According to the equation of molarity:
Molarity= no.of moles / volume per liter of Solution
when we have the molarity=0.58 M and the beaker at 150mL so V (per liter) = 150mL/1000 = 0.150 L
by substitution:
∴ No.of moles = Molarity * Volume of solution (per liter)
= 0.58 * 0.150 = 0.087 Moles
C preside over the the Senate
The equilibrium constant for the reaction is:
K subscript eq equals StartFraction StartBracket upper H subscript 2 EndBracket superscript 2 StartBracket upper O subscript 2 EndBracket over StartBracket upper H subscript 2 upper O EndBracket superscript 2 EndFraction.
<h3>What is equilibrium constant? </h3>
The equilibrium constant (Kₑq) for a given reaction is simply defined as the ratio of the concentration of the products raised to their coefficient to the concentration of the reactants raised to their coefficient.
For example, the equilibrium constant Kₑq for the reaction below is given as
2A <=> B
Kₑq = [B]/[A]²
<h3>How to determine the equilibrium constant </h3>
- 2H₂O(g) <=> 2H₂(g) + O₂(g)
- Equilibrium constant (Kₑq) =?
Kₑq = [H₂]²[O₂] / [H₂O]²
K subscript eq equals StartFraction StartBracket upper H subscript 2 EndBracket superscript 2 StartBracket upper O subscript 2 EndBracket over StartBracket upper H subscript 2 upper O EndBracket superscript 2 EndFraction.
Learn more about equilibrium constant:
brainly.com/question/17960050
We are given with the mass of pure iron that reacts with oxygen to form an oxide which has a given mass as well. the mass of oxygen reacted is 8.15-6.25 g or 1.9 grams. THen we convert the mass of the reactants to moles. Iron is equal to 0.1119 moles and oxygen is equal to 0.1188. We divide each number to the less amount. Hence iron is 1 and oxygen is approx 1. The empirical formula hence is FeO or ferrous oxide or Iron (II) oxide.
