Question

In: Chemistry

Given the following thermochemical equations: X2+3Y2--> 2XY3 H= -320 kj X2+2Z2 -- > 2Xz2 H2= -110...

Given the following thermochemical equations: X2+3Y2--> 2XY3 H= -320 kj X2+2Z2 -- > 2Xz2 H2= -110 kj 2Y2+z2 ---> 2Y2Z H3= -270 kj Calcuate the change in enthalpy for: 4XY3+7Z2--> 6Y2Z+4XZ2 H=?

Solutions

Expert Solution

X2+3Y2--> 2XY3 H= -320 kj --------------->1

X2+2Z2 -- > 2Xz2    H2= -110 kj ---------------->2

2Y2+z2 ---> 2Y2Z    H3= -270 kj ------------------>3

2 is multifly with 2

3 is multifly with 3

2X2+4Z2 -- > 4Xz2    H2= -220 kj

6Y2+3z2 ---> 6Y2Z    H3= -810 kj

---------------------------------------------------

2X2 +6Y2 + 7Z2 ------> 6Y2Z+4XZ2    H4 = -1030KJ

2X2+6Y2--> 4XY3                                 H1= -1280 kj

(-)    (-)         (-)                                             (+)

--------------------------------------------------------------------

4XY3+7Z2--> 6Y2Z+4XZ2                    H5   = 250KJ


Related Solutions

Given the following thermochemical data: ∆H°f (kJ) I. P4(s) + 6 Cl2(g) ⟶ 4 PCl3(g) –1225.6...
Given the following thermochemical data: ∆H°f (kJ) I. P4(s) + 6 Cl2(g) ⟶ 4 PCl3(g) –1225.6 II. P4(s) + 5 O2(g) ⟶ P4O10(s) –2967.3 III. PCl3(g) + Cl2(g) ⟶ PCl5(g) –84.2 IV. PCl3(g) + ½ O2(g) ⟶ POCl3(g) –285.7 Calculate the value of ∆H° for the following reaction: P4O10(s) + 6 PCl5(g) ⟶ 10 POCl3(g) Why/how is the answer 610.1 kJ?
Given the following thermochemical equations, 2Cu(s) + S(s) right-arrow Cu2S(s) ΔH°= –79.5 kJ S(s) + O2(g)...
Given the following thermochemical equations, 2Cu(s) + S(s) right-arrow Cu2S(s) ΔH°= –79.5 kJ S(s) + O2(g) right-arrow SO2(g) ΔH°= –297 kJ Cu2S(s) + 2O2(g) right-arrow 2CuO(s) + SO2(g) ΔH° = –527.5 kJ calculate the standard enthalpy of formation (in kJ mole–1) of CuO(s).    Multiplied by 1/2 Finally, using the thermodynamic values given and knowing how to add all the equations together to get the desire equation, calculate the value of ΔHf° for the final formation reaction.
1. Consider the following thermochemical equation: 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g) ∆H° = –878.2 kJ
  1. Consider the following thermochemical equation: 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g) ∆H° = –878.2 kJ (a) How much heat is released when 3.0 mol ZnS(s) reacts in excess oxygen? (b) How much heat is released when 2.3 × 10-2 mol ZnS(s) reacts in excess oxygen? (c) What is the enthalpy change when 223.9 g ZnS(s) reacts in excess oxygen? (d) What is the enthalpy change when 0.96 g ZnO(s) is produced? 2. Slaked lime (Ca(OH)2(s)) is produced...
Given the following equations: A (g) → B (g)   ΔH = –50 kJ B (g) →...
Given the following equations: A (g) → B (g)   ΔH = –50 kJ B (g) → C (g)   ΔH = –100 kJ Calculate the enthalpy changes for the following. Enter your answer in kJ but don't include units. For example, if the answer is 35 kJ, you would enter "35" without the quotes. 2 A (g) → 2 B (g) has an enthalpy change of: , C (g) → B (g) has an enthalpy change of: , A (g) →...
Calculate delta H for the reaction H(g) + Br(g) = HBr(g), given the following information: H2(g)...
Calculate delta H for the reaction H(g) + Br(g) = HBr(g), given the following information: H2(g) + Br2(g) = 2HBr(g) delta H = -72 kJ H2(g) = 2H(g) delta H = +436 kJ Br2(g)= 2Br(g) delta H = +224 kJ
Calculate ?H (298 K) per gram of fuel units of kJ*g^-1 (exclude oxygen) a.) H2(g) +...
Calculate ?H (298 K) per gram of fuel units of kJ*g^-1 (exclude oxygen) a.) H2(g) + O2(g) = H2O(g) b.) CH4(g) + 2O2(g) = CO2(g) + 2H2O(g) c.) CH3OH(l) +3/2 O2(g) = CO2(g) + 2H2O(g) d.) C6H14(g) + 9 1/2 O2(g) = 6CO2(g) + 7H2O(g)
Consider the reaction Fe(s) + 2HCl(aq)FeCl2(s) + H2(g) for which H° = -7.400 kJ and S°...
Consider the reaction Fe(s) + 2HCl(aq)FeCl2(s) + H2(g) for which H° = -7.400 kJ and S° = 107.9 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.097 moles of Fe(s) react under standard conditions at 298.15 K. Suniverse =  J/K (2) Is this reaction reactant or product favored under standard conditions? _________reactantproduct (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is...
2 reacts with the halogens (X2) according to the following reaction: H2(g)+X2(g)?2HX(g) where X2 can be...
2 reacts with the halogens (X2) according to the following reaction: H2(g)+X2(g)?2HX(g) where X2 can be Cl2, Br2, or I2. Reactant/Product ?H?f(kJ/mol) ?S?f(J/mol?K) H2(g) 0 130.7 Cl2(g) 0 223.1 HCl(g) -92.3 186.9 Br2(g) 30.9 245.5 HBr(g) -36.3 198.7 I2(g) 62.42 260.69 HI(g) 26.5 206.6 Assuming deltaGo for the reaction between hydrogen and Cl2 is -190.46 kJ calculate Kp for the reaction between hydrogen and Cl2.
Given the following thermochemistry equations: NH4NO2(s) -------> N2 (g) + 2H2O(l); ΔH = -300.12 kJ/mol NH3...
Given the following thermochemistry equations: NH4NO2(s) -------> N2 (g) + 2H2O(l); ΔH = -300.12 kJ/mol NH3 (aq) + HNO2 (ac) ------> NH4O2 (aq); ΔH = -38.04 kJ/mol NH402(s) -------> NH402(aq); ΔH = 19.85 kJ/mol H2 (g) + 1/2 O2 (g) ------> H2O (l) ΔH = -284.24 kJ/mol 1/2 N2 (g) + 3/2 H2 (g) ------> NH3(ac) ΔH = -85.27 kJ/mol Calculate the ΔH for the formation of HNO2
Given the following thermochemistry equations: C(s) + 1/2 O2(g) -------> CO (g); ΔH = -110.4 kJ/mol...
Given the following thermochemistry equations: C(s) + 1/2 O2(g) -------> CO (g); ΔH = -110.4 kJ/mol H2 (g) + 1/2 O2 (g) ------> H2O (l); ΔH = -285.5 kJ/mol CO(g) + 1/2 O2(g) -------> CO2 (g); ΔH = -283.0 kJ/mol HCOOH (l) + 1/2 O2 (g) ------> H2O (l) + CO2(g); Δ = -259.6 kJ/mol a) Calculate the ΔH for the formation of HCOOH. b) Calculate the ΔH of the reaction if 0.76 mL of HCOOH is obtained. c) If...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT