Answer:
I believe the correct answer is
C.)Reasoning
Explanation:
The answer is a identical
The pressure of the oxygen gas collected : 718 mmHg
<h3>Further explanation</h3>
Given
P tot = 748 mmHg
P water vapour = 30 mmHg
Required
P Oxygen
Solution
Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases
Can be formulated:
P tot = P1 + P2 + P3 ....
The partial pressure is the pressure of each gas in a mixture
P tot = P H₂O + P Oxygen
P Oxygen = 748 mmHg - 30 mmHg
P Oxygen = 718 mmHg
Answer: = 1.834 M
= 0.004 M
= 0.166 M
Explanation:
Initial concentration of = 0.15 M
Initial concentration of = 2.0 M
The given balanced equilibrium reaction is,
Initial conc. 2 M 0.15 M 0
At eqm. conc. (2-x) M (1-6x) M (x) M
The expression for equilibrium constant for this reaction will be,
Now put all the given values in this expression, we get :
By solving the term 'x', we get :
= (2-x) = 2-0.166 = 1.834 M
= (1-6x) = 1-6(0.1660)= 0.004 M
= x = 0.166 M
Answer:
I could create a slower reaction because the particles might be moving slower due to the cold. if it was warm there will be a faster reaction. similar to the elements movements in solids and liquids.