Chlorine trifluoride has 10 electrons around the central chlorine atom. This means there are five electron pairs arranged in a trigonal bipyramidal shape with a 175° F − C l − F bond angle.

Solution for Calculate ΔH (in kJ/mol) for the reaction shown below: ClF(g)+F2(g)→ClF3(g) Use the following reactions and enthalpies:…

Q: Calculate ∆Gº for the reaction, 2CH4(g)+3O2(g)→2CO(g)+4H2O(g), given ∆Gºf for CH4(g)=-50.8 kJ/mol,…

Answer the questions about chlorine trifluoride, ClF3, a molecule with an expanded octet. There are ----- valence electrons, ----- REDs, the shape is -----, and the bond angles are -----. Since the bonds are polar covalent, and because it is not symmetrical, ClF3 is a Blank 5. ----- molecule.

The molecular geometry of chlorine trifluoride is T-shaped. The central atom chlorine is attached to three fluorine atoms.

The Lewis dot structure of {eq}{\rm{Cl}}{{\rm{F}}_{\rm{3}}} {/eq} is as follows, it helps to determine the bonding and non-bonding electrons.

Identify the limiting reactant and determine the theoretical yield of ClF3 in grams. Chlorine gas reacts with fluorine gas to form chlorine trifluoride: Cl2(g) + 3 F2(g) --------> 2 ClF3(g) A 2.00-L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 729 mmHg.

Chlorine trifluoride has 5 regions of electron density around the central chlorine atom (3 bonds and 2 lone pairs).

Oxidation of gaseous ClF by F2 yields liquid ClF3, an important fluorinating agent. Use the following thermochemical equations to calculate ΔH o/rxn (1) 2 ClF(g) + O2(g) → Cl2O(g) + OF2(g) ΔHo = 167.5 kJ (2) 2 F2(g) + O2(g) → 2 OF2(g) ΔHo = −43.5 kJ (3) 2 ClF3(l) + 2 O2(g) → Cl2O(g) + 3 OF2(g) ΔHo = 394.1 kJ for the production of ClF3:

Answer to: Calculate Delta H for the reaction ClF(g) + F2(g) to ClF3(g) given the following data: By signing up, you'll get thousands of...