Explanation:
According to Le Chatelier's principle, any disturbance caused in an equilibrium reaction will shift the equilibrium in a direction that will oppose the change.
As the given reaction is as follows.
(a) When increase the temperature of the reactants or system then equilibrium will shift in forward direction where there is less temperature. It is possible for an endothermic reaction.
Thus, formation of 
will increase.
- (b) When we decrease the volume (at constant temperature) of given reaction mixture then it implies that there will be increase in pressure of the system. So, equilibrium will shift in a direction where there will be decrease in composition of gaseous phase. That is, in the backward direction reaction will shift.
Hence, formation of will decrease with decrease in volume.
- When we increase the mount of
then equilibrium will shift in the direction of decrease in concentration that is, in the forward direction.
Thus, we can conclude that formation of will increase then.
Answer:
The pressure of the gas after getting compressed is 1.92 L.
Explanation:
To calculate the new pressure, we use the equation given by Boyle's law. This law states that pressure is directly proportional to the volume of the gas at constant temperature.
The equation given by this law is:
(At constant temperature)
where,
are initial pressure and volume.
are final pressure and volume.
We are given:
Putting values in above equation, we get:
The pressure of the gas after getting compressed is 1.92 L.
The number of covalent bonds is determined by the number of valence electrons of an element. The number of electrons tells the maximum number of bonds an element allows. In this case, an oxygen atom requires two bonds. So for Sio2, each oxygen atoms are bonded in double bonds to Si. Hence there are two covalent bonds.
Based on the principle of conservation of energy, the heat capacity of the calorimeter is calculated using the formula:
- c = {m2 × w × (t2 - t1) - m2 × w × (t2 -t1)}/m3 × (t2 -t1)
<h3>What is a calorimeter?</h3>
A calorimeter is an equipment used to determine heat of reaction.
The calorimeter works on the principle of conservation of energy:
Quantity of heat energy is calculated using the formula below:
- q = mass × heat capacity × temperature difference
In the experiment, the following procedure is followed:
- Mass of the hot water, cold water and calorimeter are recorded
- temperature of the hot water is recorded
- temperature of the the cold water and calorimeter is recorded
- final temperature of the mixture is recorded
- heat capacity of the calorimeter is calculated using the formula: heat gained by calorimeter and cold water = heat lost by hot water.
Assuming that;
- mass of hot water = m1
- mass of cold water =m2
- mass of calorimeter = m3
- initial temperature cold water and calorimeter = t1
- final temperature of mixture = t2
- heat capacity of water = w
- heat capacity of calorimeter = c
Therefore, the heat capacity of the calorimeter is calculated using the formula:
- c = {m2 × w × (t2 - t1) - m2 × w × (t2 -t1)}/m3 × (t2 -t1)
Learn more about calorimeters at: brainly.com/question/1407669
