4NH3 + 7O2 → 4NO2 + 6H2O
When the rate of disappearance of NH3 is 0.48 M/s , the rate of appearance of H2O is ________ M/s
4NH3 + 7O2 → 4NO2 + 6H2O When the rate of disappearance of NH3 is 0.48...
QUESTION 12 4NH3 + 702 + 4NO2 + 6H20 When the rate of disappearance of O2 is 0.48 M/s, the rate of appearance of NO2 is *Please report 2 significant figures. Numbers only, no unit. No scientific notation.
Nitrogen dioxide reacts with water to produce oxygen and ammonia: 4NO2(g)+6H2O(g)→7O2(g)+4NH3(g) How many grams of NH3 can be produced when 4.10 L of NO2 reacts at 385 ∘C and 735 mmHg ?
Calculate ∆H°rxn using ∆Hf° for the reaction 4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(l ) Compound ∆H°f (kJ/mol) NH3(g) -46.0 NO2 (g) +34.0 H2O(l) -285.9
Refer to the following equation: 4NH3(g) + 7O2(g) ® 4NO2(g) + 6H2O(g) How many molecules of water are produced for each mole of NO2 given off?
from the balanced equation 4NH3 +7O2 - 4NO2 + 6H2O. How many grams of oxygen are necessary to produce 4.50 moles of NO2? I think its 11 grams or 22 grams but im not sure. please help!! First the number of moles of O2, molesO2= (4/7) moles NO2 Notice those came from the balanced equation. Put in 4.5 moles NO2, and you have moles of O2. Grams of O2? multiply moles of O2 by 32. what do you mean I...
Question 8. A study of the system, 4NH3(g) + 7O2
----------> 2N2O4(g) * 6H2O(g), was carried out. A system was
prepared with [NH3]=[O2]= 3.60M as the only components intially. At
equilibrium, [N2O4] is 0.600M. Calculatevthe equilibrium
concentratiok of NH3.
AUIUS H2Se, HzTe, and H2S in order of increasing acid strength. 8. A study of the system, 4NH3(g) + 702(9) 2N2O4(9) + 6H2O(g), was carried out. A system was prepared with (NH2) = (O2) = 3.60 M as the only components...
QUESTION 8 Consider the reaction: 4NH3 +702-4NO2 + 6H20. At a certain instant, the rate of disappearance of the oxygen gas is 1.20 M/s. Which of the following is NOT true? Choose this answer only if all of the other choices are true. The rate of appearance of water at the same instant would be 1.03 M/S. The rate constant for this reaction changes with temperature, but not with the concentrations of reactants used. The initial rate of disappearance of...
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 nitrogen dioxide and steam, as follows: 4NH3(g) + 7O2(g) ---> 4NO2(g) + 6H2O(g) Using the following bond energies, estimate the enthalpy change for the reaction. BE(O–H) = 464 kJ/mol BE(N–H) = 389 kJ/mol BE(O=O) = 498 kJ/mol BE(N–O) = 222 kJ/mol BE(N=O) = 590 kJ/mol
Consider the following reaction: 4NH3(g) + 7O2(g) à 4 NO2(g) + 6H2O (l) Is it a balanced or unbalance equation? How many liters of nitrogen dioxide gas is produced from 527 g of gaseous ammonia? Hint: At standard temperature & pressure, 1 mole gas occupies 22.4 Liters