The chemical reaction that the situation demonstrates would be a double replacement reaction.
In double replacement reactions, the two reactants participating in the reaction are similarly built in terms of their chemical bonds and they exchange ions to form the products of the reaction. Two products are also formed from the two reactants.
It is as opposed to single replacement reactions in which the two reactants are not similar bond-wise. One of the reactants replaces or displaces one of the ions in another reactant.
In this case, the situation can be represented as follows:
Amanda-Janice + Deja-Eden ----> Amanda-Eden + Deja-Janice
Thus, it is a form of double replacement reaction.
More on double replacement reactions can be found here: brainly.com/question/392491?referrer=searchResults
Molecules in food contain chemical energy that cells use to produce ATP = adenosine triphosphate.
Answer:
B) ) –1615.1 kJ mol^–1
Explanation:
since
SiO2(s) + 4 HF(aq) → SiF4(g) + 2 H2O(l) ∆Hºrxn = 4.6 kJ mol–1
the enhalpy of reaction will be
∆Hºrxn = ∑νp*∆Hºfp - ∑νr*∆Hºfr
where ∆Hºrxn= enthalpy of reaction , ∆Hºfp= standard enthalpy of formation of products , ∆Hºfr = standard enthalpy of formation of reactants , νp=stoichiometric coffficient of products, νr=stoichiometric coffficient of reactants
therefore
∆Hºrxn = ∑νp*∆Hºfp - ∑νr*∆Hºfr
4.6 kJ/mol = [1*∆HºfX + 2*(–285.8 kJ/mol)] - [1*(–910.9kJ/mol) + 4*(–320.1 kJ/mol)]
4.6 kJ/mol =∆HºfX -571.6 kJ/mol + 2191.3 kJ/mol
∆HºfX = 4.6 kJ/mol + 571.6 kJ/mol - 2191.3 kJ/mol = -1615.1 kJ/mol
therefore ∆HºfX (unknown standard enthalpy of formation = standard enthalpy of formation of SiF4(g) ) = -1615.1 kJ/mol
