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4 years ago

Please help me! This is too hard!?

Chemistry

1 answer:

Annette [7]4 years ago

5 0

Answer: 59.24 atm

Explanation:

Given that:

Original Volume of gas V1 = 2.7L

Temperature T1 = 42.7°C

Convert Celsius to Kelvin

(42.7°C + 273 = 315.7K)

Pressure P1 = 684.9 torr

Final Volume V2 = 0.14 L

Final temperature T2 = 803.1°C

Convert Celsius to Kelvin

(803.1°C + 273 = 1076.1K)

Final pressure = ?

Then, apply the combined gas equation

(P1V1)/T1 = (P2V2)/T2

(684.9 torr x 2.7L)/315.7K = (P2 x 0.14L)/1076.1K

1849.23/315.7 = 0.14P2/1076.1

Then, cross multiply

1849.23 x 1076.1 = 315.7 x 0.14P2

1989956.403 = 44.198P2

Divide both sides by 44.198

1989956.403/44.198 = 44.198P2/44.198

45023.67 torr = P2

Now, convert the pressure in torr to atmosphere

If 760 torr = 1 atm

45023.67 torr = Z atm

Then, cross multiply

760 torr x Z = 45023.67 torr x 1 atm

Z = 45023.67 torr / 760 torr

Z = 59.24 atm

Thus, the new pressure of the gas will be 59.24 atm

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26.833 liters

Aluminum oxide has a formula of Al₂O₃, which means for every mole of aluminum used, 1.5 moles of oxygen is required (3/2 = 1.5).

Given 42.5 g of aluminum divided by its atomic mass (26.9815385) gives 1.575 moles of aluminum.

Since it takes 1.5 moles of oxygen per mole of aluminum to make aluminum oxide, you'll need 2.363 moles of oxygen atoms.

Each molecule of oxygen gas has 2 oxygen atoms, so the moles of oxygen gas will be 2.363/2 = 1.1815

Finally, you need to calculate the volume of 1.1815 moles of oxygen gas.
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3 years ago

Calculate the atomic mass of Carbon if the two common isotopes of carbon have masses of

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Answer:

Average atomic mass of carbon = 12.01 amu.

Explanation:

Given data:

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Average atomic mass = ?

Solution:

Average atomic mass of carbon = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass) / 100

Average atomic mass of carbon = (12.000×98.89)+(13.003×1.11) /100

Average atomic mass of carbon= 1186.68 + 14.43333 / 100

Average atomic mass of carbon = 1201.11333 / 100

Average atomic mass of carbon = 12.01 amu.

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3 years ago

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2 years ago

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3 years ago

The burning of magnesium is a highly exothermic reaction. How many kilojoules of heat are released when 0. 75 mol of Mg burn in

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Taking into account the definition of enthalpy of a chemical reaction, the quantity of heat released when 0.75 moles of Mg are burned is 451.5 kJ.

<h3>Enthalpy of a chemical reaction</h3>

The enthalpy of a chemical reaction is known as the heat absorbed or released in a chemical reaction when it occurs at constant pressure. That is, the heat of reaction is the energy that is released or absorbed when chemicals are transformed into a chemical reaction.

The enthalpy is an extensive property, that is, it depends on the amount of matter present.

<h3>Heat released in this case</h3>

In this case, the balanced reaction is:

2 Mg(s) + O₂ (g) → 2 MgO(s) + 1204 kJ

This equation indicates that when 2 moles of Mg reacts with 1 mole of O₂, 1204 kJ of heat is released.

When 0.75 moles of Mg are burned, then you can apply the following rule of three: if 2 moles of Mg releases 1204 kJ of heat, 0.75 moles of Mg releases how much heat?

$heat=\frac{0.75 moles of Mgx1204 kJ}{2 moles of Mg}$

heat= 451.5 kJ

Finally, the quantity of heat released when 0.75 moles of Mg are burned is 451.5 kJ.

Learn more about enthalpy of a chemical reaction:

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