H2(g) + Cl2(g) ---------> 2HCl(g)
H0rxn = [2H0f(HCl)] - [H0f(H2) + H0f(Cl2)]
- 186 = [2H0f(HCl)] - [ 0 + 0]
[2H0f(HCl)] = - 186
H0f(HCl) = - 93.0 KJ
answer = - 93.0
The value of ΔH° for the reaction below is-186 k. H2 (g) + Cl2 (g)-> 2HCl...
Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g) ΔH =-184.6 kJ/mol If 5.0 moles of H2 reacts with 5.0 moles of C12 to form HC1 at 1.0 atm, what is Δ U for this reaction? Assume the reaction goes to completion and Δ V= 0 L (The conversion factor is 1 L·atm = 101.3 J.) kJ
DH=DUIDIN 1. In following reaction H2(g) + Cl2(g) + 2HCl(g) AH=- 184.6 kJ/mol If 4 moles of H2 react with 4 moles of Cl, to form HCI. Calculate AU for this reaction, assumimg the reaction goes to completion against a pressure of 138.0 atm at constant volume. (IL atm = 101.3 J) pranai DU=q tw A) -738.4 kJ B) -369.2 kJ C) 138.0 kJ D) 184.6 kJ E) 244.5 kJ 4H =-92.3 ou-bH
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Hydrogen sulfide decomposes according to the following reaction, 2 H25(g)2 H2(g)+S2(g) Δ5° = +78.1 J/K, ΔH° = +169.4 kJ. The reaction is spontaneous at O T< 2169 K O T>1891 K O T1891 K T> 2169 K
the reaction 2HCl=H2(g)+Cl2(g) has a Kc=3.2x10^-32.A 0.500-L reaction vessel initially contains 0.025 mol of HC The reaction 2HCI(g)Hlg) + Cl(e) has a K 0.025 mol of HCI. 3.2x103. A 0.500-L reaction vessel initially contains A. Write an equation for Ke using the chemical entities. B. Set up and complete an ICE table C. Determine the equilibrium concentrations of H2 and Ch. To receive full credit, you must show any appropriate substitutions and all of your algebra work. Use the attached...
The reaction of hydrogen and chlorine gases produces hydrogen chloride. Cl2(g) + H2(g) → 2HCl(9) AHºrn =-184 kJ/mol Calculate the quantity of heat evolved if 180.g of chlorine reacted with 4.0 g of hydrogen. (a) (b) (c) (d) (e) -180 kJ 470 kJ 370 kJ 2.5 kJ 180 kJ
A student measures the reaction H2(g) + Cl2(g) <=> 2 HCl(g) concentrations at a few different temperatures and obtains the equilibrium constant. The student wants to use the van't Hoff equation to roughly determine the reaction enthalpy assuming that it does not change over the region of interest. T(K) 300 500 1000 Keq 4x1031 4x108 So the student plots the data in the Ink vs 1/T diagram and obtains a linear fitting shown below: 80 4x1018 60 In(K) 40 20...
Calculate Δ Hrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions and their ΔH values: C(s)C(s)H2(g)+++2H2(g)2Cl2(g)Cl2(g)→→→CH4(g),CCl4(g),2HCl(g),ΔH=−74.6 kJΔH=−95.7 kJΔH=−184.6 kJ
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For the reaction 2HBr(g) + Cl2(g)—>2HCl(g) + Brz(9) AH° = -81.1 kJ and AS° = -1.2 J/K The equilibrium constant for this reaction at 269.0 K is Assume that AHⓇ and AS are independent of temperature. Submit Answer Retry Entire Group 8 more group attempts remaining For the reaction N2(g) + 3H2(g) +2NH3(g) AH° = -92.2 kJ and A Sº = -198.7 JK The equilibrium constant for this reaction at 308.0 K is Assume that AHⓇ and AS are independent...