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10) Use the following decomposition reaction to answer the following questions: 2H2O(g) + heat - 2H2(g)...
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
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?
consider the following reaction 2H2(g)+O2(g)--> 2H2O (I) delta H= -572KJ A) how much heat is evolved when 1.00 mole of H2O (I) is produced? B) how much heat is evolved when 4.03g H2 are reacted with 40.0g of O2? C) the total volume of hydrogen gas needed to fill the Hindenburg was 2.0*10^8 L at 1.0 atm and 25 degree C. How much HEAT was evolved when the Hidenburg exploded, assuming all of the hydrogen reacted (plenty of oxygen)?
Consider the reaction 2H2 (g) + O2 (g) 2H2O(g) How will the equilibrium shift when hyDragen gas is removed? The reaction will shift toward both the reactants and products. The reaction will not shift toward either the products or reactants. The system will shift toward the reactants. The system will shift toward the products. Consider the exothermic reaction Fe2O3(s) + 2Al(s) Al2O3(s) + 2Fe(s) In what direction will the equilibrium shift when heat is removed? The reaction will shift toward...
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 Ho- 485
Use bond energies to calculate ?Hrxn for the
reaction.
2H2(g)+O2(g)?2H2O(g)
Note: The answer is NOT 442 kJ or 442kJ/mol
It gave me this hint when I got the answer wrong: The bond
energies of H?H, O=O, and H?O are provided in the introduction. To
determine the enthalpy of this reaction, sum all of the bond
energies for the reactants (accounting for stoichiometric ratios as
is), and subtract the bond energies for the product. Note how many
bonds are in each...
1. Given the following reaction, use Stoichiometry to answer the following questions: 2 H2O2 (I) → 2 H2O (I) + O2 (g) ΔH° = -196.1 kJ a. When O2 is formed is the reaction exothermic or endothermic? How can you tell from the information provided with the balanced equation? b. How many grams of hydrogen peroxide are required to form 4.20 mol O2? c. How much heat is exchanged when 24 kg of hydrogen peroxide decomposes? d. How much oxygen...
NEED ANSWERS ASAP PLZ
QUESTION 4 AH° = -560 kJ Look at this reaction: 2H2(g) + O2(g) --> 2H20(1) Which one of the following statements is true? O Heat is absorbed during the reaction O The reaction is endothermic O The enthalpy change is positive O This reaction is exothermic QUESTION 3 If AH = 25 J for a certain process, that process O releases heat O is exothermic. O is endothermic. O can't tell
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= ?