Q1. Nitrogen gas reacts with oxygen gas to produce nitrogen monoxide in an exoth
ID: 1001441 • Letter: Q
Question
Q1. Nitrogen gas reacts with oxygen gas to produce nitrogen monoxide in an exothermic reaction. When the temperature of the reaction at equilibrium is lowered the equilibrium will
shift towards reactants
shift towards products
no change in equilbrium when the temperature is changed
no change in equilibrium for exothermic reactions
Q2. When the pressure is lowered on the reaction of solid carbon with liquid oxygen to produce gaseous carbon monoxide the equilibrium will
shift towards products
shift towards reactants
remain unchanged
none of the above
Q.3 When the equilibrium constant expression is written for the combination or synthesis reaction of nitrogen trifluoride what is the exponent of the concentration of fluorine?
1
2
3
0
4
Explanation / Answer
Q1 This is can be explain by Le Chatelier's principle this law of equilibrium.Since reaction is exothermic in forward direction so on cooling it shift towards product
shift towards products
Q2. Since in product is gaseous pressure is increase in forward direction so on lowering pressure it shifted towards product to maintain equilibrium cinstant equal.
shift towards products
Q3. reaction is
N2 +3 F2 = 2NF3
exponent of concentration of F2 = 3
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