Part A
Use the following data at 298.15 K to complete this problem:
ΔH∘R(kJ⋅mol−1) | |
1/2H2(g)+1/2O2(g)→OH(g) | 38.95 |
H2(g)+1/2O2(g)→H2O(g) | -241.841 |
H2(g)→2H(g) | 435.994 |
O2(g)→2O(g) | 498.34 |
Assuming ideal gas behavior, calculate ΔH∘R and
for the following reaction:
OH(g)→H(g)+O(g)
Express your answer to five significant figures and include the appropriate units.
Part B
Assuming ideal gas behavior, calculate ΔU∘R and for the following reaction: OH(g)→H(g)+O(g)
Express your answer to five significant figures and include the appropriate units.
Part C
Assuming ideal gas behavior, calculate ΔH∘R and for the following reaction: H2O(g)→2H(g)+O(g)
Express your answer to five significant figures and include the appropriate units.
Part D
Assuming ideal gas behavior, calculate ΔU∘R and for the following reaction: H2O(g)→2H(g)+O(g)
Express your answer to five significant figures and include the appropriate units.
Part E
Assuming ideal gas behavior, calculate ΔH∘R and for the following reaction: H2O(g)→H(g)+OH(g)
Express your answer to five significant figures and include the appropriate units.
Part F
Assuming ideal gas behavior, calculate ΔU∘R and for the following reaction: H2O(g)→H(g)+OH(g)
Express your answer to five significant figures and include the appropriate units.
Part A Use the following data at 298.15 K to complete this problem: ΔH∘R(kJ⋅mol−1) 1/2H2(g)+1/2O2(g)→OH(g) 38.95...
6. Use the following data at 298.15 K to complete this problem: ( mol) 8.95 241.841 435.994 498.34 H2(g)-+2H(g) 02g) 20g) a) Assuming idealgas bechuavion, calculate standard enhalpy change for the the following reaction: OHH0) b) Assuming ideal gas behavior, calculate At Sachon and for the following reaction: H20g-2H(g)+0(g) c) Assuming ideal gas behavior, calculate Affo R and for the following reaction: H:0gHgOHg)
Consider the exothermic reaction CH4(g)+2O2(g)→CO2(g)+2H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero. Reactant or product ΔH∘f (kJ/mol) CH4(g) -201 CO2(g) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate units.
Calculate ΔG∘R at 594 K assuming that ΔH∘R is constant in the temperature interval of interest. Part A Calculate ΔGe for the reaction Express your answer to four significant figures and include the appropriate units. CO(g) + ,02 (g) CO2 (g) at 298.15 K ΔGR: -2572x105 J-mol 1 Previous Answers Correct Part B Calculate ΔGk at 594 K assuming that ΔΗ¡ is constant in the temperature interval of interest Express your answer to four significant figures and include the appropriate...
PART A. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g) Express your answer using four significant figures. PART B. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(g) Express your answer using three significant figures. PART C. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: C(s)+O2(g)→CO2(g) Express your answer using four significant figures. PART D. Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction:...
Hess's Law Given the following data: P(s) + 3/2H2(g) → PH3(g) ΔH°= +5.0 kJ PH3(g) + 2O2(g) → H3PO4(l) ΔH°= -1272.0 kJ 2P(s) + 5/2O2(g) → P2O5(s) ΔH°= -1492.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°= -286.0 kJ calculate ΔH° for the reaction: H3PO4(l) → 1/2P2O5(s) + 3/2H2O(l) ΔH°=?? also please explain how you found the answer
Part A) What is ΔH∘rxn for the following chemical reaction? CO2(g)+2KOH(s)→H2O(g)+K2CO3(s) You can use the following table of standard heats of formation (ΔH∘f) to calculate the enthalpy of the given reaction. Element/ Compound Standard Heat of Formation (kJ/mol) Element/ Compound Standard Heat of Formation (kJ/mol) H(g) 218 N(g) 473 H2(g) 0 O2(g) 0 KOH(s) −424.7 O(g) 249 CO2(g) −393.5 K2CO3(s) −1150kJ C(g) 71 H2O(g) −241.8kJ C(s) 0 HNO3(aq) −206.6 Express the standard enthalpy of reaction to three significant figures and...
Calculate KP at 499 K for the reaction NO(g) + 1/2O2(g) → NO2(g) assuming that ΔH°R is constant over the interval 298-600 K.
Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D Use the following data: Substance ΔH∘fΔHf∘ (kJ/mol)kJ/mol) AA -273 BB -417 CC 223 DD -475 Express your answer to three significant figures and include the appropriate units.
2. Given the following data: H2O(l) → H2(g) + 1/2O2(g) ΔH° = 285.8 kJ 2HNO3(l) → N2O5(g) + H2O(l) ΔH° = 76.6 kJ 2N2(g) + 5O2(g) → 2N2O5(g) ΔH° = 28.4 kJ Calculate ΔH° for the reaction: 1/2N2(g) + 3/2O2(g) + 1/2H2(g) → HNO3(l) Note that you should be able to answer this one without needing to use any additional information from the thermo table. I've attempted this question multiple times. I am able to get to the simplified eqaution...
Part A Hydrogen and oxygen combine to form H,O via the following reaction: 2H2(g) + O2(g) → 2H2O(g) How many liters of oxygen (at STP) are required to form 14.9 g of H2O? Express the volume to three significant figures and include the appropriate units. HMÅ O ? VE Value Units Submit Request Answer