Hi, can someone please explain in steps how they got the answer?
Hi, can someone please explain in steps how they got the answer? Calculate Δ Hrm for...
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
Calculate ΔHrxn for the following reaction: CH4 (g) + 4Cl2(g) → CCl4(g) + 4HCl(g) Using the following reactions: C(s) + 2H2(g) → CH4(g) ∆H = -74.6 kJ C(s) + 2Cl2(g) → CCl4(g) ∆H = -95.7 kJ H2(g) + Cl2(g) → 2HCl(g) ∆H = -184.6 kJ
Part A Calculate A H xn for the following reaction: CHA(g) + 4Cl2(g) → CCl4(g) + 4HCl(g) given these reactions and their AH values: | C(s) + C(s) + H2(g) + Express the enthalpy in kilojoules to one decimal place. 2H2 (g) 2Cl2(g) Cl2(g) + CH4(g), + CCL(g), + 2HCl(g), AH = -74.6 kJ AH = -95.7 kJ AH = -184.6 kJ %AM * o aj ? AH,,n= Submit Request Answer
A) A 9.55−g sample of a piece of diamond at 185 oC was placed in a container containing water at 87.0 oC. If the final temperature of the mixture is 91.5 oC, what is the mass of the mixture?The specific heat capacity of diamond and water are 0.52 J g−1 oC−1 and 4.184 J g−1 oC−1 respectively. Question options: A) 50.1 g B) 125 g C) 24.7 g D) 34.2 g B)Calculate the enthalpy for the reaction:CH4 + 4Cl2 →...
Express the enthalpy in kJ
Acceptable units Acceptable units X C Get Homework Help With + X um.ecollege.com/course.html?courseld-15350726&OpenVellumHMAC=c1df59a153217665a9f9526c8fe3a8b9# 10001 Course Home <Chapter 6 Exercise 6.82 - Enhanced - with Feedback < 24 of 34 Calculate A H for the following reaction: CH (g)+ 4C2(g) CC4(g) + 4HCI (g) given these reactions and their AH values: C(s) C(s) + 2C12(g) 2H2(g) CH4(g), CCL(g), AH=-74.6 kJ AH-95.7 kJ H2(g) + Cl2(g) 2HCI(g), AH=-184.6 kJ Express the enthalpy in kilojoules to one decimal...
Calculate ΔHrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) Use the following reactions and given ΔH′s. C(s)+2H2(g)→CH4(g) ΔH=−74.6kJ C(s)+2Cl2(g)→CCl4(g) ΔH=−95.7kJ H2(g)+Cl2(g)→2HCl(g) ΔH=−184.6kJ
82. Calculate A Hex for the reaction. CH4(8) + 4 C12(8) — CCl4(8) + 4 HCl(8) Use the following reactions and given AH's: C(s) + 2 H2(8) — CH4(8) AH = - 74.6 kJ. C(s) + 2 C12(8) - CĊ14(8) AH = -95.7 kJ X2 H2(8) + Cl2(8) —> 2HCl(8) AH = -92.3 kJ_x2 x 2 X2
A) Calculate ?Hrxn for the following reaction: CaO(s)+CO2(g)?CaCO3(s) Use the following reactions and given ?H values: Ca(s)+CO2(g)+12O2(g)?CaCO3(s), ?H= -812.8 kJ 2Ca(s)+O2(g)?2CaO(s), ?H= -1269.8 kJ B) Calculate ? Hrxn for the following reaction: CH4(g)+4Cl2(g)?CCl4(g)+4HCl(g) given these reactions and their ?H values: C(s)+2H2(g) ---> CH4(g), ? H=-74.6kJ C(s)+2Cl2(g) ---> CCl4(g), ? H=-95.7kL H2(g)+Cl2----> 2HCl(g), ? H=-184.6kJ
please explain each step in clear writing.
Chloroform (CHCI3) is formed from methane and chlorine in the following reaction: CH4 (g)3C12 (g)3HC1(g)+CHCI3 (g) Calculate A, Ho, the enthalpy change for this reaction, using the standard molar enthalpy change of formation of CHCI3 (g), AfH° = -103.1 kJ mol1, and the standard enthalpy changes for the following reactions: CH4 (g)202 (g)2H2O (e) CO2 (g) AH°=-890.4 kJ mol-1 2HC1(g) H2 (g)Cl2 (g) A,.H +184.6 kJ mol1 C(graphite)O2 (g)CO2 (g) A H°=-393.5 kJ...
I know the right answer is
-233.8 but can someone please show the steps to get there?
Thanks!
Question4 10 10 pts The value of [delta)Ho for: 2 H2S (g) +SO2 (g) 3 S (s) + 2 H20 () is: H2 (g) 1/2 02 (g)H2O) [deltajH°-285.8 kJ H2 (g)S (s) > H2S (g) [delta)H°-20.5 kJ S (s) +O2 (8) >SO2 (g) (deltajHo --296.8 kJ +603.1 k 454.9 k +233.8 k 233.8 kJ -603.1 kJ