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2 years ago

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A family leaves for summer vacation by driving on the highway. The car's tires start the trip with a pressure of 3.8atm at a tem

perature of 19oC and a volume of 1.7L. What is the pressure of the tires after driving, when the temperature within the tire increases to 105oC?

1 answer:

goldenfox [79]2 years ago

4 0

Answer: The pressure of the tires after driving is 4.9atm

Explanation: Please see the attachments below

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Give two examples (i.e. list 2 elements that are examples) of: a. an atom with a half-filled subshell b. an atom with a complete

elena55 [62]

Answer:

an atom with a half-filled subshell - hydrogen

an atom with a completely filled outer shell - argon

an atom with its outer electrons occupying a half-filled subshell and a filled subshell- copper

Explanation:

The outermost shell or the valence shell of the atom is the last shell in the atom. Chemical reactions occur at this outer most shell. The number of electrons on the outermost shell of an atom determines the group to which it belongs in the periodic table as well as its chemical properties.

Hydrogen has a half filled 1s sublevel. Only one electron is present in this sublevel.

Let us consider argon

1s2 2s2 2p6 3s2 3p6

The outermost ns and np levels are completely filled. Thus the outermost shell is completely filled.

In the last case; let us look at the electronic configuration of nitrogen;

1s2 2s2 2p3

The outermost 2p subshell is exactly half filled while the 2s sublevel is fully filled. The outermost shell of nitrogen is made up of 2s2 and 2p3 sublevels.

4 0

2 years ago

The solubility of acetanilide is 12.8 g in 100 mL of ethanol at 0 ∘C, and 46.4 g in 100 mL of ethanol at 60 ∘C. What is the maxi

weqwewe [10]

Answer: 72.41% and 26.90% respectively.

Explanation:

At 60°C, you can dissolve 46.4g of acetanilide in 100mL of ethanol. If you lower the temperature, at 0°C, you can dissolve just 12.8g, which means (46.4g-12.8g)=33.6g of acetanilide must have precipitated from the solution.

We can calculate recovery as:

$\%R=\frac{crystalized\ mass}{initial\ mass}*100 =\frac{33.6\ g}{46.4\ g}*100=72.41\%$

So the answer to the first question is 72.41%.

For the second part just use the same formula, the mass of the precipitate is the final mass minus the initial mass, (171mg-125mg)=46mg.

$\%R=\frac{crystalized\ mass}{initial\ mass}*100 =\frac{46\ mg}{171\ mg}*100=26.90\%$

So the answer to the second question is 26.90%.

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2 years ago

A reaction produces a gas, which is collected in a glass cylinder. When a glowing splint is placed inside the container, it burn

Gnesinka [82]

Answer:

true

Explanation:

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2 years ago

The pH of an acidic solution is 2.11. What is [H⁺]

BartSMP [9]

Answer:

denotes the molar hydrogen ion concentration

Explanation:

3 0

2 years ago

Read 2 more answers

In Part B the given conditions were 1.00 mol of argon in a 0.500-L container at 27.0 ∘C . You identified that the ideal pressure

dimaraw [331]

Answer : The percent difference between the ideal and real gas is, 4.06 %.

Explanation : Given,

Ideal pressure (true value) = 49.3 atm

Real pressure (measured value) = 47.3 atm

The formula used to calculate percent difference is :

Percent difference = $\frac{\text{True value - Measured value}}{\text{True value}} \times 100$

Percent difference = $\frac{(49.3- 47.3)atm}{49.3atm}\times 100$

Percent difference = 4.06 %

Therefore, the percent difference between the ideal and real gas is, 4.06 %.

4 0

2 years ago