Answer: The equilibrium concentration of CO at 1000 K is 0.016 M , the equilibrium concentration of at 1000 K is= 0.033 M and the equilibrium concentration of at 1000 K is 0.139 M
Explanation:
Initial concentration of
Initial concentration of
The given balanced equilibrium reaction is,
Initial conc. 0.1550 M 0.172 M 0 M
At eqm. conc. (0.1550-x) M (0.172-x) M (x) M
The expression for equilibrium constant for this reaction will be,
we are given :
Now put all the given values in this expression, we get :
Thus the equilibrium concentration of CO at 1000 K is= (0.1550-x) M =(0.1550-0.139) M = 0.016 M
Thus the equilibrium concentration of at 1000 K is= (0.172-x) M =(0.172-0.139) M = 0.033 M
Thus the equilibrium concentration of at 1000 K is= x M = 0.139 M
In a chemical reaction, the atoms of the starting species called reactants rearrange to form new substances which are the products of the chemical reaction. The identities of the atoms involved in the reaction remain the same. Their number also stays the same before and after the reaction
Freezing could be a good answer
Answer:
The correct answer is 0.020 atm.
Explanation:
Partial pressure is calculated by using the formula,
Partial pressure = Mole fraction × Total pressure
The partial pressure of oxygen in a mixture can be calculated by using the formula,
Mole fraction of oxygen in mixture = Number of moles of oxygen / No. of moles of oxygen + No. of moles of Helium
(1 gg or gigagram is equal to 10⁹ grams)
= 2 × 10⁹/32 /2 × 10⁹/32 + 98 × 10⁹ / 4
= 2.54 × 10⁻³
Now the partial pressure of oxygen = Mole fraction of oxygen × Total pressure of oxygen
= 2.54 × 10⁻³ × 8.0 atm
= 0.02032 atm
= 0.020 atm
Answer & Explanation:
You could group them as acids and bases:
<u>Acids</u>
HCl
H₂SO₄
HClO₃
<u>Bases</u>
NaOH
Ca(OH)₂
LiOH