The volume of 0.98 mol oxygen gas at 275 k and a pressure of 2.0 atm is 11.06L.
<h3>How to calculate volume?</h3>
The volume of a given mass of gas can be calculated using the following formula:
PV = nRT
Where;
- P = pressure
- V = volume
- R = gas law constant
- T = temperature
- n = number of moles
According to this question, 0.98 moles of oxygen gas at 275 k contains a pressure of 2.0 atm. The volume is calculated as follows:
2 × V = 0.98 × 0.0821 × 275
2V = 22.13
V = 11.06L
Therefore, the volume of 0.98 mol oxygen gas at 275 k and a pressure of 2.0 atm is 11.06L.
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Is it Technology? What have you already tried?
Answer:
high pressure of 200-300 atm.
low temp. of between 400-500 degrees celsius:this is for continuous development of ammonia since it decomposes at high temp fathermore the reaction is exothermic
a catalyst to speed up the rate of reaction:i guess it is finely divided iron impregnated in aluminium oxide
platinum can be used as a catalyst but it is easily poisoned
hope it helps
Explanation:
Answer : The equilibrium will shift in the left direction.
Explanation :
Le-Chatelier's principle : This principle states that if any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.
The given reaction is:
As per question, when we are adding 
then the concentration of is increased on product side then the equilibrium will shift in the direction where decrease of concentration of takes place. Therefore, the equilibrium will shift in the left direction.
Thus, the equilibrium will shift in the left direction.
Answer: possibly diffusion
Explanation:
all particles are in motion unless at a certain degree so they'd spread throughout the room diluting as they continue to spread out.
