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2 years ago

A discarded spray paint can contains only a small volume of the propellant gas at a

Chemistry

1 answer:

Katena32 [7]2 years ago

5 0

Answer:

1.24 × 10³ kPa

Explanation:

Step 1: Given data

Initial pressure of the gas (P₁): 34.5 kPa

Initial volume of the can (V₁): 473 mL

Final pressure of the gas (P₂): ?

Final volume of the can (V₂): 13.16 mL

Step 2: Calculate the final pressure of the gas in the can

If we assume that the gas in the can behaves as an ideal gas and that the temperature remains constant, we can calculate the final pressure of the gas using Boyle's law.

P₁ × V₁ = P₂ × V₂

P₂ = P₁ × V₁ / V₂

P₂ = 34.5 kPa × 473 mL / 13.16 mL = 1.24 × 10³ kPa

You might be interested in

Which aqueous solution has the lowest freezing point c6h12o6, c2h5oh, ch3cooh, or nacl?

Eddi Din [679]

Depression of a freezing point of the solutions depends on the number of particles of the solute in the solution.
1 mol of C6H12O6 after dissolving in water still be 1 mol, because C6H12O6 does no dissociate in water.
1 mol of C2H5OH after dissolving in water still be 1 mol, because C2H5OH does no dissociate in water.
1 mol of NaCl after dissolving in water gives 2 mol of particles (ions), because NaCl is a strong electrolyte(as salt) and completely dissociates in water.
NaCl ----->Na⁺ + Cl⁻
1 mol of CH3COOH after dissolving in water gives more than 1 mol but less than 2 moles, because CH3COOH is a weak electrolyte (weak acid) and dissociates only partially.

So, most particles of the solute is going to be in the solution of NaCl,
so the lowest freezing point has the aqueous solution of NaCl.

3 0

3 years ago

Sucrose is very soluble in water. at 25◦c, 211.4 grams of sucrose will dissolve in 100 g of water. given that the density of the

stiv31 [10]

Molarity of solution is mathematically expressed as,
M = $\frac{x\text{weight of solute(g)}}{\text{Molecular weight X Volume of solution(l)}}$

We know that volume = mass/density
Given: mass of solution = 100 g, Density = 1.34 g/ml
∴ volume = 100/1.34 = 88.49 ml = 0.08849 l

Also, we know that molecular weight of sucrose = 342.3 g/mol
∴M = $\frac{x\text{211.4}}{\text{342.3 X 0.08849}}$
= 6.979 M

Thus, molarity of solution is 6.979 M

8 0

2 years ago

Elements occur in a number of isotopic forms. In this problem, you will learn about the notation used to distinguish different i

alina1380 [7]

Answer:

Number of protons, Z = 14
Number of neutrons, N = 14

Explanation:

1) About isotopes:

Isotopes are different kind of atoms of the same element. Hence, they have the atomic number (Z), which is the number of protons, the same number of electrons (talking about to neutral atoms, not ions), and different number of neutrons N).

This is, it is the number of neutrons what distinguish different isotopes of an element.

2) About the notation used to distinguish different isotopes:

A superscript and a subscript, both to the left of the chemical symbol of the element, are used to distinguish different isotopes:

A ←------------- This superscript tells the mass number of the isotope

X ←--------- This is the chemical symbol of the element

Z ←-------------- This subscript is the atomic number of isotope

In our case, the notiation for the isotope of silicon is: ²⁸₁₄ Si

So, we have:

28 is the mass number (A)
14 is the atomic number (Z)
Si is the chemical symbol.

Now, you can answer the questions of the part A:

Number of protons: Z = 14

Number of neutrons N:

mass number = number of protons + number of neutrons

A = Z + N

⇒ N = A - Z = 28 - 14 = 14

In conclusion:

Number of protons, Z = 14
Number of neutrons, N = 14

5 0

3 years ago

The temperature of 6.24 L of a gas is increased from 25.0°C to 55.0°C at constant pressure. The new volume of the gas is Questio

Sphinxa [80]

Answer:

Heating this gas to 55 °C will raise its volume to 6.87 liters.

Assumption: this gas is ideal.

Explanation:

By Charles's Law, under constant pressure the volume $V$ of an ideal gas is proportional to its absolute temperature $T$ (the one in degrees Kelvins.)

Alternatively, consider the ideal gas law:

$\displaystyle V = \frac{n \cdot R}{P}\cdot T$ .

$n$ is the number of moles of particles in this gas. $n$ should be constant as long as the container does not leak.
$R$ is the ideal gas constant.
$P$ is the pressure on the gas. The question states that the pressure on this gas is constant.

Therefore the volume of the gas is proportional to its absolute temperature.

Either way,

$V\propto T$ .

$\displaystyle V_2 = V_1\cdot \frac{T_2}{T_1}$ .

For the gas in this question:

Initial volume: $V_1 = \rm 6.24\; L$ .

Convert the two temperatures to degrees Kelvins:

Initial temperature: $T_1 = \rm 25.0\;\textdegree{C} = (25.0 + {\rm 273.15})\; K = 298.15\;K$ .
Final temperature: $T_1 = \rm 55.0\;\textdegree{C} = (55.0 + {\rm 273.15})\; K = 328.15\;K$ .