Consider this equilibrium:N2(g) + 3H2(g) 2NH3(g) + energy.

Certain conditions provide less than 10% yield of NH3 at equilibrium. Which statement describes this equilibrium?

Answers

Answer 1

Answer: This is the complete answer, including the set of answer choices:

Certain conditions provide less than 10% yield of NH3 at equilibrium. Which statement describes this equilibrium?

A. The Keq is large and products are favored.
B. The Keq is small and products are favored.
C. The Keq is large and reactants are favored.
D. The Keqis small and reactants are favored.
E. The conditions of the reaction must be known to answer the question

To answer you must know that the equilibrium yield is the quantity of product obtained.

In this case it is 10% of NH3.

That means that the equilibrium is more favorable to the reactants.

Given that Ke relates the concentration of products / concentration of reactants, the answer is the Ke is small and reactants are favored

Answer 2

Answer:

Final answer:

This equilibrium has a low yield of NH3 and can be improved by adjusting the conditions and using the principles of Le Chatelier.

Explanation:

This equilibrium can be described as an equilibrium with a low yield of NH3. The fact that less than 10% yield of NH3 is obtained suggests that the forward reaction (N2(g) + 3H2(g) -> 2NH3(g) + energy) is not favored under the given conditions. To increase the yield of NH3, the conditions can be adjusted to shift the equilibrium towards the product side.

The Le Chatelier's principle can be applied to achieve a higher yield of NH3. One possible way is to increase the concentration of the reactants (N2 and H2) or decrease the concentration of the product (NH3). Another way is to increase the temperature, as this reaction is exothermic. By increasing the temperature, the equilibrium will shift in the reverse direction to consume the excess energy.

In summary, this equilibrium is characterized by a low yield of NH3, which can be improved by adjusting the conditions and using the principles of Le Chatelier.

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Which two factors must be equal when a chemical reaction reaches equilibrium?(1) the concentration of the reactants and the concentration of the products
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Answers

The correct answer is option 3. Equilibrium is achieved in a chemical reaction when the rate of the forward reaction is the same for the rate of the backward reaction and when the reaction has stopped.

A substance that can be separated into two or more substances only by a chemical change is

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A substance that can be separated into two or more substances only by a chemical change is known as a heterogeneous mixture

At STP, which 2.0-gram sample of matter uniformly fills a 340-milliliter closed container?

Answers

Answer;

D, Xe (g)

Solution and explanation;

If 2g has a volume of 340ml.

Density is 1000/340*2 = 5.88g/litre.

-This rules out the two solids, choices 2) &3)

If 1 litre has mass 5.88g,

then 22.4 liters (volume at STP) has mass 5.88*22.4 = 131.8g/mol

molar mass Br2 = 80*2 = 160g/mol NO

molar mass Xe = 131.3g/mol = YES.

Answer is Xe

Final answer:

To determine the matter filling a closed container at STP given a 2.0 gram sample, you can use the ideal gas law equation to find the number of moles. Then, divide the number of moles by the volume and the gas constant to solve for the pressure. Compare the pressure obtained to known substances' vapor pressures at STP to identify the matter.

Explanation:

The question is asking for the specific type of matter that would uniformly fill a 340-milliliter, closed container at STP (Standard Temperature and Pressure) when given a 2.0-gram sample. To determine the matter, we can use the ideal gas law equation, PV = nRT, and rearrange it to solve for n, the number of moles. Then, we can use the molar mass of the substance to find its identity.

First, convert the volume from milliliters to liters by dividing it by 1000: 340 mL ÷ 1000 = 0.34 L. Next, convert the mass from grams to moles using the molar mass of the substance:

1.(Conversion factor) Given: 2.0 g sample, 1 mole = molar mass

2.(Calculation) Moles of substance = 2.0 g ÷ molar mass

Once you have the number of moles, divide it by the volume (in liters) and the universal gas constant (0.0821 L·atm/mol·K) and solve for the pressure:

1.(Ideal Gas Law) PV = nRT

2.(Substitution) P × 0.34 L = n × 0.0821 L·atm/mol·K

3.(Isolation) P = (n × 0.0821 L·atm/mol·K) ÷ 0.34 L

After solving for the pressure, compare it to known substances' vapor pressures at STP to determine the identity of the matter in the container.

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What would be the best way to measure Carbon Dioxide in a Soft Drink can?And yes, we were going to do it by taste.

Answers

Read the nutritional facts which says what percent of CO2 there is. If the serving size is there, the calculate accordingly

I sort of know how carbonated beverages are carbonated: a lot of CO2CO2 gets pushed into the liquid, and the container is sealed. There are at least two things I don't know. First, how much carbon dioxide is actually dissolved in the liquid? Second, what is the resulitng partial pressure of CO2CO2 in the headspace and the total pressure in the headspace? I'm interested in cans, plastic bottles, and glass bottles. I know from experience that there is some variation among manufacturers even for the same beverage, so I will be happy with general numbers or a good estimate.

Plants and animals interact with organic molecules differently. Explain how.

Answers

Answer:

All animals, all fungi, and some kinds of bacteria are heterotrophs and consumers

Explanation:

Which quantity represents 0.500 Mole at STP

Answers

0.500 moles is roughly .5*6.022*10^23=3.011*10^23 atoms. This is independent of STP.

Final answer:

0.500 mole of any gas at standard temperature and pressure (STP) is equivalent to 11.2 liters. This is calculated using Avogadro's Law.

Explanation:

The quantity that represents 0.500 Mole at Standard Temperature and Pressure (STP) refers to the volume of gas. According to Avogadro's law, which states that equal volumes of gases at the same temperature and pressure contain an equal number of molecules, 1 mole of any gas at STP occupies a volume of 22.4 liters. Therefore, 0.500 mole of a gas at STP would occupy a volume of 11.2 liters.

Here's how you calculate this: Use Avogadro's law proportion, which is V1/n1 = V2/n2. Given n1 is 1 mole, V1 is 22.4 liters (which are standard values at STP) and n2 is 0.500 mole (your desired quantity), you can solve for V2 :

V2 = V1 * n2 / n1 = 22.4 L * 0.500 mol / 1 mol = 11.2 L.

So, 0.500 mole of any gas at STP would have a volume of 11.2 liters.