Energy can be extracted from water by:___________
1 answer:
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Explanation:
Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.
This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.
- On removal of reactant from equilibrium reaction ,shifts the equilibrium in backward direction.
- On addition of reactant from equilibrium reaction ,shifts the equilibrium in forward direction.
- On removal of product from equilibrium reaction, shifts the equilibrium in forward direction.
- On addition of product from equilibrium reaction, shifts the equilibrium in backward direction.
1. Water vapor is removed
On removal of water vapor from equilibrium will decrease the product which will lead to moving forward of an equilibrium that is equilibrium will shift to right direction.
2. is added
On addition of from equilibrium will increase the reactant which will lead to moving forward of an equilibrium that is equilibrium will shift to right direction.
3.The reaction is done in a glass reaction vessel. HF(g) attacks and reacts with the glass
Due to reaction of HF with glass will result in decrease in amount of HF present at equilibrium. So, order to counter this equilibrium will shift in backward direction or in left direction.
4. If the reaction is endothermic, and you want to make the equilibrium shift to the right to maximize the products, would you heat or cool the reaction vessel.
I endothermic reaction , heat is added to the reaction for which we can treat heat as a reactant.Now, we want to shift the equilibrium to right which means in the forward direction.
And this can be done by increasing the reactant amount, here by adding more heat to the equilibrium will shift the reaction to the right side.
So, for increasing heat we will heat the reaction vessel.
0.216 moles of gas can the container hold if a sealed container can hold 0.325 L of gas at 1.00 atm and 293 K.
<h3>What is an ideal gas equation?</h3>The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).
PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.
Given data:
R = gas constant = 0.08206 L.atm / mol K
T = temperature, Kelvin
V=5 L
P = 1.05 atm
T = 296 K
Putting value in the given equation:
Moles = 0.216 moles
Hence, 0.216 moles of gas can the container hold if a sealed container can hold 0.325 L of gas at 1.00 atm and 293 K.
Learn more about the ideal gas here:
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