Since no physical data is given so its value could be pridicted in term of postive and negtive
1) ∆s would be positive because 3 mole gas and 1 mole solid is giving 2 mole of solid amd 3 mole of gas.
2) ∆s is negtive because no of moles decreases in product hence less randomness
3)∆s is negtive because reactants have 6 mole of has while product has 3 mole of gas
4) ∆s ~ 0 means it aprrosches to zero butits value is less than 0 because size of aluminum atom is more than Fe
5) ∆s is postive because product have more moles of gas.
Question 4 [10] Predict the value of AS for the following reactions. (a) Au2S3(s) + 3H2(g)...
Determine which of the following chemical equations are correctly balanced. Fe2O3(s)+CO(g)→2Fe(s)+CO2(g) Al2S3(s)+H2O(l)→2Al(OH)3(s)+3H2S(g) 2Cr(s)+3O2(g)→Cr2O3(s) SiO2(s)+4HF(aq)→SiF4(g)+2H2O(l)
For each of the following reactions, calculate the grams of indicated product when 17.2 g of the first reactant and 10.5 g of the second reactant are used. Part B: Fe2O3(s)+3H2(g)→2Fe(s)+3H2O(l) Calculate the mass of Fe. Part C Al2S3(s)+6H2O(l)→2Al(OH)3(aq)+3H2S(g) Calculate the mass of H2S
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ
question 17.57 entropy change for H2(g) + CuO(s) → H2O(0) + Cu(s) 17.56 Use the data in Appendix G to calculate the standard entropy change for 2Al(s) + Fe2O3(s) → Al2O3(s) + 2Fe(s) OBJECTIVE Define Gibbs free energy and relate the sign of a Gibbs free-energy change to the direction of spontane- ous reaction. 17.57 Calculate AGº for the following reactions and state whether each reaction is spontaneous under standard con- ditions at 298 K. (a) Fe2O3(s) + 2Al(s) →...
Which of the following reactions would ΔH = ΔE? 2Al(s) + 6HCl(aq) --> 2AlCl3(aq) + 3H2(g) CaCO3(s) --> CaO(s) + CO2(g) C(s) + O2(g) --> CO2(g) C3H4(g) + 4O2(g) --> 3CO2(g) + 2H2O(l) Zn+2(aq) + 2OH-(aq) --> Zn(OH)2(s)
Calculate the enthalpy of reaction for the following reaction: Question 19 Not yet answered Marked out of 1.00 Fe2O3(s) + 3CO(g) – 2Fe(s) + 3C02(9) P Flag question AH °(Fe2O3(s)) = -824.2 kJ/mol AH°(CO(g)) = -110.5 AH°(Fe(s)) = ? AH°(CO2(g)) = -393.5 kJ/mol Answer:
Which of the reactions are exothermic? 2 Mg(s) + 0, (g) 2 MgO(s) + heat NH, (g) + HCl(g) NH,Cl(s) + heat AgCl(s) + heat — Ag+ (aq) + CI+ (aq) 2 Fe2O3(s) + 3 C(s) + heat - 4Fe(s) + 3 CO2(g) C(graphite) + O2(g) — CO2(g) + heat CH,(g) + 2O2(g) — CO2(g) + 2 H2O(1) + heat about us Careers privacy policy terms of use contact us help %
10. A student determines the value of the equilibrium constant to be 3.99x1013 for the following reaction. 4HCK(g) + O2(g) +2H2O(g) + 2Cl2(g) Based on this value of Keq AGⓇ for this reaction is expected to be (greater, less) than zero Calculate the free energy change for the reaction of 2.45 moles of HCl(e) at standard conditions at 298K. AGºrx Submit Answer Retry Entire Group 9 more group attempts remaining A student determines the value of the equilibrium constant to...
Question 13 Given the following reactions Fe2O3(s) + 3CO(g) →2Fe(s) + 3CO2(g) 3Fe(s) + 4CO2(g) + 4CO(g) + Fe3O4(s) AH° = -28.0 kJ AH° = +12.5 kJ the AH° of the reaction 3Fe2O3(s) + CO(g) + CO2(g) + 2Fe3O4(s) is