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Stolb23 [73]
3 years ago
9

A sample of ideal gas is in a sealed container. The pressure of the gas is 485 torr , and the temperature is 40 ∘C . If the temp

erature changes to 74 ∘C with no change in volume or amount of gas, what is the new pressure, P2, of the gas inside the container?
Chemistry
1 answer:
Fantom [35]3 years ago
3 0

Answer:

537.68 torr.

Explanation:

  • We can use the general law of ideal gas:<em> PV = nRT.</em>

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R is the general gas constant,

T is the temperature of the gas in K.

  • If n and V are constant, and have different values of P and T:

<em>(P₁T₂) = (P₂T₁).</em>

P₁ = 485 torr, T₁ = 40°C + 273 = 313 K,

P₂ = ??? torr, ​T₂ = 74°C + 273 = 347 K.

∴ P₂ = (P₁T₂)/(P₁) = (485 torr)(347 K)/(313 K) = 537.68 torr.

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n=\frac{m}{M}

Here, m is mass and M is molar mass.

Putting the values,

n=\frac{2.493 g}{63.546 g/mol}=0.03923 mol

Now, in 1 mole of Cu there are 6.303\times 10^{23}atoms thus, in 0.03923 mol, number of Cu atoms will be:

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What is the volume that you should dilute 30mL of a 12.0M H2SO4 solution to obtain a 0.160M H2SO4 solution?
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What volume of a 0.155 M potassium hydroxide solution is required to neutralize 25.7 mL of a 0.388 M hydrobromic acid solution
vekshin1

Answer: Therefore, the volume of a 0.155 M potassium hydroxide solution  is 56.0 ml

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

According to the neutralization law,

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Therefore, the volume of a 0.155 M potassium hydroxide solution  is 56.0 ml

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