Answer: 64.8
Explanation:Please see attachment for explanation
Answer:
Le'chetelliers principle states that when an external factor such as temperature and pressure is added to a system in equilibrium...the disequilibrium will shift so as to annul the effect
Explanation:
To know the cause of increase in pressure in the above equation ...
You should note 2 things
1. the number of moles of all gaseous elements on both side and 2. How change in temperature will affect the equilibrium....
There are 4 moles on the left and 2 on the right ..
making it 4 : 1
so...increase in temperature will shift the equilibrium to the favour the reaction with fewer molecules thereby shifting it right ...the reverse is the case as to decrease in temperature
however; increase in temperature ...if it's an endothermic reaction having a positive sign...tge equilibrium will shift to the right and there will be increase in K....the reverse also is the case as to an exothermic reaction where delta h is negative -ve
To solve this we assume
that the gas is an ideal gas. Then, we can use the ideal gas equation which is
expressed as PV = nRT. At a constant temperature and number of moles of the gas
the product of PV is equal to some constant. At another set of condition of
temperature, the constant is still the same. Calculations are as follows:
P1V1 =P2V2
V2 = P1 V1 / P2
V2 = 153 x 3.00 / 203
<span>V2 = 2.26 L</span>
A chemical reaction does happen between sodium and water to form Sodium Hydroxide (NaOH) and Hydrogen Gas (H-2)
