# H2 + F2--> 2HF deltaH = 518.0 kJ H2 ----> 2H deltaH = 436.8 kJ F2 ---> 2F deltaH = 158.2 kJ (a) calculate Delta H for H + F---> HF (b) what is the standard enthalpy change of formation

368 results
1. ## Chem

In photosynthesis, plants form glucose and oxygen from carbon dioxide and water. 6CO_2+6H_2O --> C_6H_12_O_6+6O_2 a) Calculate deltaH rxn at 15 degree C b) Calculate deltaS rxn at 15 c) Calculate deltaG rxn at 15 thanks!

2. ## Chemistry

How much heat is absorbed/released when 20.00 g of NH2 reacts in the presence of excess O2 to produce NO and H2O according to the following chemical equation: 4NH3 + 5O2 --> 4NO + 6H2O, deltaH= +1168 kJ. The answer is 342.9 kJ of heat absorbed. I want to

3. ## Chemistry!

Consider the equilibrium system: N204 (g) = 2 NO2 (g) for which the Kp = 0.1134 at 25 C and deltaH rx is 58.03 kJ/mol. Assume that 1 mole of N2O4 and 2 moles of NO2 are introduced into a 5 L contains. What will be the equilibrium value of [N204]? Options

4. ## Chemistry

Calculate Delta H for the reaction CH4(g)+NH3(g)-->HCN(g)+3H2(g) given, N2(g)+3H2(g)->2NH3(g) DeltaH=-91.8kj C(s)+2H2(g)->CH3(g) DeltaH=-74.9kj h2(g)+2C(s)+N2(g)->2HCN(g) DeltaH=270.3kj

5. ## chemistry

how to calculate delta h for the reaction 2B(s)+3H2(g)arrow B2H6(g)given the following data: 2B(s)+3/2O2(g)arrowB2O3(s) deltaH=-1273kj B2H6(g)+3O2(g)arrowB2O3(s)+3H2O(g) deltaH=-2035kj H2(g)+1/2O2(g)arrowH2O(l) deltaH=-286kj H2O(l)arrowH2O(g) deltaH=+44kj

6. ## Chemistry

Given: Cu2O(s) + 1/2 O2(g) → 2CuO(s) deltaH°= -144 kJ 2Cu2O(s) → 2Cu(s) + 2CuO(s) deltaH°= 22 kJ Calculate the standard enthalpy of formation of CuO(s).

7. ## Chemistry

H2 + F2--> 2HF deltaH = 518.0 kJ H2 ----> 2H deltaH = 436.8 kJ F2 ---> 2F deltaH = 158.2 kJ (a) calculate Delta H for H + > HF (b) what is the standard enthalpy change of formation of F2 Help please!!! i think this is easier than i'm making it. for (b)

8. ## Chemistry

Given the following equations: 2 H2 (g) + O2 (g)--> 2 H2O (l) deltaH = -571.6 kJ N2 (g) + O2 (g)-->2 NO (g) deltaH = +180.5 kJ N2 (g) + 3 H2 (g) --->2 NH3 (g) deltaH = -92.22 kJ Determine the enthalpy change (deltaH) for the following reaction: 2 NO (g) +

9. ## Chem

Calculate delta H for the formation of one mole of N2O5 from the elements at 25 degrees C using the following data. 2H2 + O2 - 2H2O delta H = -571.6 kJ N2O5 + H2O - 2HNO3 deltaH = -73.7 kJ 1/2N2 + 3/2O2 + 1/2H2 - HNO3 delta H = -174.1 kJ

10. ## Chem

Calculate the enthalpy change in the reaction of H2 with F2 to produce HF. The H–H and F–F bond energies are 436 and 155 kJ/mol, respectively, and the H–F bond energy is 567 kJ/mol H2 (g) + F2 (g) --> 2HF (g)

11. ## Chemistry

Calculate the standard enthalpy change for the reaction 2C8H18(l)+17O2(g)> 16CO(g) + 18H2O(l) Given 2C8H18(l)+25O2(g)>16CO2(g)+18H2O(l) deltaH=-11020 kj/mol 2CO(g)+ O2(g)>2CO2(g) Delta H=-566.0 kj/mol The > is supposed to be an arrow :)

Find the value of delta H net for the following equation: SnBr2(s) + TiCl4(l) -> TiBr2(s) + SnCl4(l) Use the following reactions to help solve for the net value: 1) SnCl2(s) + TiBr2(s) -> SnBr2(s) + Ticl2(s) Delta H=+4.2 2) SnCl2(s) + Cl2(g) -> TiCl4(l)

13. ## Chemistry

Calculate DeltaHrxn for the following reaction: C + H2O --> CO + H2 Use the following: C + O2 --> CO2 DeltaH = -393.5 kJ 2CO + O2 --> 2CO2 DeltaH = -566.0 kJ 2H2 + O2 --> 2H2O Delta H = -483.6 kJ DeltaHrxn = ?

14. ## Chemistry

Rewrite the following using a thermochemical equation with a deltaH value: a) The standard molar enthalpy of combustion for propane is -2220kJ/ mol.

15. ## Chemistry

How much heat is absorbed/released when 35.00 g of NH3(g) reacts in the presence of excess O2(g) to produce NO(g) and H2O(l) according to the following chemical equation? 4NH3(g)+5O2(g)--->4NO(g)+6H2O(l) DeltaH=1168kj

16. ## General Chemistry

Calculate the standard heat of formation of acetaldehyde , 2C(s) + 2 H2(g) +1/2 O2 (g) ---> CH3CHO(g) given the following information? CH3CHO(g) + 5/2 O2 (g) --> 2H2O(l) + 2 CO2(g) DeltaH rxn =-1194 KJ H2(g)+ 1/2 O2 (g) --> H2O (l) DeltaH rxn =-286 KJ/mol

17. ## help !! chemistry

H2O(g) + Cl2(g) 2 HCl(g) + ½ O2(g) Heat of Reaction is WebAssign will check your answer for the correct number of significant figures. kJ Changed: Your submitted answer was incorrect. Your current answer has not been submitted. Information: COCl2(g) +

18. ## Chemistry

Determine ∆G° (in kcal) for the reaction CCl4(ℓ) + H2(g) HCl(g) + CHCl3(ℓ) at 25 °C under standard conditions. The following information is available: At 25 °C C(graphite) + 2Cl2(g) CCl4(ℓ) ∆S° = -56.23 cal K-1 C(graphite) + Cl2(g) + H2(g)

The deltaS for a reaction is 3.0 J/(mol*K) at 25 degrees C. Caluculate the deltaG for the reaction when DeltaH = -394 kL and determine whether it will occur spontaneously at this temperature

20. ## Chemistry

Copper metal can be obtained by heating copper oxide in the presence of carbon monoxide, CO, according to the reaction: CuO(s) + CO(g) --> Cu(s) + CO2(g) Calculate Delta H° in kJ using the following thermochemical equations. Reactions 2CO(g) + O2(g) -->

21. ## Chemistry2

WO3 (s) + 3 H2 (g) -> W (s) + 3 H20 (g) Tungsten is obtained commercially by the reduction of WO3 with hydrogen according to the equation above. The following data related to this reaction are available. DeltaH(kilojoules/mole) for WO3 is -839.5. DeltaH

22. ## Chemistry

An exothermic reaction is spontaneous above 400K but non spontaneous below it. Of the deltaH for the reaction is -40.0 kcal, what are the values of deltaS and deltaG at 400K?

23. ## Chemistry

Hydrazine, N2H4, is a colorless liquid used in rocket fuel. What is the enthalpy change for the process in which hydranzine is formed from its elements? N2(g) + H2(g) => N2H4(l) Use the following reactions and enthalpy changes: N2H4 + O2 => 2H2O DeltaH =

24. ## chemistry

C3H6O + 4O2 --> 3CO2(g) + 3H2O(g) deltaH= -1790kJ the density of C3H6O is 0.79g/mL. HOw much heat is released by the combustion of 150mL of acetone?

25. ## Chemistry

CO(g) + 2H_2(g) CH_3OH (g) deltaH=-90.7kJ Methanol is prepared industrially from synthesis gas (CO and H_2) Would the fraction of methanol obtained at equilibrium be increased by raising the temperature? Explain. Thank you :)

26. ## Chemistry Lab

Data and Calculations: 1. Volume of water in calorimeter: 100.0 mL 2. Mass of water in calorimeter (water's density 1.00g/mL): 100.0g 3. Initial Temperature of water in calorimeter:19.5 degrees Celsius 4. Final Temperature of water in calorimeter: 3.0

27. ## chem

HNO3 (g) + 4H2 (g) ---> NH3 (g) + 3H2O (g) deltaH = -637 kJ Calculate the enthalpy change when one mole of hydrogen reacts; and What is the enthalpy change when 10.00 g of ammonia is made to react with excess of steam to form nitric acid and hydrogen

28. ## chemistry

given the following thermochemical equations: 4B(s) + 3O2(g) -> 2B2O3(s) deltaH=-2509.1 kJ 2H2(g) + O2(g) -> 2H2O(l) deltaH=-571.70 kJ B2H6(g) + 3O2(g) -> B2O3(s) + 3H2O(l) deltaH=-2147.5 kJ calculate the standard enthalpy of formation (in kJ.mol^-1) of

29. ## chemistry

DeltaH and DeltaU are nearly the same in all the following processes except a.F2(g)+H2(g) --> 2HF(g) b.3O2(g) --> 2O3(g) c.CuO(s) +H2(g) --> Cu(s) +H20(g) d.CH4(g) +CI2(g) --> CH3Cl(g) +HCl(g) e.C6H6(s) --> C6H6(l)

30. ## Chemistry

The change in entropy for a reaction is 3.0 J/(mol·K) at 25°C. Calculate the change in free energy for the reaction when ΔH = –394 kJ/mol and determine whether it will occur spontaneously at this temperature. Is the answer -395 kJ/mol? and second

31. ## chemistry

Chlorobenzene boils at 131.8C. Use Trouton's Rule to estimate deltaH of vaporization.

32. ## chemistry

HNO3 (g) + 4H2 (g) „³ NH3 (g) + 3H2O (g)deltaH = -637 kJ Calculate the enthalpy change when one mole of hydrogen reacts and What is the enthalpy change when 10.00 g of ammonia is made to react with excess of steam to form nitric acid and hydrogen gases?

33. ## SCIENCE 1

for following reaction at equilibrium if we increase the reaction temperature the equilibrium will 2SO3(g)2SO2(g)+O2(g)(deltaH degrees=198kJ) A. not shift B.the question can not be answered because Keq is not given C.shift to the right D. shift to the left

34. ## chemistry

Consider these reactions where M represents a generic metal 1. 2M(s) +6HCl(aq) --> 2MCl3(aq)+3H2(g) (deltaH)= -725.0 kj 2. HCl(g)-->HCl(aq) (deltaH)= -74.8kj 3. H2(g)+CL2(g) --> 2HCl(g) (deltaH)=-1845.0kj 4. MCL3(s) --> MCl3(aq) (deltaH)= -476.0kj Use the

35. ## Chemistry

In the equation Q = mc(deltaT), I learned that Q means heat transfer. Is it the heat transfer from the system to the surroundings, i.e. the system loses/absorbs heat or is it from the surroundings to the system? A couple of places on the Internet say that

36. ## chemistry

To which one of the following reactions occurring at 25°C does the symbol deltaH°f[H2SO4(l)] refer

37. ## Chem

Calculate the enthalpy change in the reaction of H2 with F2 to produce HF. The H–H and F–F bond energies are 436 and 155 kJ/mol, respectively, and the H–F bond energy is 567 kJ/mol H2 (g) + F2 (g) --> 2HF (g)

38. ## Chemistry

If you were to prepare a 1.00 molal solution of CaCl2 beginning with water at 27.0 C, what would the final temperature of the solution be (in C)? Assume that the specific heats of both pure H2O and the solution are the same, 4.18 J/K*g. The dissolution of

39. ## Chemistry

Glycine,C2H502N, is important for biological energy.Find the heat of combustion deltaHrxn. Delta H [C2H5O2N]=-537.3 kj/mol DeltaH [ CO2(g)=-393.5 kj/mol DeltaH[H2O(l)]-285.8 kj/mol

40. ## Chem

Hydrogen peroxide decomposes according to the following: H2O2--> H2O(l) + 1/2O2(g); deltaH = -98.2kJ Calculate the change in enthalpy, deltaH, when 1.00g of Hydrogen peroxide decomposes

41. ## Chemistry

The combustion of benzoic acid releases 26.38kJ/g and is often used to calibrate a bomb calorimete. The combustion of 1.045g of benzoic acid caused the temperature of the calorimeter to rise by 5.985 degreeC.Using the same calorimeter, a sample of 0.876g

42. ## Chemistry

How much heat is evolved when 500kg of Ammonia is evolved according to the following equation: N2(g)+3H2(g)2NH3(g) [deltaH =-91.8K]

43. ## Chemistry

calculate the enthalpy for the reaction D + F = G + H using G + C = A + B deltaH = 277 C + F = A delta H = 303 D = B + H delta H = -158

1)Which thermochemical equation and data does not agree with the other two written? a) 2NO (g)+ O2 (g) ->2 NO2 (g) deltaH=-169.8 b) NO (g) + 1/2 O2 (g) -> NO2 (g) delta H = -56.6 c) 4 NO2 (g) -> 4 NO (g) + 2 O2 (g) delta H = +226.4 d)all three equations

45. ## Chemistry

Hydrochloric acid reacts with Magnesium to form Magnesium Chloride and Hydrogen gas. deltaH= -442kJ If 15mL of 1.0M HCl reacts with .3g of Mg, how many L of H2 are produced? How much heat is produced?

46. ## Thermochemistry

How many Joules of heat are required to completely convert 80.0g of water at 60 Degrees Celsius to steam at 100 Degrees Celsius *NOTE THE VALUES ARE IN kJ per MOL c=4.179 J/gC, DeltaH-Fusion = 6.01 kJ/mol, DeltaH-Vaporization= 40.7 kJ/mol

47. ## Chemistry

If 0.120 moles of water are produced in the reaction H+(aq)+OH-(aq)=H2O deltaH=-56.2kj/mol

48. ## chemistry

calculate the enthalpy of formation, per mole, of sucrose, C12H2211O(s). C12H22O11(s) + 12O2(g) --> 12CO2(g) +11H2O(l) deltaH=-5.65*10^3 kJ

49. ## Chem 2

need to figure out how to calculate. the value of DeltaH for the reaction below is -72kj_____kj of heat are released when 1.0 mole of HBr is formed in this reaction. H2(g)*Br2(g)> 2HBr(g) I know the answer is 36 but need help

50. ## Chemistry 2

When 5.0g of CaCl2 was dissolved in 50 ml of water in a coffee cup calorimeter, the temperature of the solution rose from 22.3C to 30.5C. What is the qsoultion in J and what is the qrxn in J? What is the deltaH in kJ/mol of CaCl2 dissolved?

51. ## chemistry

2CO2(G)--->2CO(g)+O2(g), deltaH=566kj what is Kc and state whether the reaction favors products or reactants? A.)[CO2]=1.5M, [CO]=1.2M, [O2]=0.05M B.)[CO2]=8.3M, [CO]=0.05M, [O2]=0.50M C.)[CO2]=0.05M, [CO]=0.75M, [O2]=0.07M any work would be much

52. ## Chem

I don't understand the effect of temperature on a reaction. For exmaple: CO + 3H2 CH4 + H2O deltaH= -230 KJ If there were an increase in temperature then the CH4 and H2O would have a harding time becoming the CO and H2 so therefore the reaction would move

53. ## AP Chemistry

Hey guys! I'm really lost on this equation. Any help? H2(g) yIelds 2H(g) Delta H = 436 kJ/mol F2(g) yields 2F(g) DeltaH = 158 kJ/mol H(g) + F(g) yields HF(g) DeltaH = -568 kJ/mol Calculate deltaH for: H2(g) + F2(g) yields 2 HF(g)

54. ## Chemistry

Calculate deltaH for the reaction NO (g) + O (g) ----> NO2(g) given following NO + O3 ----> NO2 + O2 deltaH=-198.9 kj O3 ---> 3/2 O2 deltaH= -142 kj O2 -----> O2(g) deltaH=495

55. ## Chemistry

Find the value of delta H net for the following equation: SnBr2(s) + TiCl4(l) -> TiBr2(s) + SnCl4(l) Use the following reactions to help solve for the net value: 1) SnCl2(s) + TiBr2(s) -> SnBr2(s) + Ticl2(s) Delta H=+4.2 2) SnCl2(s) + Cl2(g) -> TiCl4(l)

56. ## Maths

Transform the following relationships/funtions into linear form and identify expressions for the x and y variables. a) (x^2/a^2) + (y^2/b^2) = 1 where a and b are constants. b) k(T) = (kT/h)exp((deltaS)/R)exp(-(deltaH)/RT) where k, deltaS, deltaH and R are

57. ## physics

A toy cannon fires a .11 kg shell with initial velocity vi=10m/s in the direction 52 degrees above the horizontal. The shell's trajectory curves downward because of gravity, so that time t=.61 s the shell is below the straight line by some vertical

58. ## chemistry

Gibbs free energy What is the equilibrium constant at 25 C? deltaG= deltaH - (T(K)+deltaS) deltaS= -121.1 deltaH= -77.36 so at 25 C deltaG = -77.36 - (298*(-121.1)) deltaG ~ 3.6*(10^4) so my question is: what *is* the equilibrium constant, or perhaps more

59. ## chemistry

if my reaction is 2Na + 2H2O -> 2NaOH +H2, and i have been given 1 gram of sodium, how would i measure the theoretical change in heat of the reaction, assuming the reactants are at room temperature? Look in your text, probably in the appendix, for delta H0

60. ## Math - exponential function

Find all real numbers that satisfy (6^x)(7^(2x)) = 86, 436. Here's what I did: ln(6^x)(7^(2x)) = ln86,436 ln(6^x) + ln(7^2x) = ln86,436 x = [ln(86,436)] / [(ln(6) + (2)ln(7)] x = 2 Please correct my answer! Thanks.

61. ## Chemistry

ln 555.6/281.1 = -deltaH vap/8.314J/k mol [1/256.1K - 1/242K]. I have to solve for delta Hvap. I know that the left side would be7.21. I am not sure what step to do next.

62. ## CHEM HELP!!!

The solubility of AgCl(s) in water at 25 C is 1.33x10^-5 M and its deltaH of solution is 65.7 kJ/mol . What is its solubility at 60.1 C ? Please explain how to solve for this!!

63. ## Physics

What is the gibbs free energy for the reaction a)temperature b)800 degrees celsius c)comment on whether the reactions are spontaneous or not (CHEMICAL REACTION) deltaH = -100kJ delta S= -200 J/K

64. ## Chemistry

Consider the reaction 2H2O(g) --> 2H2(g) + O2(g) deltaH = +483.6 kJ/mol at a certain temperature. If the increase in volume is 32.7 L against an external pressure of 1.00 atm, calculate deltaU for the reaction. (1 L * atm = 101.3 J)

65. ## Chemistry

The amount of solar radiation received anually in arizona is about 8.4 x 10^6 KJ/m^2. What mass of carbon must be burned into carbon dioxide to produce the same amount of energu in the following reaction? C + 02 --->CO2 deltaH=-393.5Kj

66. ## chemistry

The water gas shift reaction used commercially to produce H2(g): CO (g)+ H2O (g) --> CO2 (g) + H2(g). DeltaH=-41.2 kJ/mol Delta S= -42.1 J/mol*K Delta G= -28.6 kJ\mol Determine Kp at 850 K

67. ## ap chemistry

What is the activation energy Ea for this reaction? Answer in units of kJ The deltaH is 160 kJ X is at 160 (beginning of reaction) Y is at 300 (end of reaction)

68. ## chem

it has been a while since ive done these so i just need a refresher. im looking for the heat of hydration of lithium chloride and sodium chloride. compound Lattice Energy deltaH soln LiCl -834 kj/mol -37.0 kj/mol NaCl -769 kj/mol +3.88 kj/mol what is delta

Use the equation for the synthesis of hydrogen to answer the following. C (s) + H2O (l) -> CO (g) + H2 (g) deltaH = + 31.3 kcal/mol carbon deltaS = +32 cal/(mol•K) Calculate the energy change (deltaH) when 5.00 g of carbon is consumed. Calculate the

70. ## college chem 2

Calculate the deltaS univ for the dissolving of NaCl at room temp. S' NaCl(s)=72.11 J/k*mol; S' NaCl(aq)=115.5 J/k*mol;deltaH' NaCl(s)=-411.12 kJ/mol; deltaH' NaCl(aq)=-407.27 kJ/mol.

71. ## chemistry

In which case will the equilibrium constant (K) be less than 1 at 298 K? (a) DeltaH = 4.55 kJ/mol ,deltaS = 28.0 J/mol K (b) delta H = - 4.55 kJ/mol ,deltaS = 28.0 J/mol K (c)deltaH = 4.55 kJ/mol ,deltaS= - 28.0 J/mol K (d) both (a) and (b) I know the

72. ## Chemistry

Mg(s) + 2 HCl(aq) --> MgCl2(aq) + H2 (g) DeltaH= -4.6x10^2 kJ How much heat is evolved when 0.598 g of Mg are dissolved in excess HCl? I'm not sure how to go about this problem. What I thought to do was: 0.598 g x 1 mol Mg/24.31 g Mg x 2 mol HCl/ 1 mol Mg

73. ## chem

1. Calculate the heat (calories) produced by the solution of 3.75 g of NaOH Hint: Remember that the reaction is exothermic. 2. Calculate the number of calories that would be produced if one mole of sodium hydroxide was dissolved. (Î”HsolnNaOH) For #1.

74. ## Chemistry

If 0.120 moles of water are produced in the reaction H+(aq)+OH-(aq)=H2O deltaH=-56.2kj/mol

75. ## Chemistry

If 0.120 moles of water are produced in the reaction H+(aq)+OH-(aq)=H2O deltaH=-56.2kj/mol what is qrxn

76. ## science

For the following reaction if the reaction temperature was increased would the equilibrium shift to the right or the left,not shift at all,or you cant answer the question because Keq is not given? 2SO3(g)2SO2(g)+O2(g)..(deltaH degrees =198kj) Why???

77. ## Chemistry

When a 8.00 g of KBr is dissolved in water in a calorimeter that has a total heat capacity of 4.6 kJ·K^-1 the temperature decrases by 0.290 K. Calculate the molar heat of solution of KBr in kJ/mol. DeltaH soln = ?

78. ## Physical Chemistry1

One mole of an ideal monatomic gas at 300 K and 1 atm is compressed adiabatically by application of a constant external pressure of 25 atm until mechanical equiliibrium is achieved. Calculate the final temperature of the gas, as well as q, w, deltaU and

For the equation: deltaHrxn = qrxn / mol substance to calculate deltaH per mole what does the mol substance mean? Does this mean that you use the mm of the substance or if you already calculated the # of moles of a substance do you use that?

80. ## Chemistry

For the equation: deltaHrxn = qrxn / mol substance to calculate deltaH per mole what does the mol substance mean? Does this mean that you use the mm of the substance or if you already calculated the # of moles of a substance do you use that?

81. ## chemistry

HNO3 (g) + 4H2 (g) ---> NH3 (g) + 3H2O (g) deltaH = -637 kJ Calculate the enthalpy change when one mole of hydrogen reacts; and What is the enthalpy change when 10.00 g of ammonia is made to react with excess of steam to form nitric acid and hydrogen

82. ## Physical Chemistry Help!

I am posting a link to the jpeg file of the physical chemistry homework i need help with, because everytime I try typing it out, I just get wierd symbols. If somebody could please help, that would be greatly appreciated! Thanks~ =) img.photobucket. com/

83. ## chemistry

it has been a while since ive done these so i just need a refresher. im looking for the heat of hydration of lithium chloride and sodium chloride. compound Lattice Energy deltaH soln LiCl -834 kj/mol -37.0 kj/mol NaCl -769 kj/mol +3.88 kj/mol what is delta

84. ## Check 1 question.

Help please!i'm not sure if i'm right. Honestly i'm not that confident about most of my work. In which of the following thermochemical equations would the deltaH be considered a heat of solution? C6H6 (s)--> C6H6 (l), deltaH = +9.87 kJ 2C8H18(l) + 25O2

85. ## Chemistry Check

Determine the missing values of deltaH in the diagram shown below ^ | ^ N2O3(g) + 1/2 O2(g) (Enthalpy)| | ^ | | deltaH= +16.02 | | | | | | 2 NO2(g) | | | ^ | |deltaH=? | | | | | | deltaH=?| | | | | | | | N2(g)+202(g) | Answer: Delta H for the right= 66.36

86. ## Chemistry

Use the equation for the synthesis of hydrogen to answer the following. 10 points. C (s) + H2O (l) -> CO (g) + H2 (g) deltaH = + 31.3 kcal/mol carbon deltaS = +32 cal/(mol•K) Calculate the energy change (deltaH) when 5.00 g of carbon is consumed.

87. ## chemistry

1. the solubility of AgCl in water is 3.97x10^-6 at 0*C and 1.91X10^-4 at 100*C. calculate Ksp for AgCl at each temp. 2. using the data from #1 and the clausius- Clapeyron equation, calculate deltaH* and deltaS* for the formation of a saturated solution of

88. ## Chemistry

Calculate the free energy (ΔG˚) of reaction (kJ) for the equation as written at 298 K (Dependence of temperature on enthalpy can be disregard). If the answer is negative, enter the sign and then the magnitude. Express your answer to three significant

89. ## chemistry

calculate the enthalpy of formation, per mole, of sucrose, C12H2211O(s). C12H22O11(s) + 12O2(g) --> 12CO2(g) +11H2O(l) deltaH=-5.65*10^3 kJ

90. ## pre-ap chemistry

HOW MANY GRAMS OF OCTANE WOULD BE NEEDED TO RELEASE 3,500 kJ OF HEAT? 2C8H18 + 25O2-----> 16CO2 + 18H2O DeltaH= -5,530 kJ/mole of reaction

91. ## Chemistry

K1 = 0.727 K2 = 12.1 T1 = 2000 T2 = 3000 Solve for the standard enthalpy of formation. They gave me the formula ln(K2/K1) = DeltaH /R (T2 - T1 / T1T2) The answer is supposed to be in KJ/mol and I keep getting 2.022 but its not right. I'm not sure what Im

92. ## chemistry

Is deltaH standard of TdeltaS standard more important in determining whether KHT will be soluble in water at a given temperature?

93. ## chemistry

Delta H is given and is-6186.0 Calculate the difference, deltaH-deltaE=delta(PV) for the combustion reaction of 1 mole of methyl octane. (Assume standard state conditions and 298 K for all reactants and products.)

94. ## Chemistry

What is the entropy of CH3OH? My CRC tables list 239.865 J/K*mol @ 298.15o K. Do you also know the enthalpy? deltaHof= -201.000 kJ/mol according to the CRC Handbook,1995-96 edition.

95. ## Chemistry

If DeltaH for the reaction I2 (s) Delta 2I (g) is 153 kJ/mol. What is the longest wavelength of light that can break an I – I bond? In other words, what is the minimum energy, expressed in terms of wavelength, required to break one I – I bond?

96. ## chemistry

A+B ---- C deltaH=-100kj and temp.=25C which direction would the reaction shift if.. a. the concentration of A was decreased b. the concentration of C was increased c. The temp. was increased to 100C

97. ## chemistry

2CO2(G)--->2CO(g)+O2(g), deltaH=566kj what is Kc and state whether the reaction favors products or reactants? A.)[CO2]=1.5M, [CO]=1.2M, [O2]=0.05M B.)[CO2]=8.3M, [CO]=0.05M, [O2]=0.50M C.)[CO2]=0.05M, [CO]=0.75M, [O2]=0.07M

98. ## Chem

In photosynthesis, plants form glucose and oxygen from carbon dioxide and water. 6CO_2+6H_2O --> C_6H_12_O_6+6O_2 a) Calculate deltaH rxn at 15 degree C b) Calculate deltaS rxn at 15 c) Calculate deltaG rxn at 15 thanks!

99. ## Chemistry

N2 and O2 gases react to form dinitrogen pentoxide(N2O5).Calculate deltaH and deltaU for this process per mol of N2 gase knowing that when 101.7g of N2 react with 102.97g of O2 at 25DegC and a constant pressure of 1 atm, 533.5kJ of energy is released as

100. ## chemistry

If I use 0.524g of Mg to react with 60.0mL of 1.0M H+. The density of H+ is 1.00 g/mL, and the specific heat capacity equals what water's is. The Final and Initial temp. are 65.8 and 22. Mg(s) + 2H+(aq) ----> Mg2+(aq) + H2(g) so to find the deltaH of this

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