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If nitrogen gas (N2) is added to a mixture of nitrogen (N2) and oxygen (O2), the overall reaction equilibrium and the partial pressures of the gases may change, but no new reactions would occur under standard conditions. The added N2 would increase the total pressure of the gas mixture without affecting the concentrations of O2 significantly, as nitrogen is inert in this context. This could lead to a decrease in the reaction quotient (Q) relative to the equilibrium constant (K) for any reactions involving N2 and O2, but since N2 is not reactive, the system would remain stable.
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What would happen if n2 were added to n2g plus o2g 2nog at equilibrium?
More No will be produced
What can be said about the reaction 2NH3g N2g 3H2g?
The reaction 2NH3(g) ⇌ N2(g) + 3H2(g) is an example of a dynamic equilibrium where ammonia (NH3) decomposes into nitrogen (N2) and hydrogen (H2) gases. The forward reaction is exothermic, meaning it releases heat, while the reverse reaction is endothermic. The equilibrium position can be affected by changes in temperature, pressure, or concentration, according to Le Chatelier's principle. This reaction is significant in the context of ammonia production and various industrial applications.
What would happen if n2 were added to n2g plus o2g 2nog at equilibrium?
More No will be produced
What would happen if o2 were added to n2g o2g - 2nog at equilibrium?
More NO would form.
What would happen if NO were added to N2g O2 g 2NO g at equilibrium?
Adding NO to the system at equilibrium would increase the concentration of the NO product. According to Le Chatelier's principle, the system will counteract this change by producing more of the reactants, N2 and O2.
Which of the following is true for the gas phase reaction shown below 2NH3g N2g plus 3H2g ΔH equals 160.58 kJ?
ΔS is positive and ΔG is negative at low temperatures only
12 l of ammonia were produced by the haber process how many liters of hydrogen were used during the reaction the reaction took place at stp 0c and 1.0 ATM n2g plus 3h2g 2nh3g?
According to the balanced chemical equation, 3 liters of hydrogen is required to produce 2 liters of ammonia. So, for 12 liters of ammonia, you would need 18 liters of hydrogen. This is because the ratio of hydrogen to ammonia in the reaction is 3:2.
Determine the change in volume that takes place when 1.95-L sample of N2g is heated from 250.0 K to 442.2 K?
To determine the change in volume, you can use the ideal gas law equation: V2 = V1*(T2/T1). Substituting the values, the change in volume would be V2 - V1 = V1*(T2/T1) - V1. Just plug in the initial volume of 1.95 L, initial temperature of 250.0 K, and final temperature of 442.2 K to find the change in volume.
How do you balance this equation h2g n2g nh3g?
3H2(g) + N2(g) ---> 2NH3(g)
What can be said about the reaction 2NH3g N2g 3H2g?
The reaction 2NH3(g) ⇌ N2(g) + 3H2(g) is an example of a dynamic equilibrium where ammonia (NH3) decomposes into nitrogen (N2) and hydrogen (H2) gases. The forward reaction is exothermic, meaning it releases heat, while the reverse reaction is endothermic. The equilibrium position can be affected by changes in temperature, pressure, or concentration, according to Le Chatelier's principle. This reaction is significant in the context of ammonia production and various industrial applications.
