Dark matter absorb light emit radiation and been observed directly.

A chemical reaction is said to have attained equilibrium when the rate of forward reaction is equal to the rate of reverse reaction. We are told that the Kc of the reaction is 0. 0108.

In the first case:

CaCO3 - 15.0 g/100g/mol/10 L = 0.015 M

CaO - 15.0 g/56 g/mol/10 L = 0.027 M

CO2 - 4.25 g/44 g/mol / 10 L = 0.0096 M

Q = [0.027] [0.0096]/0.015

Q = 0.017

Since Q > K, the concentration of CaCO3 increases

In the second case;

CaCO3 - 2.5 g/100g/mol/10 L =0.0025 M

CaO - 25.0 g/56 g/mol/10 L = 0.045 M

CO2 - 5.66 g/44 g/mol / 10 L = 0.013 M

Q = [0.045 ] [ 0.013]/[0.0025 ]

Q = 0.23

Q > K the concentration of CaCO3 increases

In the third case;

CaCO3 - 30.5 g/100g/mol/10 L =0.031 M

CaO - 25.5 g/56 g/mol/10 L =0.046 M

CO2 - 6.48 g//44 g/mol / 10 L = 0.015 M

Q = [0.046] [ 0.015]/[0.031]

Q = 0.022

Q> K hence the concentration of CaCO3 increases

Missing parts: At 900oC, Kc = 0.0108 for the reaction: CaCO3(s) <===> CaO(s) + CO2(g) A mixture of CaCO3, CaO, and CO2 is placed in a 10.0 Liter vessel at 900oC. For the following mixtures, will the amount of CaCO3 increase, decrease, or remain the same as the system approaches equilibrium? CaCO3 CaO CO2 At Equilibrium, CaCO3 will ?? 15.0 g 15.0 g 4.25 g Answer 2.5 g 25.0 g 5.66 g Answer 30.5 g 25.5 g 6.48 g Answer

Learn more about equilibrium: brainly.com/question/17960050

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3 years ago

. Which statement is true about healthy eating?

lbvjy [14]

<u>You can eat fast food occasionally in </u><u>moderation</u><u>.</u><u> </u>

<u> $\: \: \: \: \:$ </u>

Because if you eat it daily then u will ruin your health.

<h2>—<u>WtfHawty</u><u> </u><u>☽</u></h2>

4 0

2 years ago

Read 2 more answers

When the chemical reaction 2no(g)+o2(g)→2no2(g) is carried out under certain conditions, the rate of disappearance of no(g) is 5

viktelen [127]

The rate of disappearance of O2(g) under the same conditions is 2.5 × 10⁻⁵ m s⁻¹.

<h3>What is the rate law of a chemical equation? </h3>

The rate law of a chemical reaction equation is usually dependent on the concentration of the reactant species in the equation.

The chemical reaction given is;

$\mathbf{2 NO_{(g)} + O_{2(g)} \to 2 NO_{2(g)} }$

The rate law for this reaction can be expressed as:

$\mathbf{= -\dfrac{1}{2}\dfrac{d[NO]}{dt} = -\dfrac{1}{1}\dfrac{d[O_2]}{dt}= +\dfrac{1}{2}\dfrac{d[NO_2]}{dt}}$

Recall that:

The rate of disappearance of NO(g) = 5.0× 10⁻⁵ m s⁻¹.

Since both NO and O2 are the reacting species;

Then:

The rate of disappearance of NO(g) is equal to the rate of disappearance of O2(g)

$\mathbf{= -\dfrac{1}{2}\dfrac{d[NO]}{dt} = -\dfrac{1}{1}\dfrac{d[O_2]}{dt}}$

$\mathbf{= -\dfrac{1}{2} \times 5.0 \times 10^{-5} = rate \ of \ disappearance \ of \ O_2}$

Thus;

The rate of disappearance of O2 = 2.5 × 10⁻⁵ m s⁻¹.

Therefore, we can conclude that two molecules of NO are consumed per one molecule of O2.

Learn more about the rate law here:

brainly.com/question/14945022

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2 years ago