4NH3 + 5O2 → 4NO + 6H2O
mole of NH3 x ____________ = mole of H2O
mole of NH3 x ____________ = mole of NO
mole of NH3 x ____________= mole of O2
mole of O2 x ___________= mole of NO
(a) 4 moles of NH3 produces 6 moles of H2O so conversion factor = 6/4 = 1.5
(b) 4 moles of NH3 produces 4 moles of NO, hence conversion factor is = 4/4 = 1
(c) 4 moles of NH3 require 5 moles of O2 so conversion factor of NH3 to O2 = 5/4 = 1.25
(d) 5 moles O2 produces 4 moles of NO, so conversion factor = 4/5 = 0.8
Write conversion factors (or coefficient ratio) for the following reaction: 4NH3 + 5O2 → 4NO +...
Consider the following reaction: 4NH3 + 5O2 4NO + 6H2O Determine the following rates at a time when the rate of consumption of O2 is 1.26e-03 M/s. a) rate of consumption of NH3 M/s b) rate of formation of NO M/s c) rate of formation of H2O M/s d) rate of reaction M/s
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 ---> 4NO + 6H2O When 20.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent? A) NO B) O2 C) H2O D) no reagent is limiting E) NH3 What is the coefficient for O2 when the following combustion reaction of a hydrocarbon is balanced? ___C7H14 + ___ O2 ---> ___ CO2 + __ H2O A) none of these B) 10...
Determine delta sub r H in Kj/mol for this reaction. 4No+6H2O --> 4NH3 +5O2 using the equations and the enthalpy change of the reactions given. N2 + O2 --> 2NO delta sub r H= 180.1 NH3 --> 1/2 N2 +1.5H2. delta sub r H= 54.3 2H2O --> 2H2 + O2 delta sub r H= 486.7
Consider the following equilibrium reaction: 4NH3(g) + 5O2(g) <---> 4NO(g) + 6H2O(g) Heat = -904.4 kJ How does each of the following changes affect the yield of NO at equilibrium? Answer increase, decrease, or no change. a. increase [NH3] b. Increase [H2O] c. Decrease [O2] d. Decrease the volume of the container in which the raction occurs. e. Add a catalyst f. Increase temperature
Consider the following reaction: 4NH3+5O2 -> 4NO+6H2O If 6.0 mol NH3 react with 7.0 mol O2, how many moles of reactions can be completed?
Calculate the ^Ho in (kj) for the following reaction : 4NH3 (s) + 5O2 (g) ---> 4NO (g) + 6H2O (l) ^Ho: NH3 - 46.0 NO 90.0 H2O - 286 A. - 1,172 B. - 1,716 C. - 150 D. - 1,356
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 +5O2 → 4NO + 6H2O What is the theoretical yield of water, in moles, when 40.0g NH3 and 50.0g O2 are mixed and allowed to react: 1.87 mol 3.53 mol 1.57 mol 1.30 mol None of these
(1) Which of the following statements is correct for the equation shown here? 4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2O(g) (a) 6 g of H2O are produced for every 4 g of NH3 reacted. (b) 1 mole of NO is produced per mole of NH3 reacted. (c) 2 moles of NO are produced for every 3 moles of O2 reacted. (2) Silicon reacts with chromium(III) oxide according to the equation 3Si(s) + 2Cr2O3(s) ⟶ 3SiO2(s) + 4Cr(s) If 59.4 g...
Consider the reaction4NH3(g) +5O2(g) ⇌ 4NO(g)+6H2O(g) where ΔS° rxn= 180.5 J/KUsing standard thermodynamic data (in the Chemistry References), calculate the entropy change of the surroundings and the universe at 25°C.
The following question refers to the reaction: 4NH3(g) + 5O2(g) ⇌ 4NO(g) + 6H2O(g) The reaction as written is exothermic. What will happen if heat is added to the system? (A) The equilibrium will shift to the left (B) The equilibrium will shift to the right (C) The NO concentration will remain constant, but there will be more water vapour (D) The equilibrium position will not change if heat is added (E) The system increase in temperature Explanation will be...