A chemist knows that the
kJ for the reaction 2H2(g) + O2
(g) ---> 2H2O (g) ,and that
kJ
for the reaction H2 (g) + F2 (g) ---> 2HF
(g).
With this information he calculated the
for the reaction 2H2O (g) + 2F2
(g) ---> 4HF(g) + O2 (g) and
predicted whether
was positive or negative. How?
A chemist knows that the kJ for the reaction 2H2(g) + O2 (g) ---> 2H2O (g)...
2. Use Hess’s Law to determine the enthalpy of the reaction below. 2F2(g) + 2H2O(l) → 4HF(aq) + O2(g) DH˚= ? H2(g) + F2(g) → 2HF(aq) DH˚ = -546.6 kJ 2H2 (g) + O2(g) → 2H2O(l) DH˚ = -571.6 kJ a. 42 kJ b. -1120 kJ c. -251 kJ d. -521 kJ e. -1690 kJ
18. Given that AHorxn = -546.6 kJ H2 (g)+F2 (g)2HF (g) AH°rxn = -571.6 kJ 2H2 (g)+ O2 (g) 2H20 (1) Calculate the value of AHrxn for 2F2 (g) 4HF (g) + O2 (g) +2H20 (I)
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
Hydrogen is burned according to the following chemical reaction: 2H2(g) + O2(g) → 2H2O(l) ∆Hrxn = -286 kJ Given 100 g of H2 and excess O2, how much heat is released?
Calculate AH for the reaction CyHa(s) + 6F2(8) 2CF4(8) + 4HF(G) given the following information: As part of your answer, show how the equations can be added together to give the overall or net equation H2(g) + F2(g) + 2HF(g) AH--537 kJ C(s) + 2F2(8) CF4(8) AH--680. kJ 2C(s) + 2H2(g) → C2H4(8) AH- +52.3kJ HTML Editore BIVA-A- IEE311xx, - E V O 1 12pt - Paragraph -
From the enthalpies of reactio:
H2(
9.) From the enthalpies of reaction Hale) + F(b) → C(s) + 2F2(g) → 2C(s) + 2H2(g) → Calculate AH for the reaction of ethylene with F2: CzHa() + 6F2(g) 2HF(8) CF(b) CzH4(g) AH =-537 kJ AH = -680 kJ AH = +52.3 kJ → 2CF4(g) + 4HF(E)
For the reaction 2H2O(g)−⇀↽−2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g) the equilibrium concentrations were found to be [H2O]=0.250 M,[H2O]=0.250 M, [H2]=0.490 M,[H2]=0.490 M, and [O2]=0.750 M.[O2]=0.750 M. What is the equilibrium constant for this reaction?
The elementary reaction 2H2O(g)−⇀↽−2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O,H2O, H2,H2, and O2O2 reach 0.0200 atm,0.0200 atm, 0.00550 atm,0.00550 atm, and 0.00700 atm,0.00700 atm, respectively. What is the value of the equilibrium constant at this temperature? kp= ?
Given that H2(g) + F2(g) → 2 HF(g) AH;xn = -546.6 kJ 2 H2(g) + O2(g) + 2H,0(1) AH;x= -571.6 kJ calculate the value of AHEX for 2F2(g) + 2 H20(1) + 4HF(g) + O2(8) AH
2 pts Question 14 Consider the reaction 2H2(g) + O2(g) → 2H2O(l) AH = -286 kJ Which of the following is true? The reaction is exothermic The reaction is endothermic The reaction is neutral with respect to energy change Heat is absorbed by the system Information is not enough to tell about the energy change