From the following enthalpy changes in equations (1) and (2), find the ΔH° for equation (3).
(1) 2P(s) + 3Cl2(g) →2PCl3 (l) ΔH° = -640 kJ
(2) 2P(s) + 5Cl2 (g) → 2PCl5 (s) ΔH° = -886 kJ
(3) PCl3(l) + Cl2 (g) → 2PCl5 (s)
From the following enthalpy changes in equations (1) and (2), find the ΔH° for equation (3)....
From the following enthalpy changes in equations (1) and (2), calculate the heat of reaction for equation (3). (1) C(s) + 1/2 O2 (g) → CO (g) ΔH°= -110.5 kJ (2) CO (g) + 1/2 O2 (g) → CO2 (g) ΔH°= - 283.0 kJ (3) C(s) + O2(g) →CO2(g)
Given the standard enthalpy changes for the following two reactions: (1) Sn(s) + Cl2(g) ------> SnCl2(s) . ΔH° = -325.1 kJ (2) Sn(s) + 2Cl2(g)-----> SnCl4(l) . ΔH° = -511.3 kJ what is the standard enthalpy change for the reaction: (3) SnCl2(s) + Cl2(g) ------> SnCl4(l) . ΔH° = ? _____kJ
Given the standard enthalpy changes for the following two reactions: (1) 4C(s) + 5H2(g)-------> C4H10(g)...... ΔH° = -125.6 kJ (2) C2H2(g) ----> 2C(s) + H2(g)......ΔH° = -226.7 kJ what is the standard enthalpy change for the reaction: (3) 2C2H2(g) + 3H2(g)--------->C4H10(g)......ΔH° = ? kj
Given the thermochemical equations: A(g) ⟶B(g)ΔH=90kJmolB(g) ⟶C(g)ΔH=−140kJmolA(g) ⟶B(g)ΔH=90kJmolB(g) ⟶C(g)ΔH=−140kJmol Find the enthalpy changes for three given reactions. 3A(g)⟶ 3B(g)3A(g)⟶ 3B(g) ΔH=ΔH= kJ/mol B(g)⟶A(g)B(g)⟶A(g) ΔH=ΔH= kJ/mol A(g)⟶C(g)A(g)⟶C(g) ΔH=ΔH= kJ/mol
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g) → CHCl3(l) + 3 HCl(g) ΔH°rxn = ? ΔH°f (kJ/mol): -75 -134 -92 A. +662 kJ B. +117 kJ C. -151 kJ D. -335 kJ The equation that corresponds to the enthalpy of formation for NH3(g) is A. N(g) + 3H(g) → NH3(g) B. N(g) + 3/2 H2(g) → NH3(g) C. 1/2 N2(g) + 3H(g) → NH3(g) D. 1/2 N2(g) + 3/2 H2(g) →...
Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the thermochemical equations below: CaCO3(s) → CaO(s) + CO2(g) Report your answer to three significant figures in scientific notation. Equations: ΔH°rxn (kJ) Ca(s) + CO2(g) + 1/2O2(g) → CaCO3(s) -812.5 2Ca(s) + O2(g) → 2CaO(s) -1270.3
Calculate the standard enthalpy change, ΔH°rxn, in kJ for the following chemical equation, using only the thermochemical equations below: 2COBr2(g) + 4NO(g) → 4NOBr(g) + 2CO(g) Report your answer to three significant figures in scientific notation. Equations: ΔH°rxn (kJ) CO(g) + Br2(g) → COBr2(g) -3 1/2N2(g) + 1/2O2(g) → NO(g) 90.4 1/2N2(g) + 1/2O2(g) + 1/2Br2(g) → NOBr(g) 82.1
A chemist measures the enthalpy change ΔH during the following reaction: 2Na (s) + Cl2 (g) → 2NaCl (s) =ΔH−822.kJ Use this information to complete the table below. Round each of your answers to the nearest /kJmol . A chemist measures the enthalpy change AH during the following reaction: 2Na(s) + Cl2(g)→2 NaCl(s) NH=-822. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol reaction △H kJ NaCl(s) → Na(s) + Cl2(g)...
Calculate the value of ΔH° for the following reaction: P4O10(s) + 6PCl5(g) ---> 10Cl3PO(g) P4(s) + 6Cl2(g) ---> 4PCl3(g) ΔH° = -1225.6 kJ P4(s) + 5O2(g) ---> P4O10(s) ΔH° = -2967.3 kJ PCl3(g) + Cl2(g) ---> PCl5(g) ΔH° = -84.2 kJ PCl3(g) + (1/2)O2(g) ---> Cl3PO(g) ΔH° = -285.7 k please explain well i do not understand these kind of problems
Using the enthalpy changes given below, calculate the enthalpy change for the following equation: N2(g) + 2O2(g) -----> 2 NO2 using the following equations: 2NO -----> N2 + O2 delta H + -180.0 kJ NO2 -----> NO + 1/2 O2 delta H= 112.0 kJ