Advertisements
Advertisements
प्रश्न
The formation of ammonia from N2(g) and H2(g) is a reversible reaction
\[\ce{N2(g) + 3H2(g) <=> 2NH3(g) + Heat}\]
What is the effect of increase of temperature on this equilibrium reaction.
पर्याय
equilibrium is unaltered
formation of ammonia is favoured
equilibrium is shifted to the left
reaction rate does not change
उत्तर
equilibrium is shifted to the left
APPEARS IN
संबंधित प्रश्न
The equilibrium constant for a reaction at room temperature is K1 and that at 700 K is K2 If K1 > K2, then
Solubility of carbon dioxide gas in cold water can be increased by ______.
Consider the reaction where Kp = 0.5 at a particular temperature
\[\ce{PCl5(g) <=> PCl3 (g) + Cl2 (g)}\]
if the three gases are mixed in a container so that the partial pressure of each gas is initially 1 atm, then which one of the following is true.
A 20 litre container at 400 K contains CO2 (g) at pressure 0.4 atm and an excess (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when the pressure of CO2 attains its maximum value will be:
Given that: \[\ce{SeCO3(S)≅ SrO + CO2 (g)}\] [Kp = 1.6 atm]
State Le – Chateller principle.
A sealed container was filled with 0.3 mol H2(g), 0.4 mol I2(g) and 0.2 mol HI(g) at 800 K and total pressure 1.00 bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 870 for the reaction, \[\ce{A2 (g) + B2 (g) <=> 2 AB (g)}\].
