B5h9(l) is a colorless liquid that will explode when exposed to oxygen. how much heat is released when 0.211 mol of b5h9 reacts with excess oxygen where the products are b2h3(s) and h2o(l). the standard enthalpy of formation of b5h9(l) is 73.2 kj/mol, the standard enthalpy of formation of b2h3(s) is -1272 kj/mol and that of h2o(l) is -285.4 kj/mol. express your answer in kj.

958 kJ  heat is released when 0.211 mol of reacts with excess oxygen.

Explanation:

The balanced chemical reaction is,

The expression for enthalpy change is,

where,

n = number of moles

(as heat of formation of substances in their standard state is zero

Now put all the given values in this expression, we get

Thus 2 moles of release heat = 9075.9 kJ

0.211 moles of release heat =

hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey

b..

is the correct one

explanation:

covalent bonds form as valence electrons are shared between two atoms. lewis structures and structural formulas are common ways of showing the covalent bonding in organic molecules. formal charge describes the changes in the number of valence electrons as an atom becomes bonded into a molecule.