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Norma-Jean [14]
3 years ago
5

A new grill has a mass of 30.0 kg. you put 1.5 kg of charcoal in the grill. you burn all the charcoal and the grill has a mass o

f 30.0 kg. what is the mass in kg of the gases given off? (assume that the charcoal is pure carbon solid and that it burns completely in oxygen).
Chemistry
1 answer:
atroni [7]3 years ago
7 0

The reaction for burning of charcoal or complete combustion is as follows:

C(s)+O_{2}(g)\rightarrow CO_{2}(g)

From the above balanced reaction, 1 mole of carbon releases 1 mole of CO_{2} gas.

Converting mass of charcoal into moles as follows:

n=\frac{m}{M}

Molar mass of pure carbon is 12 g/mol thus,

n=\frac{1.5\times 10^{3} g}{12 g/mol}=125mol

The same moles of CO_{2} is released. Converting these moles into mass as follows:

m=n×M

Molar mass of CO_{2} is 44 g/mol thus,

m=125mol\times 44 g/mol=5.5\times 10^{3}g

Converting mass into kg,

1g=10^{-3}kg

Thus, total mass of gas released is 5.5 kg.

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The equilibrium constant, Kc, for the following reaction is 0.967 at 650 K. 2NH3(g) N2(g) 3H2(g) When a sufficiently large sampl
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Answer: Concentration of NH_3 in the equilibrium mixture is 0.31 M

Explanation:

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The given balanced equilibrium reaction is,

                 2NH_3(g)\rightleftharpoons N_2(g)+3H_2(g)

Initial conc.            x                0           0

At eqm. conc.     (x-2y) M     (y) M   (3y) M

The expression for equilibrium constant for this reaction will be:

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