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3 years ago

How many moles of Co2 will be produced if 9.0 moles of O2 completely react?

1 answer:

8 0

<span>It depends on what was being combusted.

Supposing the simplest case, where carbon is being burnt:

C + O2 → CO2

(9.0 mol O2) x (1 mol CO2 / 1 mol O2) = 9.0 mol CO2

The answer would be different if the fuel contained any oxygen atoms, for example, alcohol.</span><span>
</span>

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Consider the following equilibrium reaction having gaseous reactants and products.4HCl + O2 ⇌ 2H2O + Cl2Which of the following w

Eddi Din [679]

According to what is known about chemical equilibrium and Le Chatelier's principle, when you increase the amount of the reactants, the reaction will be moved to the products, this is because, the most reactants we have the most products we can produce.

From the given choices, the one that goes according to this reason is the third one: The volume of water vapor increases.

6 0

1 year ago

What is the percent composition of hydrogen in vinegar (CH3COOH)?

barxatty [35]

Answer:

%H = 6.72 %

Explanation:

Percent composition of an element is the total mass of that element divided by the molecular mass of compound (or molecular mass) of which it is present in.

So,

Percent composition of Hydrogen will be given as,

%H = Total mass of H / Molecular Mass of Acetic Acid × 100

So,

Total Mass of H = 1.01 × 4 = 4.04 g

Molecular Mass of Acetic acid = 60.052 g/mol

Putting values in above formula,

%H = 4.04 g/mol ÷ 60.052 g/mol × 100

%H = 6.72 %

6 0

3 years ago

If the mass of the products of a chemical reaction was 100 g, what was

Rzqust [24]

If the mass of all of the products in a chemical reaction is equal to 100g then the mass of the reactants in that same reaction had to have had a mass of 100g this is due to the law of conservation of matter stating matter cannot be created or destroyed in a chemical reaction.

4 0

3 years ago

1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure.

Arada [10]

Answer:

Explanation:

Given that:

number of moles of super cooled liquid water = 1

Melting enthalpy of ice = 6020 J/mol

Freezing point =0 °C = (0 + 273 K)= 273 K

The decrease in entropy of the system during freezing for 1 mol (i.e during transformation from liquid water to solid ice ) = - 6020 J/mol × 1 mol /273 K = -22.051 J/K

Entropy change during further cooling from 0 °C (273 K) to -10 °C (263 K)

$\Delta \ S = \int\limits^{T_2}_{T_1}\dfrac{nC_p(s)dT}{T}$

$\Delta \ S = {nC_p(s)In \dfrac{T_2}{T_1}$

$\Delta \ S = {(1*37.7)In \dfrac{263}{273}$

Δ S = -1.4 J/K

Total entropy change of the system = - 22.05 J/K - 1.4 J/K = - 23.45 J/K

Entropy change of universe = entropy change of the system+ entropy change of the surrounding

According to the second law of thermodynamics

Entropy change of universe >0

SO,

Entropy change of the system + entropy change in the surrounding > 0

Entropy change in the surrounding > - entropy change of the system

Entropy change in the surrounding > - (- 23.53 J/K)

Entropy change in the surrounding > 23.53 J/K

b) Make some comments on entropy changes from the obtained data.

From the data obtained; we will realize that the entropy of the system decreases as cooling takes place when water is be convert to ice , randomness of these molecules reduces and as cooling proceeds , hence, entropy reduces more as well and the liberated heat will go into the surrounding due to this entropy of the surrounding increasing.

4 0

3 years ago

A graph of 1/[A]t vs. time will give you a straight line if the reaction is which order?

castortr0y [4]

The answer is: "second order" .
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5 0

3 years ago