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1 year ago

What volume of air contains 10.0g of oxygen gas at 273 k and 1.00 atm?

Chemistry

2 answers:

pashok25 [27]1 year ago

8 0

<u>Answer:</u> The volume of air will be 7.00 L

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of oxygen gas = 10.0 g

Molar mass of oxygen gas = 32 g/mol

Putting values in above equation, we get:

$\text{Moles of oxygen gas}=\frac{10.0g}{32g/mol}=0.3125mol$

To calculate the volume of gas, we use the equation given by ideal gas that follows:

$PV=nRT$

where,

P = pressure of the gas = 1.00 atm

V = Volume of the gas = ?

T = Temperature of the gas = 273 K

R = Gas constant = $0.0821\text{ L. atm }mol^{-1}K^{-1}$

n = number of moles of gas = 003125 mol

Putting values in above equation, we get:

$1.00atm\times V=0.3125mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 273K\\\\V=\frac{0.3125\times 0.0821\times 273}{1.00}=7.00Ll$

Hence, the volume of air will be 7.00 L

VARVARA [1.3K]1 year ago

7 0

12.3g 02times1 mol 02/32.0 g 02=mol 02
.38mol/x=20.95/100
x=1.8mol air...

PV=nRT

101.3kPa times V =1.8 mol times 8.31[kPa *L]/{k*mol}*273k
V=40.3Lair

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Answer:

The pH of the solution is 8.

Explanation:

To which options are correct, let us determine the concentration of the hydroxide ion, [OH-] and the pH of the solution. This is illustrated below:

1. The concentration of the hydroxide ion, [OH-] can be obtained as follow:

pOH = –Log [OH-]

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–6 = Log [OH-]

[OH-] = Antilog (–6)

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2. The pH of the solution can be obtained as follow:

pH + pOH = 14

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From the calculations made above,

[OH-] = 1x10^–6 mol/L

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Therefore, the correct answer is:

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1 year ago

The gas in a sealed container has an absolute pressure of 125.4 kilopascals. If the air around the container is at a pressure of

AlexFokin [52]

Answer: C. 25.6 kPa

Explanation:

The Gauge pressure is defined as the amount of pressure in a fluid that exceeds the amount of pressure in the atmosphere.

As such, the formula will be,

PG = PT – PA

Where,

PG is Gauge Pressure

PT is Absolute Pressure

PA is Atmospheric Pressure

Inputted in the formula,

PG = 125.4 - 99.8

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The gauge pressure inside the container is 25.6kPa which is option C.

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2 years ago

A student has two samples of NaCl, each one from a different source. Assume that the only potential contaminant in each sample i

bija089 [108]

Answer:

The correct option is;

A. Which sample has the higher purity

Explanation:

The information given relate to the presence of two samples of NaCl, from different sources

The only potential contaminant in each of the sources = KCl

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The molar mass of NaCl = 58.44 g/mol

The molar mass of KCl = 74.5513 g/mol

Let the number of moles of KCl in the sample = X

For a given mass of NaCl, KCl mixture, we have;

The molar mass of potassium = 39.0983 g/mol

The molar mass of chlorine = 35.453 g/mol

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Therefore;

Each mole of KCl, will yield 35.453 g/mol per 74.5513 g/mol of KCl

While each mole of NaCl will yield 35.453 g/mol per 58.44 g/mol of NaCl

Therefore, the pure sodium chloride sample will yield more chlorine per unit mass of sample.

As such if the two samples have the same mass, the sample with the contaminant of KCl will yield less mass of chlorine per unit mass of the sample, from which the student will be able to tell the purity of the solution.

The sample with the higher purity will yield a higher mass chlorine per unit mass of the sample.

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2 years ago

2N2H4(l) + N2O4(l) → 3N2(g) + 4H2O(g) [balanced] How many moles of N2H4 is required to produce 28.3 g of N2? Assume that all rea

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Answer: 0.67 moles of $N_2H_4$

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To calculate the moles, we use the equation:

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According to stoichiometry:

3 moles of $N_2$ is produced by 2 moles of $N_2H_4$

Thus 1 mole of $N_2$ is produced by= $\frac{2}{3}\times 1=0.67moles$ of $N_2H_4$

Thus 0.67 moles of $N_2H_4$ are required to produce 28.3 g of $N_2$

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2 years ago

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Rina8888 [55]

Answer:

The equation for the rate of this reaction is R = [NO] + {O2}

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The rate-determining step of a reaction is the slowest step of a chemical reaction which determines the rate (speed) at which the overall reaction would take place.

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2 years ago