Given the thermochemical equation: 2HI (g) rightarrow H_2 (g) + I_2 (s) Delta H degree =...

Question

Question

Answer 1

Answer #1

udi 26-48 KJ nio This i the hezt

Answer 2

Similar Homework Help Questions

Given reactions 1 and 2 below, calculate delta H degree_Rxn and delta U degree_Rxn for reaction...

Given reactions 1 and 2 below, calculate delta H degree_Rxn and delta U degree_Rxn for reaction 3. Rxn 1 H_2(g) + I_2(s) rightarrow 2 HI(g) delta H degree_Rxn = +52.96 kJ/mol Rxn 2 2H_2(g) + O_2(g) rightarrow 2 H_2 O(g) delta H degree_Rxn = -483.64 kJ/mol Rxn 3 4 HI(g) + O_2(g) rightarrow 2 I_2(s) + 2 H_2O(g) delta H degree_Rxn = ? delta U degree_Rxn = ?
H_2(g) + I_2(g) rightarrow 2HI(g) Initial concentration [H_2] = 2: [I_2] = 2: [HI] = 3...

H_2(g) + I_2(g) rightarrow 2HI(g) Initial concentration [H_2] = 2: [I_2] = 2: [HI] = 3 Kc = 55.17 Is the system at equilibrium? If not, which direction should equilibrium shift? What is equilibrium concentration of each species? 55.17 == [3 + 2X]^2/[2 - X]^2 X = ? Relative strength of acid and base: The stronger the acid, the weaker its conjugate base The stronger the base, the weaker its conjugate acid
Given the following thermochemical equation: 2 Al + Fe_2O_2 rightarrow Al_2O_2 + 2Fe delat H =...

Given the following thermochemical equation: 2 Al + Fe_2O_2 rightarrow Al_2O_2 + 2Fe delat H = - 852 kJ What is Delta H when 0.100 mal of Al_2O_3 react with 0.250 mol of Fe? _____ kJ Using the data from Appendix G of the textbook, calculate Delta H for the combustion of 1.00 mole of C_2H_5OH(l). Note that (g) or (l) after the chemical formula denotes whether the compound is a gas or liquid. Some compounds have entries for both....

The equation for the formation of hydrogen iodide from H_2 and l_2 is: H_2(g) + I_2(g)...

The equation for the formation of hydrogen iodide from H_2 and l_2 is: H_2(g) + I_2(g) 2 HI(g) The value of K_p for the reaction is 69.0 at 790.0 degree C. What is the equilibrium partial pressure of HI in sealed reaction vessel at 790.0 degree C if the initial partial pressures of H_2 and l_2 are both 0.1800 atm an initially there is no HI present?
Hydrogen iodide undergoes decomposition according to the equation 2HI(g) reversiblearrow H_2(g) + I_2(g) The equilibrium constant...

Hydrogen iodide undergoes decomposition according to the equation 2HI(g) reversiblearrow H_2(g) + I_2(g) The equilibrium constant K_P at 500 K for this equilibrium is 0.060. Suppose 0.316 mol of HI is placed in a 8.00-L container at 500 K. What is the equilibrium partial pressure of I_2(g)? (R = 0.0821 L middot atm/(K middot mol)) 0.040 atm 0.020 atm 0.062 atm 0.0078 atm 0.32 atm
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ...

For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ and Delta S degree = -198.7 J/K at 345 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 345 K. The standard enthalpy change for the reaction of 2.30 moles of N_2(g) at this temperature would be kJ. For the reaction 2 H_2O_2(l) rightarrow 2 H_2O(l) + O_2(g) Delta G degree = -236.9 kJ and Delta H degree =...

Given the reaction 2HI(g) H_2(g) + I_2(g) K_eq = 1.0 times 10^1 A sample mixture of...

Given the reaction 2HI(g) H_2(g) + I_2(g) K_eq = 1.0 times 10^1 A sample mixture of H1, H2, and I_2 at equilibrium, was found to have [H_2] = 3.6 times 10^-4 M and |HI] = 7.0 times 10^-2 M. Calculate the molar concentration of I_2 in the equilibrium mixture. [I_2] = M
Determine Delta S degree_rxn for H_2 (g) + I_2 (g) 2 HI (g) given the following...

Determine Delta S degree_rxn for H_2 (g) + I_2 (g) 2 HI (g) given the following information: a. -41.10 J/K b. 398.75 J/K c. -165.29 J/K d. + 41.10 J/K e. + 165.29 J/K
Use Hess's Law to determine Delta H for the reaction 2 Al(s) + 3 Cl_2(g) rightarrow...

Use Hess's Law to determine Delta H for the reaction 2 Al(s) + 3 Cl_2(g) rightarrow 2 AlCl_3(s) given: 2 Al(s) + 6 HCl(aq) rightarrow 2 AlCl_3(aq) + 3 H_2(g) Delta H = -1049 kJ HCl(g) rightarrow HCl(aq) Delta H = -74.8 kJ H_2(g) + Cl_2(g) rightarrow 2 HCl(g) Delta H = -185 kJ AlCl_3(s) rightarrow AlCl_3(aq) Delta H = -323 kJ

Please Answer and explain. thanks Consider the following thermochemical equations. Cu_2O(s) + 1/2 O_2(g) rightarrow 2CuO(s)...

Please Answer and explain. thanks Consider the following thermochemical equations. Cu_2O(s) + 1/2 O_2(g) rightarrow 2CuO(s) Delta H degree = - 144 kJ Cu_2O(s) rightarrow Cu(s) +CuO(s) Delta H degree = +11 kJ Calculate the standard enthalpy of formation of CuO(s). a) - 166 kJ b) - 299 kJ c) +299 kJ d) +155 kJ e) -155 kJ