Consider the reaction
H2(g) + O2(g) = H2O2(l)
Calculate ▲H for the complete reaction of 40.0g of H2(g) and excess O2(g).
▲H°rxn = -184.5kJ
Consider the reaction H2(g) + O2(g) = H2O2(l) Calculate ▲H for the complete reaction of 40.0g...
Consider the following gas reaction at STP: H2(g) +O2(g) -->H2O2(g). Calculate the final volume if 2.0 moles of hydrogen gas react with 2.0 moles of oxygen gas. (R=0.08206 L*atm/mol*K)
calculate enthalpy of H for the reaction N2H4(l) + 2H2O(l) -> N2(g) + 4H2)(l) Given the reactions N2H4(l) + O2(g) -> N2(g) + 2H2O(l) Enthalpy of H = -6.22.2 kJ H2(g) + (1/2)O2(g) -> H2O(l) enthalpy of H = -285.8 kJ/mol H2(g) + O2(g) -> H2O2(l) enthalpy of H = -187.8 kJ
Consider the reaction: 2 H2O2(g) ⇄ 2 H2O(g) + O2(g). 1.75 moles of H2O2 are initially placed in a 2.50 L reaction vessel. When equilibrium is reached 1.20 moles of H2O2 are left. Calculate the equilibrium constant Kc. 5.5×10-3 2.4×10-3 2.0×10-4 2.3×10-2 3.9×10-4
Consider the following data. CH4(g) C(s) + 2 H2(g) H = +74.8 kJ C(s) + O2(g) CO2(g) H = -393.5 kJ 2 H2(g) + O2(g) 2 H2O(l) H = -571.7 kJ Use Hess's law to calculate H for the reaction below. CH4(g) + 2 O2(g) CO2(g) + 2 H2O(l) H = _____ kJ
Calculate Gibbs free energy for this reaction (in kJ): 2 H2O2(l) → 2 H2O(l) + O2(g) what is the answer?
1.Calculate the free energy(ΔG°)of the following reactions: a)H2(g) + O2(g)→ H2O2(g) b)H2O2(g) + H2(g) → 2 H2O (g) How do the free energy values for these two reactions compare to the free energy of the combustion of hydrogen gas? Hint: (ΔG) is a state function, therefore Hess’s law is applicable.The combustion of hydrogen gas is modeled by the overall equation is 2 H2(g) + O2(g)→ 2 H2O(g). 2.Based on your calculations in the previous question and your understanding of reaction...
For the voltaic cell shown, calculate the standard emf. Pt(s), H2(g) l H+(aq) ll H+(aq), H2O2(aq), H2O(l) l Pt(s) St. Red. Pot. (V) H+/H2 = 0 H2O2/H2O = 1.78
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)?
The value of Kp for the reaction H2(g) + O2(g) H2O2(g) is 2.3 × 106 at 610K. Determine the value for K for this reaction at 610K. a. 1.2 × 1010 b. 4.6 × 104 c. 1.2 × 108 d. 2.3 × 106 e. 4.3 × 10–7
Consider the reaction 2H2(g) + O2(g) +2H2O(l) What is the mass of water, H.O(l). produced when 6.25 g of O2(g) reacts with excess H2(g)?