For the following reaction, if O2 is used up at a rate of 1.45Mhr, what is the rate of formation of H2O?
4NH3+5O2→4NO+6H2O
For the following reaction, if O2 is used up at a rate of 1.45Mhr, what is...
For the following reaction, to get the rate of formation of H2O, what must we multiply the rate of consumption of O2 by? 4NH3+5O2→4NO+6H2O Report your answer as a fraction.
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
Calculate the change of enthalpy for the reaction N2 + O2 --> 2NO from the following reactions: Reaction 1: 4NH3 + 3O2 --> 2N2 + 6H2O Change in enthalpy: -1530 kJReaction 2: 4NH3 + 5O2 --> 4NO + 6H2O Change in enthalpy: -1170 kJReaction 3: 2N2 + 6H2O --> 4NH3 + 3O2 Change in enthalpy: +1530 kJ
1)For the following reaction, to get the rate of formation of SiO2, what must we multiply the rate of formation of H2O by? 2Si2H2+5O2⟶4SiO2+2H2O 1/2 2 −1/2 −2 2)For the following reaction, if O2 is used up at a rate of 4.42Mhr, what is the rate of consumption of NH3? 4NH3+5O2→NO+4H2O =____moles per liter hour 3)All of the following are true about catalysts, EXCEPT: Select the correct answer below: Catalysts can speed up the rate of a reaction. They cause...
When NH3(g) reacts with O2(g) according to the following reaction, 226kj of energy is released for each mole of NH3 (g) that reacts. Complete the following thermochemical equation. 4NH3(G) + 5O2(g) = 4NO(g) + 6H2O ^H = _______ kj
. Given the following reaction at 25o C. 4NH3(g) + 5 O2(g) 4NO(g) + 6H2O(l) ΔHo = -1168 kJ ΔHo f(NH3) = -46.2 kJ/mol; ΔHo f(H2O) = -285.8 kJ/mol. What is the standard enthalpy of formation of NO gas at 25o C?
For the following reaction, if NH3 is used up at a rate of 0.30Mmin, what is the rate of formation of N2? 2NH3→N2+3H2 Answer should be in two significant figures.
Use standard enthalpies of formation to determine the ΔHo in kJ for the following reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) ΔHfo (NH3(g)) = -45.90 kJ/mol ΔHfo (NO(g)) = 90.29 kJ/mol ΔHfo (H2O(g)) = -241.83 kJ/mol
If the reaction consumes (uses up) 31.7 moles of ammonia, how many grams of water will be produced using the following equation? 4NH3 + 5O2 g 4NO + 6H2O
Confused on #5
5) Calculate the enthalpy of the following reaction: N2 + O2 ---> 2NO Given: 4NH3 + 502 ---> 4NO + 6H2O AH° = -1170 kJ 2N2 + 6H2O ---> 4NH3 + 302 AH° = +1530 kJ Solution: