Using Hess's Law, calculate ΔH°R Equation: B2H6 (g) + 6 Cl2 (g) --> 2BCl3 (g) +...
Using Hess's Law, calculate ΔH°R
Equation: B2H6 (g) + 6 Cl2 (g) --> 2BCl3 (g) + 6 HCl (g)
Given these 3 equations: (please show all work)
BCl3 (g) + 3H2O (l) --> H3BO3 (g) + 3HCl (g) (ΔH°R = -112.5 KJ/mol BCl3)
B2H6 (g) + 6H2O (l) --> 2H3BO3 (g) + 6H2 (g) (ΔH°R = -493.4 KJ/mol B2H6)
H2 (g) + Cl2 (g) --> 2HCl (g) (ΔH°R = -184.6 KJ/mol H2)
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Using Hess's Law, calculate ΔH°R
Equation: B2H6 (g) + 6 Cl2 (g)
--> 2BCl3 (g) +...
calculate Δh0 ulate AHo (in kJ/mol) for the reaction: B2H6(g)+6 Cl2(g)2 BCls(g)+6 HCl(g) ven the following data: BCI...
calculate Δh0
ulate AHo (in kJ/mol) for the reaction: B2H6(g)+6 Cl2(g)2 BCls(g)+6 HCl(g) ven the following data: BCI5(g)+3 H2O(I) H3BO:(g)+3 HCl(g) AH° = -112.5 kJ/mol B2H&(g) + 6 H2O(1) 2 H3BO:(g) + 6 H2(g)AH°= -493.4 kJ/mol AHOC(HCI, g) -92.3 kJ/mol
I found the Delta H rxn to be -1376 KJ . I'm confused on the steps...
I found the Delta H rxn to be -1376 KJ .
I'm confused on the steps to find my limiting reactant and grams of
BCl3.
Question How many grams of BClz will be produced if 55.36 g of B, Ho reacted with an unknown mass of Cl, in which the reaction released 688.0 KJ of heat? Which is the limiting reactant? BH6 + 6Cl2 → 2BCl2 + 6HCI AHrxn = ? Given: 1/2H2 + 1/2012 B H6 + 6H2O BCl3...
Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g) ΔH...
Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g) ΔH =-184.6 kJ/mol If 5.0 moles of H2 reacts with 5.0 moles of C12 to form HC1 at 1.0 atm, what is Δ U for this reaction? Assume the reaction goes to completion and Δ V= 0 L (The conversion factor is 1 L·atm = 101.3 J.) kJ
Using Hess's Law to Calculate a Standard Enthalpy of Formation On the Solution Calorimetry Lab Report...
Using Hess's Law to Calculate a Standard Enthalpy of Formation On the Solution Calorimetry Lab Report Form, vou will be asked to calculate a standard enthalpy of formation for magnesium oxide based on your experimental results. Below is an example of how to do this type of calculation. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using the following thermochemical equations: 4 B(s) + 3 O2(g)-> 2 B2O3(s) 2 H2(g) + O2(g) > 2 H20(0) B2H6(8) +3 O2(g)...
a) Use Hess's law to calculate the enthalpy change for the reaction: 3C(s) + 4H2(g) +...
a) Use Hess's law to calculate the enthalpy change for the reaction: 3C(s) + 4H2(g) + ½O2(g) → C3H8O(l) Given the following thermochemical equations: 2C3H8O(l) + 9O2(g) → 6CO2(g) + 8H2O(l) ΔH = -4042.6 kJ/mol C(s) + O2(g) → CO2(g) ΔH = -393.51 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔH = -285.83 kJ/mol (in kJ/mol) A: -267.7 B: -302.6 C: -341.9 D: -386.3 E: -436.5 F: -493.3 G: -557.4 H: -629.9 b) Define if the following statement is an endothermic process or exothermic...
solution pls 13. Find the Hºrn for the reaction 2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g)....
solution pls
13. Find the Hºrn for the reaction 2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g). AH°F (NH3) = -46 kJ/mol, AH°F (HCI) = -92.3 kJ/mol Answer: -461.8 kJ 14. Use the standard enthalpies of formation to calculate AH°rxn: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) AH°F (Fe2O3) = -826 kJ/mol, AH°F (CO) = -110.5 kJ/mol, AH°F (CO2) = -393.5 kJ/mol Answer: -23 kJ 15. Given the following reaction: B2H6(g) + 6H2O(l) → 2H3BO3(g) + 6H2(g) AH°= -493.4 kJ AH°t...
Use the ΔH°f values provided to determine ΔH°rxn for the following reaction CH4(g) + 3 Cl2(g)...
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) →...
Hess's Law Given the following data: P(s) + 3/2H2(g) → PH3(g) ΔH°= +5.0 kJ PH3(g) +...
Hess's Law Given the following data: P(s) + 3/2H2(g) → PH3(g) ΔH°= +5.0 kJ PH3(g) + 2O2(g) → H3PO4(l) ΔH°= -1272.0 kJ 2P(s) + 5/2O2(g) → P2O5(s) ΔH°= -1492.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°= -286.0 kJ calculate ΔH° for the reaction: H3PO4(l) → 1/2P2O5(s) + 3/2H2O(l) ΔH°=?? also please explain how you found the answer
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g)...
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g) Using the following equations: Si(s) + O2(g) → SiO2(s) Si(s) + 2F2(g) → SiF4(g) H2(g) + F2(g) → 2HF(g) H2(g) + 4202(g) → H2O(g) AH = -910.9 kJ/mol rxn AH = -1651 kJ/mol rxn AH = -542 kJ/mol rxn AH = -241.8 kJ/mol rxn
The value of ΔH° for the reaction below is-186 k. H2 (g) + Cl2 (g)-> 2HCl...
The value of ΔH° for the reaction below is-186 k. H2 (g) + Cl2 (g)-> 2HCl (g) The value of AHfo for HCI (g) is .k/ kJ/mol. O -3.72 x 102 ○-1.27 × 102 ○-93.0 0-186 ○ +186
calculate Δh0
ulate AHo (in kJ/mol) for the reaction: B2H6(g)+6 Cl2(g)2 BCls(g)+6 HCl(g) ven the following data: BCI5(g)+3 H2O(I) H3BO:(g)+3 HCl(g) AH° = -112.5 kJ/mol B2H&(g) + 6 H2O(1) 2 H3BO:(g) + 6 H2(g)AH°= -493.4 kJ/mol AHOC(HCI, g) -92.3 kJ/mol
I found the Delta H rxn to be -1376 KJ .
I'm confused on the steps to find my limiting reactant and grams of
BCl3.
Question How many grams of BClz will be produced if 55.36 g of B, Ho reacted with an unknown mass of Cl, in which the reaction released 688.0 KJ of heat? Which is the limiting reactant? BH6 + 6Cl2 → 2BCl2 + 6HCI AHrxn = ? Given: 1/2H2 + 1/2012 B H6 + 6H2O BCl3...
Enter your answer in the provided box. Consider the reaction H2(g) + Cl2(g) → 2HCl(g) ΔH =-184.6 kJ/mol If 5.0 moles of H2 reacts with 5.0 moles of C12 to form HC1 at 1.0 atm, what is Δ U for this reaction? Assume the reaction goes to completion and Δ V= 0 L (The conversion factor is 1 L·atm = 101.3 J.) kJ
Using Hess's Law to Calculate a Standard Enthalpy of Formation On the Solution Calorimetry Lab Report Form, vou will be asked to calculate a standard enthalpy of formation for magnesium oxide based on your experimental results. Below is an example of how to do this type of calculation. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using the following thermochemical equations: 4 B(s) + 3 O2(g)-> 2 B2O3(s) 2 H2(g) + O2(g) > 2 H20(0) B2H6(8) +3 O2(g)...
solution pls
13. Find the Hºrn for the reaction 2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g). AH°F (NH3) = -46 kJ/mol, AH°F (HCI) = -92.3 kJ/mol Answer: -461.8 kJ 14. Use the standard enthalpies of formation to calculate AH°rxn: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) AH°F (Fe2O3) = -826 kJ/mol, AH°F (CO) = -110.5 kJ/mol, AH°F (CO2) = -393.5 kJ/mol Answer: -23 kJ 15. Given the following reaction: B2H6(g) + 6H2O(l) → 2H3BO3(g) + 6H2(g) AH°= -493.4 kJ AH°t...
Hess's Law Practice Find AH° for the following equation: SiO2(s) + 4HF(g) → SiF4(g) + 2H2O(g) Using the following equations: Si(s) + O2(g) → SiO2(s) Si(s) + 2F2(g) → SiF4(g) H2(g) + F2(g) → 2HF(g) H2(g) + 4202(g) → H2O(g) AH = -910.9 kJ/mol rxn AH = -1651 kJ/mol rxn AH = -542 kJ/mol rxn AH = -241.8 kJ/mol rxn
The value of ΔH° for the reaction below is-186 k. H2 (g) + Cl2 (g)-> 2HCl (g) The value of AHfo for HCI (g) is .k/ kJ/mol. O -3.72 x 102 ○-1.27 × 102 ○-93.0 0-186 ○ +186
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