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2 years ago

What is the percent yield of ferrous sulfide if the actual yield is 220.0 g and the theoretical yield is 275.6 g?

Chemistry

1 answer:

BaLLatris [955]2 years ago

7 0

<h2>Hello!</h2>

The answer is:

The third option, 79.8%

To calculate the percent yield we need to divide the actual yield by the theoretical yield, and then, multiply it by 100 in order to find the percent.

So, we from the statement we know the following information:

$ActualYield=220.0g\\TheoreticalYield=275.6g$

Let's use the following formula and substitute the given information:

$PercentYield=\frac{ActualYield}{Theoretical}*100\\\\$

$PercentYield=\frac{220g}{275.6g}*100=0.798*100=79.8(percent)$

Hence, we have that the correct option is the third option, the percent yield is 79.8%.

Have a nice day!

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Determine the value of the equilibrium constant, Kgoal, for the reaction CO2(g)⇌C(s)+O2(g), Kgoal=? by making use of the followi

marta [7]

Answer : The value of $K_{goal}$ for the final reaction is, $1.238\times 10^{-7}$

Explanation :

The following equilibrium reactions are :

(1) $2CO_2(g)+2H_2O(l)\rightleftharpoons CH_3COOH(l)+2O_2$ $K_1=5.40\times 10^{-16}$

(2) $2H_2(g)+O_2(g)\rightleftharpoons 2H_2O(l)$ $K_2=1.06\times 10^{10}$

(3) $CH_3COOH(l)\rightleftharpoons 2C(s)+O_2(g)$ $K_3=2.68\times 10^{-9}$

The final equilibrium reaction is :

$CO_2(g)\rightleftharpoons C(s)+O_2(g)$ $K_{goal}=?$

Now we have to calculate the value of $K_{goal}$ for the final reaction.

First half the equation 1, 2 and 3 that means we are taking square root of equilibrium constant and then add all the equation 1, 2 and 3 that means we are multiplying all the equilibrium constant, we get the final equilibrium reaction and the expression of final equilibrium constant is:

$K_{goal}=\sqrt{K_1\times K_2\times K_3}$

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

$K_{goal}=\sqrt{(5.40\times 10^{-16})\times (1.06\times 10^{10})\times (2.68\times 10^{-9})}$

$K_{goal}=1.238\times 10^{-7}$

Therefore, the value of $K_{goal}$ for the final reaction is, $1.238\times 10^{-7}$

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What is the atomic number of the as yet undiscovered element in which the 8s and 8p electron energy levels?

Andreyy89

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Element 118 will have just filled its 7p orbitals. therefore the predicted element to fill completely up to its 8 p orbital would have to filled a whole set of s, p, d, f and g orbitals

That's another 2 + 6 + 10 +14 + 18 = 50 electrons

To determine the total number of quantum numbers we have to find

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