Answer:
191g of water.
Explanation:
For the reaction:
SiO₂(s) + 4HF(g) → SiF₄(g) + 2H₂O(l) ΔH°rxn = -184 kJ
Two moles of water are formed and the reaction produce 184 kJ of energy. To produce 975 kJ of energy:
975 kJ energy ×[tex]\frac{2molH_{2}O}{184 kJ}[/tex] = 10,6 moles of H₂O
Using molar mass of water (18,02 g/mol), mass of H₂O must form when 975 kJ of energy are produced is:
10,6 moles of H₂O×[tex]\frac{18,02g}{1molH_{2}O}[/tex] = 191 g of water
I hope it helps!
Taking into account the definition of enthalpy of a chemical reaction, 190.8 g of H₂O must form in order to produce 975 kJ of energy.
The enthalpy of a chemical reaction as the heat absorbed or released in a chemical reaction when it occurs at constant pressure. That is, the heat of reaction is the energy that is released or absorbed when chemicals are transformed into a chemical reaction.
The enthalpy is an extensive property, that is, it depends on the amount of matter present.
In this case, the balanced reaction is:
SiO₂ (g) + 4 HF (g) → SiF₄ (g) + 2 H₂O (g)
and the enthalpy reaction ∆H° has a value of -184 kJ/mol.
This equation indicates that when 1 mole of SiO₂ reacts with 4 moles of HF to produce 1 moles of SiF₄ and 2 moles of H₂O, 184 kJ of heat is released.
Then you can apply the following rule of three: if 184 kJ are produced when 2 moles of H₂O are formed, when 975 kJ are produced how many moles of H₂O are formed?
[tex]amount of moles of H_{2} O=\frac{975 kJx2 moles}{184 kJ}[/tex]
amount of moles of H₂O= 10.6 moles
Being the molar mass of H₂O 18 g/mole, the mass of H₂O formed when 975 kJ of energy are produced is:
10.6 moles× 18 [tex]\frac{g}{mole}[/tex]= 190.8 g
Finally, 190.8 g of H₂O must form in order to produce 975 kJ of energy.
Learn more about enthalpy of a chemical reaction:
brainly.com/question/19521752
