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Georgia [21]
3 years ago
14

A container is filled to a volume of 55.2 L at 61 °C. While keeping the

Chemistry
2 answers:
mel-nik [20]3 years ago
7 0

Answer:

\boxed {\boxed {\sf 4.45 \ atmospheres}}

Explanation:

We are asked to find the pressure given a change in volume. The temperature remains constant, so we are only concerned with volume and pressure. We will use Boyle's Law, which states the volume of a gas is inversely proportional to the pressure. The formula for this law is:

P_1 V_1= P_2V_2

The initial pressure is unknown, but the volume starts at 55.2 liters.

P_1 * 55.2 \ L = P_2V_2

The volume is reduced to 28.8 liters and the pressure is 8.53 atmospheres.

P_1 * 55.2 \ L = 8.53 \ atm * 28.8 \ L

We are solving for the initial pressure, so we must isolate the variable P₁. It is being multiplied by 55.2 liters. The inverse operation of multiplication is division, so we divide both sides of the equation by 55.2 L.

\frac {P_1 * 55.2 \ L }{55.2 \ L}= \frac{8.53 \ atm * 28.8 \ L}{55.2 \ L}

P_1= \frac{8.53 \ atm * 28.8 \ L}{55.2 \ L}

The units of liters (L) cancel.

P_1= \frac{8.53 \ atm * 28.8 }{55.2}

P_1=\frac{245.664 }{55.2 } \ atm

P_1 = 4.45043478261 \ atm

The original measurements of volume and pressure have 3 significant figures, so our answer must have the same. For the number we calculated, that is the hundredths place. The 0 in the thousandths place tells us to leave the 5.

P_1 \approx 4.45 \ atm

The initial pressure inside the container is approximately <u>4.45 atmospheres.</u>

babymother [125]3 years ago
5 0

Answer:

4.45 atm

Explanation:

Applying,

PV = P'V'............ Equation 1

Where P = Initial pressure of the container, V = Initial volume of the container, P' = Final pressure of the container, V' = Final volume of the container.

make P the subject of the equation

P = P'V'/V........... Equation 2

From the question,

Given: V = 55.2 L, P' = 8.53 atm, V' = 28.8 L

Substitute these values into equation 2

P = (8.53×28.8)/55.2

P = 4.45 atm

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According to the question;

Number of moles of CO2 released = 21.3 g/44 g/mol = 0.48 moles

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VARVARA [1.3K]

Answer:

6

Explanation:

The atomic number for phosphorous is 15, meaning that it has 15 electrons (and protons). The first and second shells would be filled up with 2 and 8 electrons respectively, leaving 5 which goes on the third shell, which is also the valence shell, meaning phosphorous has 5 valence electrons.

Since the atomic number of sulfur is 16, the first and second shells are also filled up with 2 and 8 electrons respectively, leaving 6 to be on the third shell, the valence shell. Hence, sulfur has 6 valence electrons.

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How many moles are in a 12.0 g sample of NiC12
Nady [450]

Answer:

0.17 moles

Explanation:

In the elements of the periodic table, the atomic mass = molar mass. <u>Ex:</u> Atomic mass of Carbon is 12.01 amu which means molar mass of Carbon is also 12.01g/mol.

In order to find the # of moles in a 12 g sample of NiC-12, we will need to multiply the number of each atom by its molar mass and then add the masses of both Nickel and C-12 found in the periodic table:

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  • Molar Mass of C (Carbon): 12.01 g/mol

Since there's just one atom of both Carbon and Nickel, we just add up the masses to find the molar mass of the whole compound of NiC-12.

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There's 12g of NiC-12, which is less than the molar mass of NiC-12, so the number of moles should be less than 1. In order to find the # of moles in NiC-12, we need to do some dimensional analysis:

  • 12g NiC-12 (1 mol of NiC-12/70.7g NiC-12) = 0.17 mol of NiC-12
  • The grams cancel, leaving us with moles of NiC-12, so the answer is 0.17 moles of NiC-12 in a 12 g sample.

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3 years ago
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