ΔS is negative for the reaction ________.
2H2O (g) → 2H2 (g) + O2 (g)
LiOH (aq) → Li+ (aq) + OH– (aq)
CH3OH (l) → CH3OH (g)
Sr(NO3)2 (aq) + 2LiOH (aq) → Sr(OH)2 (s) + 2LiNO3 (aq)
C6H12O6 (s) → 6C (s) + 6H2 (g) + 3O2 (g)
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ΔS is negative for the reaction ________. 2H2O (g) → 2H2 (g) + O2 (g) LiOH...
AS is negative for the reaction C6H1206 (s) — 6C (s) + 6H2 (g) + 302 (g) LiOH (aq) - Li+ (aq) + OH- (aq) Sr(NO3)2 (aq) + 2LIOH (aq) → Sr(OH)2 (s) + 2LİNO3 (aq) 2H20 (g) → 2H2 (g) + O2 (g) CH3OH (1) CH3OH (g)
8) AS is negative for the reaction A) C6H1206 (s) - 6C (s) + 6H2 (g)+302 (g) B) CH30H (I)-CH30H (g) C) Sr(NO3)2 (aq) 2LiOH (aq) Sr(OH)2 (s)+ 2LiNO3 (aq) D) LiOH (aq) Li+ (aq)+OH-(aq) E) 2H20 (g) 2H2 (g) 02 (8) (Sec. 19.4)
8) AS is negative for the reaction A) C6H1206 (s) - 6C (s) + 6H2 (g)+302 (g) B) CH30H (I)-CH30H (g) C) Sr(NO3)2 (aq) 2LiOH (aq) Sr(OH)2 (s)+ 2LiNO3 (aq) D) LiOH (aq) Li+ (aq)+OH-(aq) E)...
Please help. Thanks.
AS is negative for the reaction a. C6H1206 (5) 6C (s) + 6H2 (g) + 302 (g) b. Sr(NO3)2 (aq) + 2LIOH (aq) Sr(OH)2 (s) + 2LINO3 (aq) 2H20 (8) 2H2 (g) + O2 (g) d. CH3OH (I) - CH3OH (9) e LIOH (aq) - Li+ (aq) + OH- (aq)
At what temperature is this reaction spontaneous? 2H2(g)+O2(g)⟶2H2O(g)ΔH∘=−241.82kJ;ΔS∘=−88.75J/K
1) 2H2O(g) → 2H2 (g) + O2 (g) DH = 483.6 kJ If 5 moles of water vapor decompose to form hydrogen and oxygen gas at a pressure of 1.0 atm and 125 oC, what is the change in internal energy of the system? 2)How much heat (in kJ) is evolved when 266 g of white phosphorus (P4 ) burn in air? P4 (s) + 5O2 (g)---> P4O10(s) DH = -3013 kJ 3) A quantity of 1.00 × 102 mL...
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
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?
Consider the reaction: 2H2O (l) ----> 2h2 (g) + O2 (g) What mass of H2O (MW=18.02) is required to form 1.4 L of O2 at a temperature of 30.0 degrees C and a pressure of 750 torr?
AS is negative for the reaction O CH3OH(1) + CH3OH(g) OKBr(aq) + K+ (aq) + Br(aq) O C6H12O6(s) + 6 C(s) + 6 H2(g) + 3 02 (g) O 2 NH3(g) + N2(g) + 3 H2(g) Mg(NO3)2 (aq) + 2 NaOH(aq) → Mg(OH)2 (s) + 2 NaNO3(aq) Submit Request Answer
Use Hess’s law to calculate ∆H° for the reaction:C(s) + 2H2(g) + ½O2(g) → CH3OH(l) ∆H°∘= ?using only the following data:H2(g) + ½O2(g) → H2O(l) ∆H°= -285.8 kJC(s) + O2(g) → CO2(g) ∆H°= -393.5 kJ2CH3OH(g) + 3O2(g) → 2CO2(g) + 4H2O(l) ∆H°= -1452.8 kJ