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13 Calculate AHo, 298K for the following reaction: CO(g)1/2 O2(g) CO2(g) Given: AHof,298K (in kJ mol-1):...
termine AHo for the combustion of ethanol. Given: AHof (in kJ mol-1): C2H5OH(): -277.69 CO2(g): -393.51 H2O(l): -285.83 • 13. Calculate AHO, 298K for the following reaction: CO(g) + 1/2 02(g) 2 CO2(g) Given: A Hof,298K (in kJ mol-1): CO(g): -110.53 CO2(g): -393.51
1.(3pts) Use the following data to determine the AH.. of 2 CH109) + 13 O2(g) ---> 8 CO2(g) + 10 H2O(1) Data: Substance AH(kJ/mol) Substance AH(kJ/mol CzH.(g) CH2OH() C4H10g) CH2(1) H2O(g) CO(g) O2(g) -239.0 -126.15 -156.4 -241.82 -110.53 C:H:(8) CH,OH(g) CsH (8) CH (1) H.O(1) CO2 N (8) -104.0 -2010 -146.44 + 12.0 -285.83 -393.51 0 2.(2pts) If you are given 158,0 g 0_(g) and a sufficient amount of the other reactant, calculate the heat associated with reaction in problem...
Given that ΔfG°(CO(g))=-137.17 kJ mol-1, ΔfG°(O2(g))=0 kJ mol-1, ΔfG°(CO2(g))=-394.36 kJ mol-1 the reaction 2CO(g)+O2(g) →2CO2(g) is spontaneous or non-spontaneous ?
Use Hess's law to determine Ofor the reaction → CO2(g),given that C(graphite) +202(8) — CO(8) A Hº = -110.54 kJ mol C(graphite) + O2(8) —CO2(g) A Hº = -393.51 kJ mol
Calculate the heat of reaction in (kJ) for the following reaction: 2CO(g) + O2(g) --> 2CO2(g) given the following data: C + 1/2O2 --> CO(g) delta H= -110.5 KJ/mol C + O2(g) --> CO2(g) delta H= -393.5 KJ/ mol
1.(3pts) Use the following data to determine the AHıxn of 2 C3H12O(l) + 15 O2(g) ----> 10 CO2(g) + 12 H2O(1) Substance AH(kJ/mol) Substance AH(kJ/mol) Data: CzH.(g) CH,OH(1) C.H.0(1) C6H40(1) H2O(g) CO(g) O2(g) 20.9 -239.0 -277.0 -316.0 -241.82 -110.53 C3H2(g) CHOH(9) CH 20(1) CH;60(1) H2O(1) -104.0 -201.0 -298.6 -340.0 -285.83 -393.51 CO2 N (8) 2.(2pts) If you are given 148,0 g O2(g) and a sufficient amount of the other reactant, calculate the heat associated with reaction in problem 1 and...
For the following reaction: CS2(g) + 3O2(g) → CO2(g) + 2SO2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CS2 (g) 116.70 237.80 O2 (g) 0.00 205.70 CO2 (g) -393.51 213.74 SO2 (g) -296.84 248.20 Calculate ΔG°rx (in kJ) at 794.8 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.
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.
Calculate the standard enthalpy of formation of CS2() given that AH=-393.5 kJ/mol AHo = -296.4 kj/mol a. C(s) + O2(g) CO2lg) b. S(s) +O2(g). SO2(g) AH = -1073.6 kj/mol C. CS2(I)+302(g) Co2lg) + 2S02(B)
4. Given the following standard enthalpy of formations: AH° C,H,OH() =-277.7 kJ/mol]; AHO [CH CO H) = 484.5 kJ/mol]; AH° [HO) = -285.8 kJ/mol]; AH° (O,(g) 0 kJ/mol] UnvIL Calculate the LDH for the reaction. CH.OHI)+0,(g)- CH,CO,H() H,O()