A weather balloon has a volume of 200.0 L at a pressure of 760 mm Hg. As it rises, the pressure decreases to 282 mm Hg. What is the new volume of the balloon? (Assume constant temperature)

Answers

Answer 1

Answer:

Answer:

The new volume of the balloon is 539 L

Explanation:

As the volume increases, the gas particles (atoms or molecules) take longer to reach the walls of the container and therefore collide less times per unit time against them. This means that the pressure will be less because it represents the frequency of gas strikes against the walls. In this way, pressure and volume are related, determining Boyle's law that says:

"The volume occupied by a given gas mass at constant temperature is inversely proportional to the pressure"

Boyle's law is expressed mathematically as:

Pressure * Volume = constant

o P * V = k

Having an initial state 1 and an final state 2 will be fulfilled:

P1 * V1 = P2 * V2

So, in this case, you know:

P1= 760 mmHg
V1= 200 L
P2= 282 mmHg
V2= ?

Replacing:

760 mmHg*200 L= 282 mmHg*V2

Solving:

$V2=(760 mmHg*200 L)/(282 mmHg)$

V2=539 L

The new volume of the balloon is 539 L

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Aqueous hydrochloric acid HCl will react with solid sodium hydroxide NaOH to produce aqueous sodium chloride NaCl and liquid water H2O. Suppose 9.84 g of hydrochloric acid is mixed with 3.1 g of sodium hydroxide. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits.

Answers

Answer:

1.4 g H₂O

Explanation:

In a reaction, the reactants are usually not present in exactstoichiometric amounts, that is, in the proportions indicated by the balanced equation. Frequently a large excess of one reactant is supplied to ensure that the more expensive reactant is completely converted to the desired product. Consequently, some reactant will be left over at the end of the reaction. The reactant used up first in a reaction is called the limiting reagent, because the maximum amount of product formed depends on how much of this reactant was originally present. When this reactant is used up, no more product can be formed.

Which of the following solutions would make a good buffer system? (Check all that apply.) A. A solution that is 0.10 M NH3 and 0.10 M NH4Cl B. A solution that is 0.10 M HCN and 0.10 M NaF C. A solution that is 0.10 M HCN and 0.10 M LiCN D. A solution that is 0.10 M HF and 0.10 M NaF

Answers

Answer:

A solution that is 0.10 M HCN and 0.10 M LiCN

. A solution that is 0.10 M NH3 and 0.10 M NH4Cl

Explanation:

A buffer consists of a weak acid and its conjugate base counterpart. HCN is a weak acid and the salt LiCN contains its counterpart conjugate base which is the cyanide ion. A buffer maintains the pH by guarding against changes in acidity or alkalinity of the solution.

A solution of ammonium chloride and ammonia will also act as a basic buffer. A buffer may also contain a weak base and its conjugate acid.

Answer:

Good buffer systems are:

A) NH3 + NH4Cl

C) HCN + LiCN

D) HF + NaF

Explanation:

Buffers consist in a mixture of a weak acid with its salt or a weak alkaly with its salt. All buffer systems are conformed by:

1) Weak acid + salt

2) Weak alkaly + salt

It is very important these salts come from the weak acid or weak alkaly. It means, the anion of the acid must be the anion in the salt which is going to be part of the buffer system. On the other hand, the cation of the weak alkaly must be the cation of the salt which is going to form the salt in the buffer system.

Then, when we evaluate all options in this exercise, answers are the following:

A) 0.10 M NH3 and 0.10 M NH4Cl. It is a buffer because NH3 (ammonia) is a weak alkaly and NH4Cl is a salt coming from NH3.

Buffer component reactions:

Reaction weak alkaly: NH3 + H2O <-----> NH4+ + OH-

Reaction salt in water: NH4Cl ---> NH4+ + Cl-

NH4+ is the cation of the weak alkaly so it must be part of the salt in the buffer system. Then NH4Cl is a salt from NH3.

C) 0.10 M HCN and 0.10 M LiCN. It is a buffer because HCN is a weak acid and LiCN is a salt which is coming from HCN.

Buffer component reactions:

Reaction weak acid: HCN + H2O <-----> H3O+ + CN-

Reaction salt in water: LiCN --> Li+ + CN-

CN- is the anion of the acid, so it must be part of the salt in the buffer system. Then LiCN is a salt from HCN.

D) 0.10 M HF and 0.10 M NaF. It is a buffer because HF is a weak acid and NaF is a salt which is coming from HF.

Buffer component reactions:

Reaction weak acid: HF + H2O <------> H3O+ + F-

Reaction salt in water: NaF ---> Na+ + F-

F- is the anion of the weak acid (HF), so it must be part of the salt in th buffer systema. Then NaF is a salt coming from HF.

However option B, it is not a buffer, because it is a mixture of 0.10 M HCN and 0.10 M NaF. Salt is not coming from the weak acid.

Reaction weak acid: HCN + H2O <-----> H3O+ + CN- (anion of the acid is CN-)

Rection salt in water: NaF --> Na+ + F- (anion in the salt is F-, not CN-)

Anion of the acid is CN- and the anion in the salt is F- so it is not a salt coming from the weak acid. Then option B it is not a buffer system.

5.0 liters of a gas are at an initial pressure of 5.0 atmospheres. If the temperature and amount of a gas are kept constant, what is the new volume of the gas when pressure is increased to 7.0 atmospheres?

Answers

Final answer:

Using Boyle's Law of gases which states that the pressure and volume of a gas have an inverse relationship when temperature is kept constant, we find that when the pressure of the gas increases from 5.0 to 7.0 atmospheres, the volume of the gas decreases to approximately 3.57 liters.

Explanation:

The question pertains to the application of Boyle's Law, a fundamental concept in the field of physics dealing with gases. Boyle's Law states that the pressure and volume of a gas have an inverse relationship when the temperature is held constant. This means if the pressure of a gas increases, the volume decreases, and vice versa.

In this case, you have 5.0 liters of a gas under an initial pressure of 5.0 atmospheres. The pressure is then increased to 7.0 atmospheres, and you are asked to determine the new volume of the gas. To solve this problem, we use the formula for Boyle's Law, which is P1V1 = P2V2. We know P1 (initial pressure) is 5.0 atmospheres and V1 (initial volume) is 5.0 liters. P2 (final pressure) is increased to 7.0 atmospheres and V2 (final volume) is what we are trying to find.

So, we plug the numbers into the equation and get: 5.0 atmospheres * 5.0 liters = 7.0 atmospheres * V2. Solving for V2, we find V2 to be approximately 3.57 liters. Therefore, when the pressure of the gas is increased from 5.0 atmospheres to 7.0 atmospheres, the volume decreases to around 3.57 liters, while the temperature remains constant.

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Refer to the example about diatomic gases A and B in the text to do problems 20-28.It was determined that 1 mole of B2 is needed to react with 3 moles of A2.
How many grams in one mole of B2?
__g

Answers

Final answer:

The number of grams in one mole of B2 can be calculated using the atomic mass of element B. This is found on the periodic table and then doubled for B2 since it's diatomic. If B is Oxygen for instance, 1 mole of B2 (O2) weighs 32 grams.

Explanation:

To find the number of grams in one mole of B2, we need to know the atomic mass of element B, which isn't provided in your question. However, you can find this information on the periodic table. Once you have the atomic mass of B, you can calculate the molar mass of B2 (which is two times the atomic mass of B) since 1 mole of a substance corresponds to its molar mass in grams.

For example, if element B is Oxygen (O), its atomic mass is approximately 16 g/mol. Therefore, the molar mass of B2 (O2 in this case) would be 32 g/mol. Hence, 1 mole of B2 (or O2) would weigh 32 grams.

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What mass of CO2 (in kilograms) does the combustion of a 16-gallon tank of gasoline release into the atmosphere? Assume the gasoline is pure octane (C8H18) and that it has a density of 0.70 g/mL.Express your answer in kilograms to two significant figures.

Answers

Mass of CO₂ = 1.3 x 10⁵ kg

Further explanation

A reaction coefficient is a number in the chemical formula of a substance involved in the reaction equation. The reaction coefficient is useful for equalizing reagents and products.

Reaction

2C₈H₁₈ + 25O₂⇒ 16CO₂ + 18H₂O

16 gallon = 60566,6 ml