0.25 mol of CO and 0.45 mol of NO2 are mixed in a 25 L reaction vessel at 350°C. Calculate the molarities of all compounds present in the vessel once the equilibrium is reached. (6 points) CO(g) + NO2(g) ⇌ CO2(g) + NO(g) Kc = 67.5

[CO₂] = [NO]  ≈ 0.11 mol/dm³

[CO]  = 0.25 mol/(25 L) = 0.01 mol/dm³

[NO₂] = 0.45 mol/(25 L) = 0.018 mol/dm³

Explanation:

The number of moles of CO = 0.25 moles

The number of moles of NO₂ = 0045 moles

The temperature of the vessel = 350°C

The equilibrium constant, Kc = 67.5

We have;

The product of the the concentration of the products = Kc × The product of the concentration of the reactants, therefore;

[CO₂] × [NO] = 67.5 ×(0.25/25 × 0.45/25) = 0.01215

Given that [CO₂] = [NO], we get;

[CO₂] = [NO] = √0.01215 ≈ 0.11 mol/dm³

[CO]  = 0.25 mol/(25 L) = 0.01 mol/dm³

[NO₂] = 0.45 mol/(25 L) = 0.018 mol/dm³

the answer is the first option

explanation:

just googled it m8. not that hard

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the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.