For the reaction

H2(g) + CO2(g) ⇆ H2O(g) + CO(g)

at 700°C, Kc = 0.534. Calculate the number of moles of H2 that are present at equilibrium if a mixture of 0.680 mole of CO and 0.680 mole of H2O is heated to 700°C in a 70.0−L container.

Explanation:

Hello,

In this case, given the amounts of water and carbon dioxide we should invert the given reaction as hydrogen will be producted rather than consumed:

Consequently, the equilibrium constant is also inverted:

In such a way, we can now propose the law of mass action:

And we can express it in terms of the initial concentrations of the reactants and the change due to the reaction extent:

Thus, we compute the initial concentration which are same, since equal amount of moles are given:

Hence, solving for by using the quardratic equation or solver, we obtain:

For which the correct value is 0.00561M since the other one will produce negative concentrations of water and carbon monoxide at equilibrium. Therefore, the number of moles of hydrogen at equilibrium for the same 70.0-L container turn out:

Best regards.

the answer is 303.15 or 303

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.