10. Calculate ∆Hrxn for the reaction: CH4(g) + 4Cl2 → CCl4(g) + 4HCl(g) Given that: C(s) + 2H2(g) → CH4(g) C(s) + 2Cl2(g) → CCl4(g) H2(g) + Cl2(g) → 2HCl(g) ∆H = -74.6kJ ∆H = -95.7kJ ∆H = -92.3kJ
10. Calculate ∆Hrxn for the reaction: CH4(g) + 4Cl2 → CCl4(g) + 4HCl(g) Given that: C(s)...
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) 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
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
Calculate ΔrH for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) Use the following reactions and given ΔrH's. C(s)+2H2(g)→CH4(g)ΔrH=−74.6kJmol−1C(s)+2Cl2(g)→CCl4(g)ΔrH=−95.7kJmol−1H2(g)+Cl2(g)→2HCl(g)ΔrH=−92.3kJmol−1
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
For the reaction CH4 + 4Cl2 CCl4 + 4HCl, how many grams of Cl2 are needed to make 55.2 g of CCl4?
a) consider the following reaction CH4 +4Cl2 = CCl4+ 4HCl what mass of CCl4 is formed by the reaction of 4.80g of methane with an excess of chlorine? and why b) Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the equation: 4NH3 + 5O2 = 4NO + 6H2O What mass of NO can be produced from 7.76 g of NH3? and why?
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 →...
The overall reaction to produce chloroform from methane is CH4(g) + 3Cl2(g) ---> CHCl3(l) + 3HCl(g). Use the following intermediate reactions to calculate the enthalpy of the reaction, Hrxn. 1/2 H2(g) + 1/2 Cl2(g) ---> HCl(g) Hrxn = -92.3 kj C(s) + 2H2(g) ----> CH4(g) Hrxn = -74.8 kj C(s) + 1/2 H2(g) + 3/2 Cl2(g) ----> CHCl3(l) Hrxn = -134.5 kj
find the enthalpy change H for this reaction: CH4(g) + Cl2--> CCl4(g)+HCl Using the following Equations: C(s)+H2(g)-->CH4 H= -74.6 kJ C(s) + Cl2(g)--> CCl4 H=-95.7 kJ H2(g)+Cl2(g)--> HCl H=-92.3 kJ