Calculate Δ? for the reaction:
2CH4 (g) + 3O2 (g) → 2 CO (g) + 4H2O (l)
using the following combustion antipyres:
∆c? (CH4, g) = -890 kJ mol-1 and Δc? (CO, g) = -283 kJ mol-1
Calculate Δ? for the reaction: 2CH4 (g) + 3O2 (g) → 2 CO (g) + 4H2O...
which of the following statements is not true about the reaction 2CH4+3O2 = 2CO2+4H2O a. Water is a reactant b. Methane and carbon dioxide are products c. Methane is a product d. Water and carbon dioxide are products
For the following reaction: 2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CH3OH (l) -238.40 127.19 O2 (g) 0.00 205.70 CO2 (g) -393.51 213.74 H2O (l) -285.83 69.91 Determine the temperature (to two decimal places in K) such that the reaction is in equilibrium in its standard states.
Calculate the heat of reaction AH for the following reaction: 2 CH 4(g)+302(9)2 CO(g) + 4H2O(g) You can find a table of bond energies by using the Data button on the ALEKS toolbar. Round your answer to the nearest kJ/mol. kJ X mol
For the following reaction: 2CH4(g) + O2(g) → 2CO(g) + 4H2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CH4 (g) -74.87 188.66 O2 (g) 0.00 205.70 CO (g) -110.53 197.66 H2 (g) 0.00 130.68 Calculate ΔG°rx (in kJ) at 345.31 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). Assume ΔH°f and S° do not vary as a function of temperature.
2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g)?H°f (kJ mol-1)S° (J K-1 mol-1)NH3(g)-46193O2(g)0205CH4(g)-75186HCN(g)135.1202H2O(g)-242189The above reaction is used in the industrial production of hydrogen cyanide. (The tabulated values ?H°fand S° are for 25°C. For the purposes of this question assume that ?H° and ?S° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.)?H° is -939.8?S° is 165Calculate ?G° at 1005°C, for this equation.Are the following statements about this process True...
What is the enthalpy of the reaction for the following equation: 2CH3OH(l) + 3O2(g) -----> 2CO2(g) + 4H2O(g) Given the following bond enthalpies (in kj/mol): C-H (414); C-O (360); C=O (799); O=O (498); O-H (464). Note: O=C=O
(a) Diborane (B2H6) is a highly reactive borohydride that can be used as rocket fuel. Calculate Δ? for synthesis from the elements as: 2B (s) + 3H2 (g) → B2H6 (g) Use the following data: 4B (s) + 3O2 (g) → 2B2O. (S) Δ? = -2546 kJ mol-1 B2H6 (g) + 3O2 (g) → B2O3 (s) + 3H2O (g) Δ? = -2035 kJ mol-1 2H2 (g) + O2 (g) → 2H2O (l) Δ? = -572 kJ mol-1 H2O (l) →...
Calculate the standard combustion enthalpy of propylene at 25 ° C using the standard formation enthalpy of liquid water (-286 kJ mol-1) and the following reactions: 1) CH2CHCH3 (g) + H2 (g) → CH3CH2CH3 (g); Δ? (1) = -125 kJ mol-1 2) CH3CH2CH3 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (l); Δ? (2) = -2220 kJ mol-1 3) H 2 (g) + 0.5O2 (g) → H2O (l);Δ? ((3) = -286 kJ mol-1
At 298 K, evaluate deltaG(kJ) and deltaE (V) for
2CH3OH(l) + 3O2(g) -> 4H2O(g) + 2CO2(g)
S (J/mol-K) AH°y (kJ/mol) So (J/mol-K) AH(kJ/mol) Substance Substance N2(g) CH-ОН() 126.8 0 191.5 -238.6 CO(g) NH3(g) 197.9 192.5 -110.5 -46.2 CO2(g) NO(g) 213.6 +90.4 210.6 -393.5 NO2(g) +33.8 240.5 H2(g) HNO3(aq) 130.6 146.0 -206.6 H2O( 69.9 -285.8 O2(g) 188.8 H2O(g) 0 205.0 -241.8
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:...