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3 years ago

Which property is constant in the combined gas law?

Chemistry

2 answers:

Thepotemich [5.8K]3 years ago

5 0

Answer: The correct answer is number of particles.

Explanation:

Ideal gas law states the relationship between the variables of the gas. the variables are pressure, volume and temperature of the gas.

This combined gas law is calculated by the three laws:

1) Boyle's Law: This law states that pressure of the gas is inversely proportional to the volume of the gas at constant temperature and number of moles.

$P\propto \frac{1}{V}$ (At constant temperature and number of moles)

2) Charles' Law: This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure and number of moles.

$V\propto T$ (At constant pressure and number of moles)

3) Gay-Lussac's Law: This law states that pressure of the gas is directly proportional to the temperature of the gas at constant volume and number of moles.

$P\propto T$ (At constant volume and number of moles)

From the above three laws, the combined gas law equation becomes:

$\frac{PV}{T}=k$

Or,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

As seen clearly above, number of particles in the above combined gas law equation remains constant.

Marta_Voda [28]3 years ago

4 0

Number of particles

combined gas law : P1V1/T1 = P2V2/T2

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If 8.753 g of the heptahydrate produces 8.192 g of the hexahydrate, how many grams of anhydrous nickel(ii) sulfate could be obta

Ede4ka [16]

Answer is: 4.826 grams of anhydrous nickel(II) sulfate could be obtained.

m(NiSO₄×7H₂O) = 8.753 g; mass of heptahydrate.

m(NiSO₄×6H₂O) = 8.192 g; mass of hexahydrate.

m(H₂O) = m(NiSO₄×7H₂O) - m(NiSO₄×6H₂O).

m(H₂O) = 8.753 g - 8.192 g.

m(H₂O) = 0.561 g.

m(NiSO₄) = m(NiSO₄×7H₂O) - 7 · m(H₂O).

m(NiSO₄) = 8.753 g - 7 · 0.561 g.

m(NiSO₄) = 4.826 g.

5 0

3 years ago

What the volume is.

alekssr [168]

The molar mass of NO₂ is 46.0 g/mol

The molar mass of Pb (NO₃)₂ is 331.2 g/mol

First there is a need to find the number of moles of NO₂ via the stoichiometry of reaction:

2Pb(NO₃)₂ → 2PbO (s) + 4NO₂ (g) + 02 (g)

2 × 331.2 g = 4 × 46.0 g

16.87 g = x (mass of NO₂)

mass of NO₂ = 16.87 × 4 × 46 / 2 × 331.2

mass of NO₂ = 3104.08 / 662.4

mass of NO₂ = 4.686 g of NO₂

Now the number of moles are:

1 mole NO₂ = 46.0 g

x moles of NO₂ = 4.686 g

4.686 × 1 / 46.0 = 0.101 moles of NO₂

1 mole = 22.4 L (at STP)

0.101 moles of NO₂ = 0.101 × 22.4 / 1

= 2.26 L

4 0

3 years ago

1N2 + 3H2 -->

Hunter-Best [27]

Answer:

28.23 g NH₃

Explanation:

The balanced chemical equation is:

N₂(g) + 3 H₂(g) → 2 NH₃(g)

Thus, 1 mol of N₂ reacts with 2 moles of H₂ to produce 2 moles of NH₃. We convert the moles to mass (in grams) by using the molecular weight (MW) of each compound:

MW(N₂) = 2 x 14 g/mol = 28 g/mol

mass N₂= 1 mol x 28 g/mol = 28 g

MW(H₂) = 2 x 1 g/mol = 2 g/mol

mass H₂ = 3 mol x 2 g/mol = 6 g

MW(NH₃) = 14 g/mol + (3 x 1 g/mol) = 17 g/mol

mass NH₃= 2 moles x 17 g/mol = 34 g

Now, we have to figure out which is the limiting reactant. For this, we know that the stoichiometric ratio is 28 g N₂/6 g H₂. If we have 36.85 g of H₂, we need the following mass of N₂:

36.85 g H₂ x 28 g N₂/6 g H₂ = 171.97 g N₂

We have 23.15 g N₂ and we need 171.97 g. So, we have lesser N₂ than we need. Thus, the limiting reactant is N₂.

Now, we calculate the product (NH₃) by using the stoichiometric ratio 34 g NH₃/28 g N₂, with the mass of N₂ we have:

23.25 g N₂ x 34 g NH₃/28 g N₂ = 28.23 g NH₃

Therefore, the maximum amount of NH₃ that can be produced is 28.23 grams.

5 0

3 years ago

have you ever been swimming and noticed some areas in the water are colder and other are warmer? why do you think this happens

timama [110]

Maybe because someone hasn't been swimming on tht side bacause the water changes it's tempurture from your body heat or maybe because it isnt any sun out

6 0

3 years ago

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alexandr402 [8]

Answer:

1.90 L

Explanation:

Using Boyle's law

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