Description : Given standard enthalpy of formation of `CO(-110 "KJ mol"^(-1))` and `CO_(2)(-394 "KJ mol"^(-1))`. The heat of combustion when one mole of graphite bu
Last Answer : Given standard enthalpy of formation of `CO(-110 "KJ mol"^(-1))` and `CO_(2)(-394 "KJ mol"^(-1))`. The heat ... B. `-284` KJ C. `-394` KJ D. `-504` KJ
Description : The enthalpy of formation of ammonia is `-46.0 KJ mol^(-1)` . The enthalpy change for the reaction `2NH_(3)(g)rarr N_(2)(g)+3H_(2)(g)` is :
Last Answer : The enthalpy of formation of ammonia is `-46.0 KJ mol^(-1)` . The enthalpy change for the reaction `2NH_(3)(g) ... mol^(-1)` D. `-92.0 KJ mol^(-1)`
Description : `Delta_(f)^(@)` for `CO_(2(g)), CO_((g))` and `H_(2)O_((g))` are `-393.5,-110.5` and `-241.8kJ mol^(-1)` respectively. The standard enthalpy change `(
Last Answer : `Delta_(f)^(@)` for `CO_(2(g)), CO_((g))` and `H_(2)O_((g))` are `-393.5,-110.5` and `-241.8kJ mol^(-1 ... A. `524.1` B. `41.2` C. `-262.5` D. `-41.2`
Description : Calculate the enthalpy of vaporisation per mole for ethanol. Given `DeltaS = 109.8 J K^(-1) mol^(-1)` and boiling point of ethanol is `78.5^(@)`.
Last Answer : Calculate the enthalpy of vaporisation per mole for ethanol. Given `DeltaS = 109.8 J K^(-1) mol^(-1)` ... KJ mol^(-1)` D. Some more data is required
Description : The enthalpy of formation of `CO(g), CO_(2)(g),N_(2)O(g)` and `N_(2)O_(4)(g)` is `-110,-393,+81` and 10 kJ / mol respectively. For the reaction `N_(2)
Last Answer : The enthalpy of formation of `CO(g), CO_(2)(g),N_(2)O(g)` and `N_(2)O_(4)(g)` is `-110,-393,+81` and 10 ... is A. `-212` B. `+212` C. `+778` D. `-778`
Description : How much would the boiling point of water increase if 4 mol of NaCl were added to 1kg of water?
Last Answer : Feel Free to Answer
Description : Given that standard heat enthalpy of `CH_(4), C_(2)H_(4)` and `C_(3)H_(8)` are -17.9, 12.5, -24.8 Kcal/mol. The `Delta H` for `CH_(4)+C_(2)Hrarr C_(3)
Last Answer : Given that standard heat enthalpy of `CH_(4), C_(2)H_(4)` and `C_(3)H_(8)` are -17.9, 12.5, -24.8 Kcal ... . `-30.2` Kcal C. 55.2 Kcal D. `-19.4` Kcal
Description : The enthalpy change for a given reaction at `298 K` is `-x cal mol^(-1)`. If the reaction occurs spontaneously at `298 K`, the entropy change at that
Last Answer : The enthalpy change for a given reaction at `298 K` is `-x cal mol^(-1)`. If the reaction occurs ... (-1)` C. Cannot be negative D. Cannot be positive
Description : The value of enthalpy change `(DeltaH)` for the reaction `C_(2)H_(5)OH (l)+3O_(2) (g) rarr 2CO_(2) (g) +3H_(2)O (l)` at `27^(@)C` is `-1366.5 kJ mol^(
Last Answer : The value of enthalpy change `(DeltaH)` for the reaction `C_(2)H_(5)OH (l)+3O_(2) (g) rarr 2CO_(2) (g) + ... 1369. kJ` C. `-1364.0 kJ` D. `-1361.5 kJ`
Description : The enthalpy and entropy change for the reaction, `Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)` are `30KJmol^(-1)` and `105JK^(-1)mol^(-1)` respectively. The temp
Last Answer : The enthalpy and entropy change for the reaction, `Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)` are `30KJmol^(-1)` and ` ... 285.7 K B. 273 K C. 450 K D. 300 K
Description : The enthalpy changes at 298 K in successive breaking of `O-H` bonds of water, are `H_(2)O(g) rarr H(g)+OH(g),DeltaH=498kJ mol^(-1)` `OH(g) rarr H(g)+O
Last Answer : The enthalpy changes at 298 K in successive breaking of `O-H` bonds of water, are `H_(2)O(g) rarr H(g)+OH(g), ... KJ mol"^(-1)` D. `463 "KJ mol"^(-1)`
Description : The enthalpy of combustion of `H_(2)` , cyclohexene `(C_(6)H_(10))` and cyclohexane `(C_(6)H_(12))` are `-241` , `-3800` and `-3920KJ` per mol respect
Last Answer : The enthalpy of combustion of `H_(2)` , cyclohexene `(C_(6)H_(10))` and cyclohexane `(C_(6)H_(12))` are `-241 ... "KJ mol"^(-1)` D. `242 "KJ mol^(-1)`
Description : If the enthalpy of vaporisation of water is `186.5 J mol^(-1)`, then entropy of its vaporisation will be
Last Answer : If the enthalpy of vaporisation of water is `186.5 J mol^(-1)`, then entropy of its vaporisation will be A. `0.5 ... (-1)` D. `2.0KJK^(-1)"mole"^(-1)`
Description : Ionization enthalpy of Li is 520 kJ mol^(-1) while that of F is 1681 kJ mol^(-1) . Explain.
Last Answer : Ionization enthalpy of Li is 520 kJ mol-1 while that of F is 1681 kJ mol-1. Explain.
Description : If a reaction has an enthalpy of -54.32 kJ/mol and an entropy of -354.2 J/(K*mol), what is the Gibbs free Energy at 54.3(degrees c)?
Last Answer : DeltaG = DeltaH - TDeltaS dG = -54.32 kJ/mol - (54'32+273)K(-354.2J/molK) NB Thevtemperature is quoted in Kelvin(K) and the Entropy must be converted to kJ by dividing by '1000'/ Hence dG = ... 115.94 kJ/mol dG = (+)61.61 kJ/mol Since dG is positive, the reaction is NOT thermodynamically feasible.
Description : Standard enthalpy of formation is zero for.
Last Answer : Standard enthalpy of formation is zero for. A. `C_("diamond")` B. `Br_((g))` C. `C_("graphite")` D. `O_(3(g))`
Description : Write an expression in the form of chemical equation for the standard enthalpy of formation (∆Hf) of CO (g).
Last Answer : Ans. C(s) +1/2 O2(g) → CO (g)
Description : Given that the standard free energy change (∆G°) for the hydrolysis of ATP is -7.3 K cal/mol and that for the hydrolysis of Glucose 6-phosphate is -3.3 Kcal/mol, the ∆G° for the phosphorylation of glucose is Glucose + ATP → ... -10.6 Kcal/mol (B) -7.3 Kcal/mol (C) -4.0 Kcal/mol (D) +4.0 Kcal/mol
Last Answer : Answer : C
Description : Can anyone help me with this? Chlorine and carbon monoxide gases are mixed in a 1.00L container and the following equilibrium is established: CO(g) + Cl2(g) COCl2(g).. Initially 1.5 mol of ... monoxide. At equilibrium, 0.8 mol of COCl2(g) was found. How do you calculate the percent reaction?
Last Answer : For a start, your equation isn't balanced; it should be Cl2 (Cl2, not 2Cl, because of HONClBrIF). Given this, if we assume the reaction goes to completion, 1.5 mol Cl2 will produce 1.5 mol ... .3% Incidentally, is that supposed to be CO or Co? It has no effect on the calculation, just curious.
Description : Water (specific heat cv= 4.2 kJ/ kg ∙ K ) is being heated by a 1500 W h eater. What is the rate of change in temperature of 1kg of the water? A. 0.043 K/s B. 0.179 K/s C. 0.357 K/s D. 1.50 K/s Formula: Q = mcv ( T)
Last Answer : 0.179 K/s
Description : Calculate the capacitance of two parallel plates of area 2 units separated by a distance of 0.2m in air(in picofarad) a) 8.84 b) 88.4 c) 884.1 d) 0.884
Last Answer : b) 88.4
Description : How do i Calculate the mass of 2.50 mol of CH3OH(l). Show my work and Use the appropriate number of significant digits in your final answer.?
Last Answer : Answers is the place to go to get the answers you need and to ask the questions you want
Description : A solution of `(+)`-2-chloro-2-phenyl ethane in toluene racemises slowly in the presence of small amount of `SbCl_(5)`, due to the formation of:
Last Answer : A solution of `(+)`-2-chloro-2-phenyl ethane in toluene racemises slowly in the presence of ... carbanion B. carbene C. free radical D. carbocation
Description : Entropy change of the reaction, H2O (liquid) → H2O (gas), is termed as the enthalpy of (A) Solution (B) Vaporisation (C) Formation (D) Sublimation
Last Answer : (B) Vaporisation
Description : The enthalpy change when ammonia gas is dissolved in water is called the heat of (A) Solution (B) Formation (C) Dilution (D) Combustion
Last Answer : (A) Solution
Description : The heat of combustion of carbon and monoxide are -394 and -285 KJ `mol^(-1)` respectively. The heat of formation of CO in KJ `mol^(-1)` is :-
Last Answer : The heat of combustion of carbon and monoxide are -394 and -285 KJ `mol^(-1)` respectively. The heat of formation ... B. `-109` C. `+218` D. `-218`
Description : What shows that the formation of CO 2 releases 393.5 kJ mol?
Last Answer : C(s) + O2(g) + CO2(g) + 393.5 kJ
Description : What is the standard enthalpy change at 298 K for the following reaction? `CO_(2) (g)+ C("diamond") rarr 2CO(g)` Given : `DeltaH_(f)^(@)(CO,g) = - 110
Last Answer : What is the standard enthalpy change at 298 K for the following reaction? `CO_(2) (g)+ C("diamond") rarr 2CO(g ... `+172.5 kJ//mol` D. `170.5 kJ//mol`
Description : A uniform rope of mass M=0.1kg and length L=10m hangs from the celling. `[g=10m//s^(2)]` :-
Last Answer : A uniform rope of mass M=0.1kg and length L=10m hangs from the celling. `[g=10m//s^(2) ... in the rope remain constant along the length of the rope
Description : Evaporation of 1kg of water from a solution in a single effect evaporator requires about __________ kg of steam. (A) 0.4 - 0.6 (B) 1-1.3 (C) 1.8-2 (D) 2 - 2.4
Last Answer : (B) 1-1.3
Description : A vibrating system having mass 1kg, a spring of stiffness 1000N/m and damping factor of 0.632 and it is put to harmonic excitation of 10N. Find the amplitude at resonance. A 0.079 B 7.9C 0.056 D 0.00791
Last Answer : D 0.00791
Description : 1 kg of wood contains 15% moisture and 5% hydrogen by weight. How much water is evaporated during complete combustion of 1kg of wood? a) 0.6 kg b) 200 g c) 0.15 kg d) none of the above
Last Answer : b)200 g
Description : Determine the amount of heat required to produce 1Kg of steam at a pressure of 7 bar, at a temperature 29 degree Celsius, under the following . (i) When the steam is wet having dryness fraction 0.87 (ii) When the steam is dry saturated Assume specific heat = 2.35KJ/KgK
Last Answer : P 7bar T 29ᵒC x=0.9 m =1kg C p =2.35 KJ/KgK At pressure 7 bar saturation Temp T sat =165 ᵒC h f =697.2 KJ/Kg h fg= 2064.8 KJ/Kg i) Heat required when steam is wet ... ) When the stem is dry saturated hg=hf+hfg =2762 kj Heat actually required = 2762-121.8 = 2640.2 kj
Description : Standard entropy of `X_(2)` , `Y_(2)` and `XY_(3)` are `60, 40 ` and `50JK^(-1)mol^(-1)` , respectively. For the reaction, `(1)/(2)X_(2)+(3)/(2)Y_(2)r
Last Answer : Standard entropy of `X_(2)` , `Y_(2)` and `XY_(3)` are `60, 40 ` and `50JK^(-1)mol^(-1)` , respectively ... be: A. 500 K B. 750 K C. 1000 K D. 1250 K
Description : Standard free energy (∆G°) of hydrolysis of creatine phosphate is (A) -–51.4 KJ/mol (B) –43.1 KJ/mol (C) –30.5 KJ/mol (D) –15.9 KJ/mol
Last Answer : Answer : B
Description : Standard free energy (∆G°) of hydrolysis of phosphoenolpyruvate is (A) –61.9 KJ/mol (B) –43.1 KJ/mol (C) –14.2 KJ/mol (D) –9.2 KJ/mol
Last Answer : Answer : A
Description : Standard free energy (∆G°) of hydrolysis of ADP to AMP + Pi is (A) –43.3 KJ/mol (B) –30.5 KJ/mol (C) –27.6 KJ/mol (D) –15.9 KJ/mol
Description : Standard free energy (∆G°) of hydrolysis of ATP to ADP + Pi is (A) –49.3 KJ/mol (B) –4.93 KJ/mol (C) –30.5 KJ/mol (D) –20.9 KJ/mol
Description : The standard free energy of hydrolysis of terminal phosphate group of ATP is (A) –7,300 cal/mol (B) –8,300 cal/mol (C) 10,000 cal/mol (D) +7,300 cal/mol
Last Answer : A
Description : Calculate the most appropriate unit cost for a distribution division of a multinational company using the following information. Miles travelled 636,500 Tonnes carried 2,479 Number of drivers 20 Hours worked by drivers 35,520 Tonnes miles ... 800 (a) Rs .88 (b) Rs 1.50 (c) Rs 15.84 (d) Rs28, 140
Last Answer : (d) Rs28, 140
Description : How is the enthalpy used to calculate the energy required to vaporize a volume of liquid?
Last Answer : Need answer
Description : What is bond enthalpy ? What is its unit ? How we calculate enthalpy in case of complex compound ?
Last Answer : Ans. Amount of energy Required ot break one mole of bonds of particular type b/w two atoms in gaseous state. Its unit is KJ/mole It is obtained by dividing total bond dissociation enthalpy by no. of bonds broken
Description : Formation width for bank for M.G. double line section is (a) 8.50 m (b) 8.84 m (c) 9.65 m (d) 9.81 m*
Last Answer : (d) 9.81 m*
Description : Assertion: The enthalpy of formation of gaseous oxygen molecules at `298K` and under1 atm is zero. Reason: The entropy of formation of gaseous oxygen
Last Answer : Assertion: The enthalpy of formation of gaseous oxygen molecules at `298K` and under1 atm is zero. ... D. If both Assertion & Reason are false.
Description : Since the enthalpy of elements in their natural state is taken to be zero, the heat of formation `(Delta_(f)H)` of compounds
Last Answer : Since the enthalpy of elements in their natural state is taken to be zero, the heat of formation `( ... C. is zero D. May be positive or negative
Description : The enthalpy changes of formation of the gaseous oxides of nitrogen `(N_(2)O` and `NO)` are positive because of `:`
Last Answer : The enthalpy changes of formation of the gaseous oxides of nitrogen `(N_(2)O` and `NO)` are positive ... The tendency of oxygen to form `O^(2-)`
Description : Bond dissociation enthalpy of `H_(2)` , `Cl_(2)` and `HCl` are `434, 242` and `431KJmol^(-1)` respectively. Enthalpy of formation of `HCl` is
Last Answer : Bond dissociation enthalpy of `H_(2)` , `Cl_(2)` and `HCl` are `434, 242` and `431KJmol^(-1)` respectively. ... kJ mol^(-1)` D. `-245 kJ mol^(-1)`
Description : Which reaction shows that the enthalpy of formation of H2S is Hf -20.6 kJmol?
Last Answer : H2(g) + S(s) —> H2S + 20.6 kJ
Description : What is the sign of enthalpy of formation of highly stable compound?
Last Answer : Ans. Negative.
Description : Out of carbon(diamond)and carbon (graphite) whose enthalpy of formation is taken as zero?
Last Answer : Ans. Enthalpy of formation of carbon in the form of graphite is taken as zero because it is a more commonly found in stable form of carbon.