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
find the enthalpy change H for this reaction: CH4(g) + Cl2--> CCl4(g)+HCl Using the following Equations:...
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
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
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
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
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
The reaction CH4 (8) + CCl4 (g) = 2 CH2Cl2 (B) has an enthalpy change AHI° - 18.8 kJ. You allow the equation to proceed to equilibrium at 25 °C, then raise the temperature to 50 °C. How will the equilibrium concentrations be affected by this temperature change? Concentrations of CH4 and CCl4 will increase. Concentration of CH2Cl2 will increase. Concentrations of CCl4 and CH2Cl2 will increase The concentrations will remain the same.
1. How much heat is required at constant pressure to melt 1 mole of ice at -25 C to steam at 125° C? boiling point 100c melting point 0.000'C specific heat capacities are gas(steam) 2.08, liquid 4.184 solid (ice) 2.11. All in units of JigC AH(100°C) 40.7 kJ/mol AHu (0.000°C)-6.01 kJ/mol 2. Calculate AHrxn for the reaction: CH4(g)4 Cl2(g) -CC4(g) 4 HCl (g) + Use the following reactions and given AH's: CH4(g) AH =-74.6 kJ 2 H2(g) C(s) C(s)2 Cl2(g)...
Consider the following chemical reaction: CH4 (g) + Cl2(g) + CCl4 (1) + CCl4 (I) + HCl (g) Identify the type of chemical reaction that this is classified as: oxidation-reduction (redox) O precipitation + acid-base precipitation + redox precipitation acid-base
Calculate AH® for the following: rxn CH4(8) + Cl2(g) → CCl4(!) + HCl(g) [unbalanced] -139 kJ/mol AH (CH4®= -74.87 kJ/mol a CCl4@)) = -96.0 kJ/mol AHCC140] =-139 kJ/mol AH [HCI@)) =-92.31 kJ/mol AH [HCl(aq)] =-167.46 kJ/mol Ahº [C1()] = 121.0 kJ/mol
Hi, can someone please explain in steps how they got the
answer?
Calculate Δ Hrm for the following reaction CH4(g) + 4C12 (g)CCL4 (g) +4HCl(g) given these reactions and their ΔΗ values: C(s) C(s) H2(g) + + + 2H2(g) 2C12(g) Cl2 (g) CH4 (g), CC14 (g), 2HCl(g), ΔΗ--74.6 kJ ΔΗ--95.7 kJ ΔΗ--184.6 kJ Express the enthalpy in kiloioules to one decimal place