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2 years ago

If a sample containing 2.50 ml of nitroglycerin (density=1.592g/ml) is detonated, how many total moles of gas are produced?

1 answer:

5 0

Density = mass / volume
mass of nitroglycerin = density x volume = 1.592 x 2.5 = 3.98 grams
molar mass of nitroglycerin = 3(12) + 5(1) + 3(14) + 9(16) = 227 grams
number of moles reacting = mass / molar mass = 3.98/227 = 0.017 moles

The balanced chemical equation for this reaction is as follows:
4C3H5N3O9 ..............> 12CO2(g) + 6N2(g) + O2(g) + 10H2O(g)

From the balanced equation:
4 moles of nitroglycerin produces a total of 12 + 6 + 1 + 10 = 29 moles of gas.
Therefore:
0.017 moles of nitroglycerin produces a total of:
(0.017 x 29) / 4 = 0.12325 moles of gases

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ss7ja [257]

Answer: The density of substance is $3.38g/cm^3$

Explanation:

To calculate density of a substance, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

We are given:

Mass of substance = 61.6 g

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Putting values in above equation, we get:

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2 years ago

A sample of 4.0 L of nitrogen, at 1.2 atmospheres, is transferred to a 12 L container.

Zielflug [23.3K]

Answer:

The pressure will be 0.4 atm.

Explanation:

The gas laws are a set of chemical and physical laws that allow determining the behavior of gases in a closed system. The parameters evaluated in these laws are pressure, volume, temperature and moles.

As the volume increases, the gas particles (atoms or molecules) take longer to reach the walls of the container and therefore collide with them less times per unit of time. This means that the pressure will be lower because it represents the frequency of collisions of the gas against the walls. In this way pressure and volume are related, determining Boyle's law which says:

"The volume occupied by a certain gaseous mass at constant temperature is inversely proportional to pressure"

Boyle's law is expressed mathematically as:

P*V= k

If you initially have the gas at a volume V1 and press P1, when the conditions change to a volume V2 and pressure P2, the following is satisfied:

P1*V1= P2*V2

In this case:

P1= 1.2 atm
V1= 4 L
P2= ?
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Replacing:

1.2 atm* 4 L= P2* 12 L

Solving:

$P2=\frac{1.2 atm*4 L}{12 L}$

P2= 0.4 atm

The pressure will be 0.4 atm.

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The reaction below has an equilibrium constant kp=2.2×106 at 298 k. 2cof2(g)⇌co2(g)+cf4(g) calculate kp for the reaction below.

AnnZ [28]

I believe the correct 2nd reaction is:

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where we can see that it is exactly one-half of the original

Therefore the new Kp is:

new Kp = (old Kp)^(1/2)

new Kp = (2.2 x 10^6)^(1/2)

new Kp = 1,483.24

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