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3 years ago

C3H8+5O2 →3CO2+4H20,

Chemistry

1 answer:

Dafna1 [17]3 years ago

8 0

Answer:

6.63 grams of CO₂ can be produced.

Explanation:

1 mol of C₃H₈ reacts to 5 moles of oxygen, in a combustion reaction in order to produce 3 moles of carbon dioxide and 4 moles of water.

First of all, we need to know, the limiting reactant:

5.52 g . 1mol / 44g = 0.125 moles of C₃H₈

8.03 g . 1mol/ 32g = 0.251 moles of oxygen.

1 mol of C₃H₈ can react to 5 moles of O₂

Then, 0.125 moles, must react to (0.125 . 5) /1 = 0.625 moles.

We only have 0.251 moles of O₂ and we need 0.625 moles. Cause we do not have enough oxygen, that's the limiting reagent.

5 moles of oxygen can produce 3 moles of CO₂

0.251 moles may produce (0.251 . 3) /5 = 0.1506 moles.

We convert the moles to mass : 0.1506 mol . 44g /mol = 6.63 g

Reaction is: C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

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What volume of carbon dioxide, at 1 atm pressure and 112°C, will be produced when 80.0 grams of methane is burned?

Vadim26 [7]

Answer:

158 L.

Explanation:

What is given?

Pressure (P) = 1 atm.

Temperature (T) = 112 °C + 273 = 385 K.

Mass of methane CH4 (g) = 80.0 g.

Molar mass of methane CH4 = 16 g/mol.

R constant = 0.0821 L*atm/mol*K.

What do we need? Volume (V).

Step-by-step solution:

To solve this problem, we have to use ideal gas law: the ideal gas law is a single equation which relates the pressure, volume, temperature, and number of moles of an ideal gas. The formula is:

$PV=nRT.$

Where P is pressure, V is volume, n is the number of moles, R is the constant and T is temperature.

So, let's find the number of moles that are in 80.0 g of methane using its molar mass. This conversion is:

$80.0g\text{ CH}_4\cdot\frac{1\text{ mol CH}_4}{16\text{ g CH}_4}=5\text{ moles CH}_4.$

So, in this case, n=5.

Now, let's solve for 'V' and replace the given values in the ideal gas law equation:

$V=\frac{nRT}{P}=\frac{5\text{ moles }\cdot0.0821\frac{L\cdot atm}{mol\cdot K}\cdot385K}{1\text{ atm}}=158.04\text{ L}\approx158\text{ L.}$

The volume would be 158 L.

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1 year ago

think about putting a glass of water on the counter, in the freezer, and on a hot stove how does the temperature of the water af

Shtirlitz [24]

The kinetic energy and the physical state of water depend strongly on the temperature;

Firstly, The kinetic energy of water on a hot stove is higher than that on the counter in the freezer; that the kinetic energy is directly proportional to the temperature according to the relation: $K = \frac{3RT}{2NA}$ ; where R is the universal gas constant, T is the temperature and NA is Avogadro number.

As the temperature increases, the speed of colliding molecules increases and the kinetic energy increases.

Secondly, The physical state of water depends on the temperature; water has three states (gas, liquid and solid) depends on the temperature.
If a glass of water is putt on the counter in the freezer, it will be converted to the solid state (ice).
And, as if it is putt on a hot stove, it will be vapor (gaseous state).

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3 years ago

How many grams of CaF2 would be needed to produce 1.12 moles of F2?

zlopas [31]

Step 1 : Write balanced chemical equation.

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