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2 years ago

Need helpppppp hurry pls, i just really need help

Chemistry

1 answer:

mojhsa [17]2 years ago

7 0

Answer:

6.8 mole of O₂

Explanation:

Given expression:

2H₂ + O₂ → 2H₂O

Number of moles of H₂ = 13.6moles

Unknown:

Number of moles of O₂ = ?

Solution:

In the given problem, we are to find the number of moles of oxygen gas that will use up 13.6mole of hydrogen gas;

From the reaction equation;

2 mole of H₂ will completely react with 1 mole of O₂

13.6 moles of H₂ will completely be used up by $\frac{13.6}{2}$ mole of O₂

= 6.8 mole of O₂

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Answer:

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Explanation:

ΔHrxn = 2ΔHf (Al₂O₃) - ΔHf (Fe₂O₃)

Remember that for pure elements in their standard state of temperature and pressure by definition their standard heats of formation are zero.

ΔHrxn = 2(-1675.7) - (-824.3) kJ/mol

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Given the equilibrium constants for the following two reactions in aqueous solution at 25 ∘C HNO2(aq)H2SO3(aq)⇌⇌H+(aq) + NO2−(aq

krok68 [10]

Answer : The value of $K_c$ for the final reaction is, 184.09

Explanation :

The equilibrium reactions in aqueous solution are :

(1) $HNO_2(aq)\rightleftharpoons H^+(aq)+NO_2^-(aq)$ $K_{c_1}=4.5\times 10^{-4}$

(2) $H_2SO_3(aq)\rightleftharpoons 2H^+(aq)+SO_3^{2-}(aq)$ $K_{c_2}=1.1\times 10^{-9}$

The final equilibrium reaction is :

$2HNO_2(aq)+SO_3^{2-}(aq)\rightleftharpoons H_2SO_3(aq)+2NO_2^-(aq)$ $K_{c}=?$

Now we have to calculate the value of $K_c$ for the final reaction.

Now equation 1 is multiply by 2 and reverse the equation 2, we get the value of final equilibrium reaction and the expression of final equilibrium constant is:

$K_c=\frac{(K_{c_1})^2}{K_{c_2}}$

Now put all the given values in this expression, we get :

$K_c=\frac{(4.5\times 10^{-4})^2}{1.1\times 10^{-9}}=184.09$

Therefore, the value of $K_c$ for the final reaction is, 184.09

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