D. Air molecules touch the warm ground, heating them up
Two changes would make this reaction reactant-favored
C. Increasing the temperature
D. Reducing the pressure
<h3>Further explanation</h3>
Given
Reaction
2H₂ + O₂ ⇒ 2H₂0 + energy
Required
Two changes would make this reaction reactant-favored
Solution
The formation of H₂O is an exothermic reaction (releases heat)
If the system temperature is raised, then the equilibrium reaction will reduce the temperature by shifting the reaction in the direction that requires heat (endotherms). Conversely, if the temperature is lowered, then the equilibrium shifts to a reaction that releases heat (exothermic)
While on the change in pressure, then the addition of pressure, the reaction will shift towards a smaller reaction coefficient
in the above reaction: the number of coefficients on the left is 3 (2 + 1) while the right is 2
As the temperature rises, the equilibrium will shift towards the endothermic reaction, so the reaction shifts to the left towards H₂ + O₂( reactant-favored)
And reducing the pressure, then the reaction shifts to the left H₂ + O₂( reactant-favored)⇒the number of coefficients is greater
Answer:
87.27 grams
Explanation:
The mole ratio of nitrogen to hydrogen is 1:3; while that one of hydrogen to the products (ammonia) is 3:2
Thus if 3 moles of hydrogen gas produce 2 moles of ammonia gas
7.7 moles of hydrogen will produce:
(7.7moles×2)/3
77/15 moles
1 mole of ammonia gas has a mass of 14+3=17
since the mass of an atom of nitrogen is 14 while that of hydrogen atom is 1.
Therefore 77/15 moles will have a mass of
77/15 moles × 17=87.27 grams
Explanation:
Mg + <u>2</u>HNO2 → Mg(NO2)2 + H2
