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2 years ago

Which of the following statements about subatomic particles best characterizes protons?

1 answer:

3 0

Lets get this straight:-

Protons → Positive charge, found in nucleus, heavy

Now, the only one we see that seems to be correct is A) positive charge, heavy, found in the nucleus of an atom

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3.Using Balanced Equations: C5H12+802–5CO2+6H20

Inessa [10]

Answer:

i think b is the answer hope this helps:))

8 0

2 years ago

Use a reference source to identify five facts about a neutron star or a black hole. Don’t forget to cite your sources.

sleet_krkn [62]

Answer:

Black holes are astronomical objects that have such strong gravity, not even light can escape. Neutron stars are dead stars that are incredibly dense. ... Both objects are cosmological monsters, but black holes are considerably more massive than neutron stars.

Explanation:

3 0

2 years ago

1. How much heat is required to melt 25.0 g of ice at 0°C?

tigry1 [53]

Answer: The heat required to melt 25.0 g of ice at $0^0C$ is 8350 Joules

Explanation:

Heat of Fusion tells us how much energy is needed to convert 1g of a solid to a liquid at the same temperature.

$Q=m\times L$

Q = Heat absorbed = ?

m = mass of ice = 25.0 g

L = Latent heat of fusion of ice = 334 J/g

Putting in the values, we get:

$Q=25.0g\times 334J/g=8350J$

Thus heat required to melt 25.0 g of ice at $0^0C$ is 8350 Joules

8 0

2 years ago

(2 KClO3 (s) → 2 KCl (s) + 3 O2 (g) ) If 165 mL of oxygen is produced at 30.0 °C and 90.0 kPa, what mass of KClO3 was decomposed

soldier1979 [14.2K]

Taking into account the reaction stoichiometry and ideal gas law, 0.48144 grams of KClO₃ was decomposed.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

2 KClO₃ → 2 KCl + 3 O₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

KClO₃: 2 moles
KCl: 2 moles
O₂: 3 moles

The molar mass of the compounds is:

KClO₃: 122.45 g/mole
KCl: 74.45 g/mole
O₂: 32 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

KClO₃: 2 moles ×122.45 g/mole= 244.8 grams
KCl: 2 moles ×74.45 g/mole= 148.9 grams
O₂: 3 moles ×32 g/mole= 96 grams

<h3>Ideal gas law</h3>

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

where:

P is the gas pressure.
V is the volume that the gas occupies.
T is the temperature of the gas.
R is the ideal gas constant. The universal constant of ideal gases R has the same value for all gaseous substances.
n is the number of moles of the gas.

<h3>Number of O₂ produced.</h3>

165 mL of oxygen is produced at 30.0 °C and 90.0 kPa. This is, you know:

P= 90 kPa= 0.888231 atm (being 101.325 kPa= 1 atm)
V= 165 mL= 0.165 L (being 1000 mL= 1 L)
n= ?
R= 0.082 $\frac{atmL}{molK}$
T= 30 C= 303 K (being 0 C= 273 K)

Replacing in the ideal gas law:

0.888231 atm× 0.165 L = n× 0.082 $\frac{atmL}{molK}$ × 303 K

Solving:

n= (0.888231 atm× 0.165 L)÷ (0.082 $\frac{atmL}{molK}$ × 303 K)

<u><em>n= 0.0059 moles</em></u>

Finally, 0.0059 moles of oxygen is produced at 30 °C and 90 kPa.

<h3>Mass of KClO₃ required</h3>

The following rule of three can be applied: If by stoichiometry of the reaction 3 moles of O₂ are produced by 244.8 grams of KClO₃, 0.0059 moles of O₂ are produced by how much mass of KClO₃?

$mass of KClO_{3}= \frac{0.0059 moles of O_{2}x 244.8 grams of KClO_{3}}{3 moles of O_{2}}$