minus sign and maybe not including the calorimeter constant.
2C8H18(l) + 25 O2(g) = 16 CO2(g) + 18 H2O(l) The standard enthalpy of formation for H2O(g)is −241.82kJ/mol The standard enthalpy of formation for CO2(g)is −393.5kJ/mol The standard enthalpy of formation for C8H18(l) is −249.9kJ/mol 1)how much CO2 is released from 1 tank of gas? 2) there are 3000 students and employees. Further assume that they all drive, and on an average they consume 1 tank of gas each, every week to get to and from work. If every tank is 12 gallons (1 gallon = 3.785 L) can you estimate how much heat is transferred
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:
The formulas give the enthalpy when Coal and Methane react with oxygen:C+O2->CO2+394 kJ/mol, 12 gram C gives 44 gram of CO2+394 kJCH4+ O2->CO2+2H2O+891 kJ/mol, 16 gram CH4gives 44 gram of CO2+891kJ 1-Calculate the heating value of Coal and Methane in MJ/kg and in kWh/kg.Calculate the lower heating value for Methane. 2-Calculate the amount of CO2 which is produced per kWh for Coal and Methane
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) b) What is the standard enthalpy of reaction per mole of KOH when 50.00 cm3 of 1.0 moldm-3 of Nitric Acid (HNO3) and 50.00 cm3 of 1.0 moldm-3 of Potassium Hydroxide (KOH) are mixed? According to your simulation, the temperature rose by __6.81__ oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1)
a) A 1.60 dm3 sample of a mixture of methane gas, CH4 and oxygen gas, measured at 25 oC and 101 kPa, was allowed to react in a bomb calorimeter in which, had a heat capacity of 5.30 kJ/K altogether with its contents. The complete combustion of the methane gas to carbon dioxide gas and water caused a temperature rise in the calorimeter of 6.28 K. Given that ∆Ho c (CH4) is -560 kJ/mol. i. Define the standard enthalpy of combustion of methane ii. Write a thermochemical equation for the combustion of methane iii. Knowing the ∆Ho c of methane, calculate the number of mole of methane in the mixture. iv. Calculate the total moles of gases in the calorimeter.
What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by ___0.68__ oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below: HCl (aq) + NaOH(aq) à NaCl(aq) + H2O(l)
Several ice cubes (ρi = 0.9167 g/cm3) of total volume Vi = 205 cm3 and temperature 273.15 K (0.000 °C) are put into a thermos containing Vt = 680 cm3 of tea at a temperature of 313.15 K, completely filling the thermos. The lid is then put on the thermos to close it. Assume that the density and the specific heat of the tea is the same as it is for fresh water (ρw = 1.00 g/cm3, c = 4186 J/kgK). a. Calculate the equilibrium temperature TE in K of the final mixture of tea and water. b. Calculate the magnitude of the total heat transferred QT in J from the tea to the ice cubes.
How many kJ of energy need to be added to 50.00 g of Br2 (liq) to raise the temperature of the sample by 5.0 K? The MW of Br2 is 159.81 g/mol. See the Exam 3 handout for the molar heat capacity of liquid Br2.
To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of the material was supplied with 35.548 J of heat causing the temperature of the material to rise from 297.05 K to 461.4 K. What is the specific heat of this material? Report your answer in units of J/(ºC · g) to 4 sig figs, but do NOT include units in your answer.
When, a volume of 200 cm3of Lithium hydroxide solution of concentration 1.00 mol/dm3and 200 cm3of Hydrochloric acid of concentration 100 mol/dm3 were mixed together in acalorimeter the reaction was investigated to be exothermic. Based on the information given above in question one (1), calculated the enthalpychange per mol of water produced, if the heat capacity of the calorimeter was 76 J/Kand the temperature rise was 5.25 K. (State any assumptions made)