SPE Chapter, International University of East Africa

SPE Chapter, International University of East Africa

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AM PROUD TO BE ASTUDENT OF IUEA AND I THEREFORE WELLCOMES STUDENTS TO JOIN IT ,BECAUSE IT'S A UNIVERSITY WHICH UNDERSTANDS EVERYONE REGARDED TO HOME BACK GROUND

PETROLEUM ENGINEERING STUDENTS ASSOCIATION AT THE INTERNATIONAL UNIVERSITY OF EAST AFRICA, KAMPALA UGANDA

Operating as usual

Photos from SPE Chapter, International University of East Africa's post 13/12/2016

Photos from SPE Chapter, International University of East Africa's post

Photos from SPE Chapter, International University of East Africa's post 27/10/2016

Photos from SPE Chapter, International University of East Africa's post

[08/16/16]   IUEA SPE-Chapter welcomes all new students in the university especially thoe aspiring petroleum engineers, the Chapter wishes you well and welcome to the department of stress!

Timeline photos 22/07/2016

Congratulations to two of our Senior SPE Chapter members of the International University of East Africa in Kampala, Uganda for their high performances as they await graduation. 1. Ansumana E.M. Dukuly, Jr. Seated sixth from left and 2. Mawa Joel kinyara seated second from right. We are proud of you guys. SPE Chapter IUEA says congratulations again

Congratulations to two of our Senior SPE Chapter members of the International University of East Africa in Kampala, Uganda for their high performances as they await graduation. 1. Ansumana E.M. Dukuly, Jr. Seated sixth from left and 2. Mawa Joel kinyara seated second from right. We are proud of you guys. SPE Chapter IUEA says congratulations again

[12/05/14]   Final papers are few days away, we wish all aspiring and inspiring petroleum engineering students of International University of East Africa (IUEA)

Timeline photos 05/12/2014

Timeline photos

Timeline photos 13/10/2013

Timeline photos

Timeline photos 13/10/2013

Timeline photos

Timeline photos 13/10/2013

Timeline photos

[09/25/13]   THERMODYNAMICS COURSE WORK
GROUP ONE( QUESTION 1(FIRST LAW)-4(NUMERICAL QUESTION)

MAWA JOEL KINYARA--------HEAD
TARIR DUOK G*I
GAK GABRIEL ANYANG AKOL
ANSUMANA E.M. DUKULY, JR.
TOMBE PETER MORBE
THOMAS LINO BABA
MAKER BOL JOK
AMANI DAVID BALIESIMA
MUBIRU MAHAD
BAKARI HASSAN

GROUP TWO( NUMERICAL QUESTIONS 5-11)
KESIMBO BONU------HEAD MUBIRU MAHAD BISIMWA MAROYI EDDY FRANKLYNE TUGUME ANYWAR MARTIN RUGENDABANGA BWIHANGANE BASONGO RUBI ALPHONSE SSEBULIME DOUGLAS SEKIRANDA HAMZA EDHIRUMA FAHAD
GROUP THREE(QUESTION 12-19
WABWIRE PHILLEX ------HEAD GATLUOK KOANG GACH ZEIN EL ABEDEEN ALI BADWAY ALI NOMWESIGWA BRIAN MUYISA NYUNYU KEYNES LUWAM TEKIE DAVID ELISA MATAYO ROSE KIDEN ALISON BIRUMU KECKOM JAMES

Timeline photos 25/09/2013

Timeline photos

Timeline photos 25/09/2013

Timeline photos

Timeline photos 25/09/2013

Timeline photos

[09/23/13]   Thermodynamics Tutorial Questions
First Law of Thermodynamics
1. Explain the following
i) Isolated system
ii) Closed system
iii) Open system
iv) A state function
v) A path function and give examples in each case
2. State the first law of thermodynamics and give its limitations
3. Explain the difference between the change in internal energy and the change in enthalpy accompanying a chemical or physical process

Numerical problems
1. A chemical reaction takes place in a container of cross-sectional area 50.0 cm2. As a result of the reaction, a piston is pushed out through 15 cm against an external pressure of 121 kPa. Calculate the work done by the system.
2. A sample consisting of 2.00 mol He is expanded isothermally at 22°C from 22.8 dm3 to 31.7 dm3 (a) reversibly, (b) against a constant external pressure equal to the final pressure of the gas, and (c) freely (against zero external pressure). For the three processes calculate q, w, ΔU, and ΔH.
3. A sample consisting of 2.00 mol of perfect gas molecules, for whichCV,m = 5–2R, initially at p1 = 111 kPa and T1 = 277 K, is heated reversibly to 356 K at constant volume. Calculate the final pressure, ΔU, q, and w.
4. A sample of argon of mass 6.56 g occupies 18.5 dm3 at 305 K. (a) Calculate the work done when the gas expands isothermally against a constant external pressure of 7.7 kPa until its volume has increased by 2.5 dm3. (b) Calculate the work that would be done if the same expansion occurred reversibly.
5. A sample of 2.00 mol CH3OH(g) is condensed isothermally and reversibly to liquid at 64°C. The standard enthalpy of vaporization of methanol at 64°C is 35.3 kJ mol−1. Find w, q, ΔU, and ΔH for this process.
6. The constant-pressure heat capacity of a sample of a perfect gas was found to vary with temperature according to the expression Cp /(J K−1) = 20.17 + 0.4001(T/K). Calculate q, w, ΔU, and ΔH when the temperature is raised from 0°C to 100°C (a) at constant pressure, (b) at constant volume.
7. Calculate the final temperature of a sample of carbon dioxide of mass 16.0 g that is expanded reversibly and adiabatically from 500 cm3 at 298.15 K to 2.00 dm3.
8. A sample consisting of 1.5 mol of perfect gas molecules with Cp,m = 20.8 J K−1 mol−1 is initially at 230 kPa and 315 K. It undergoes reversible adiabatic expansion until its pressure reaches 170 kPa. Calculate the final volume and temperature and the work done.
9. Given the reactions (1) and (2) below, determine (a) ΔrH and ΔrU for reaction (3), (b) ΔfH for both HCl(g) and H2O(g) all at 298 K.
(1) H2 (g) + I2(s) →2 HI (g) ΔrH = +52.96 kJ mol−1
(2) 2 H2 (g) + O2 (g) →2 H2O (g) ΔrH = −483.64 kJ mol−1
(3) 4 HI (g) + O2 (g) →2 I2(s) + 2 H2O (g)
10. For the reaction 2 C6H5COOH(s) + 13 O2 (g) →12 CO2 (g) + 6 H2O (g), ΔrU = −772.7 kJ mol−1 at 298 K. Calculate ΔrH

Second Law of Thermodynamics
11. calculate the standard Gibbs energy of the reaction CO (g) + 1/2 O2 (g) →CO2 (g) at 25°C, we write
ΔrG = ΔfG (CO2, g) − {ΔfG (CO, g) + 1/2 ΔfG (O2, g)}
= −394.4 kJ mol−1 − {(−137.2) + 1/2 (0)} kJ mol−1
= −257.2 kJ mol−1
12. Calculate the standard reaction Gibbs energy for the combustion of CH4 (g) at 298 K. [−818 kJ mol−1]


13. Calculate ΔS (for the system) when the state of 2.00 mol diatomic perfect gas molecules, for which Cp,m = 7–2R, is changed from 25°C and 1.50 atm to 135°C and 7.00 atm. How do you rationalize the sign of ΔS?
14. A sample consisting of 2.00 mol of diatomic perfect gas molecules at 250 K is compressed reversibly and adiabatically until its temperature reaches 300 K. Given that CV,m = 27.5 J K−1 mol−1, calculate q, w, ΔU, ΔH, and ΔS.
15. Calculate the change in the entropies of the system and the surroundings, and the total change in entropy, when the volume of a sample of argon gas of mass 21 g at 298 K and 1.50 bar increases from 1.20 dm3 to 4.60 dm3 in (a) an isothermal reversible expansion, (b) an isothermal irreversible expansion against pex = 0, and (c) an adiabatic reversible expansion
16. The enthalpy of vaporization of methanol is 35.27 kJ mol−1 at its normal boiling point of 64.1°C. Calculate (a) the entropy of vaporization of methanol at this temperature and (b) the entropy change of the surroundings.
17. The change in the Gibbs energy of a certain constant-pressure process was found to fit the expression ΔG/J = −73.1 + 42.8(T/K). Calculate the value of ΔS for the process.
18. Calculate the change in the molar Gibbs energy of oxygen when its pressure is increased isothermally from 50.0 kPa to 100.0 kPa at 500 K.
19. Calculate the change in chemical potential of a perfect gas when its pressure is increased isothermally from 92.0 kPa to 252.0 kPa at 50°C.

Thermodynamics Tutorial Questions
First Law of Thermodynamics
1. Explain the following
i) Isolated system
ii) Closed system
iii) Open system
iv) A state function
v) A path function and give examples in each case
2. State the first law of thermodynamics and give its limitations
3. Explain the difference between the change in internal energy and the change in enthalpy accompanying a chemical or physical process

Numerical problems
1. A chemical reaction takes place in a container of cross-sectional area 50.0 cm2. As a result of the reaction, a piston is pushed out through 15 cm against an external pressure of 121 kPa. Calculate the work done by the system.
2. A sample consisting of 2.00 mol He is expanded isothermally at 22°C from 22.8 dm3 to 31.7 dm3 (a) reversibly, (b) against a constant external pressure equal to the final pressure of the gas, and (c) freely (against zero external pressure). For the three processes calculate q, w, ΔU, and ΔH.
3. A sample consisting of 2.00 mol of perfect gas molecules, for whichCV,m = 5–2R, initially at p1 = 111 kPa and T1 = 277 K, is heated reversibly to 356 K at constant volume. Calculate the final pressure, ΔU, q, and w.
4. A sample of argon of mass 6.56 g occupies 18.5 dm3 at 305 K. (a) Calculate the work done when the gas expands isothermally against a constant external pressure of 7.7 kPa until its volume has increased by 2.5 dm3. (b) Calculate the work that would be done if the same expansion occurred reversibly.
5. A sample of 2.00 mol CH3OH(g) is condensed isothermally and reversibly to liquid at 64°C. The standard enthalpy of vaporization of methanol at 64°C is 35.3 kJ mol−1. Find w, q, ΔU, and ΔH for this process.
6. The constant-pressure heat capacity of a sample of a perfect gas was found to vary with temperature according to the expression Cp /(J K−1) = 20.17 + 0.4001(T/K). Calculate q, w, ΔU, and ΔH when the temperature is raised from 0°C to 100°C (a) at constant pressure, (b) at constant volume.
7. Calculate the final temperature of a sample of carbon dioxide of mass 16.0 g that is expanded reversibly and adiabatically from 500 cm3 at 298.15 K to 2.00 dm3.
8. A sample consisting of 1.5 mol of perfect gas molecules with Cp,m = 20.8 J K−1 mol−1 is initially at 230 kPa and 315 K. It undergoes reversible adiabatic expansion until its pressure reaches 170 kPa. Calculate the final volume and temperature and the work done.
9. Given the reactions (1) and (2) below, determine (a) ΔrH and ΔrU for reaction (3), (b) ΔfH for both HCl(g) and H2O(g) all at 298 K.
(1) H2 (g) + I2(s) →2 HI (g) ΔrH = +52.96 kJ mol−1
(2) 2 H2 (g) + O2 (g) →2 H2O (g) ΔrH = −483.64 kJ mol−1
(3) 4 HI (g) + O2 (g) →2 I2(s) + 2 H2O (g)
10. For the reaction 2 C6H5COOH(s) + 13 O2 (g) →12 CO2 (g) + 6 H2O (g), ΔrU = −772.7 kJ mol−1 at 298 K. Calculate ΔrH

Second Law of Thermodynamics
11. calculate the standard Gibbs energy of the reaction CO (g) + 1/2 O2 (g) →CO2 (g) at 25°C, we write
ΔrG = ΔfG (CO2, g) − {ΔfG (CO, g) + 1/2 ΔfG (O2, g)}
= −394.4 kJ mol−1 − {(−137.2) + 1/2 (0)} kJ mol−1
= −257.2 kJ mol−1
12. Calculate the standard reaction Gibbs energy for the combustion of CH4 (g) at 298 K. [−818 kJ mol−1]


13. Calculate ΔS (for the system) when the state of 2.00 mol diatomic perfect gas molecules, for which Cp,m = 7–2R, is changed from 25°C and 1.50 atm to 135°C and 7.00 atm. How do you rationalize the sign of ΔS?
14. A sample consisting of 2.00 mol of diatomic perfect gas molecules at 250 K is compressed reversibly and adiabatically until its temperature reaches 300 K. Given that CV,m = 27.5 J K−1 mol−1, calculate q, w, ΔU, ΔH, and ΔS.
15. Calculate the change in the entropies of the system and the surroundings, and the total change in entropy, when the volume of a sample of argon gas of mass 21 g at 298 K and 1.50 bar increases from 1.20 dm3 to 4.60 dm3 in (a) an isothermal reversible expansion, (b) an isothermal irreversible expansion against pex = 0, and (c) an adiabatic reversible expansion
16. The enthalpy of vaporization of methanol is 35.27 kJ mol−1 at its normal boiling point of 64.1°C. Calculate (a) the entropy of vaporization of methanol at this temperature and (b) the entropy change of the surroundings.
17. The change in the Gibbs energy of a certain constant-pressure process was found to fit the expression ΔG/J = −73.1 + 42.8(T/K). Calculate the value of ΔS for the process.
18. Calculate the change in the molar Gibbs energy of oxygen when its pressure is increased isothermally from 50.0 kPa to 100.0 kPa at 500 K.
19. Calculate the change in chemical potential of a perfect gas when its pressure is increased isothermally from 92.0 kPa to 252.0 kPa at 50°C.

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