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Nostrana [21]
3 years ago
14

Why is water displacement an effective way of measuring the volume of an irregular solid?

Chemistry
2 answers:
hichkok12 [17]3 years ago
6 0

Explanation:

As it is known that volume of an irregular object cannot be measured because we cannot measure the volume of a curve.

As a result, if we immerse an irregular solid object into a beaker or container filled with water then the volume of water displaced by the object will be equal to the volume of object itself.

Hence, we get to know the volume of irregular solid object by doing so that is why, water displacement is an effective way of measuring the volume of an irregular solid.

aksik [14]3 years ago
5 0
Water displamement is effective because there is no way to get an exact and accurate measurement of an irregular solid because you can't measure curved line. Water displamement gives you a proper, exact, and accurate answer.
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In a separate experiment beginning from the same initial conditions, including a temperature Ti of 25.0°C, half the number of mo
NNADVOKAT [17]

Answer:

- 178 ºC

Explanation:

The  ideal gas law   states that :

PV = nRT,

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

For the initial conditions :

P₁ V₁ = n₁ R T₁    (1)

and for the final conditions:

P₂V₂= n₂ R T₂    where   n₂ = n₁/2     then    P₂ V₂ = n₁/2 T₂    (2)

Assuming V₂ = V₁ and  dividing (2) by Eqn (1) :

P₂ V₂ = n₁/2 R T₂  / ( n₁ R T₁)      then  P₂ / P₁ = 1/2 T₂ / T₁

4.10 atm / 25.7 atm = 1/2 T₂ / 298 K ⇒ T₂ = 0.16 x 298 x 2 = 95.1 K

T₂ = 95 - 273 = - 178 º C

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If 5.57 g of Ag2O is sealed in a 75.0-mL tube filled with 760 torr of N2 gas at 28 ∘C, and the tube is heated to 310 ∘C, the Ag2
Snezhnost [94]

Answer: Total pressure = 7293.2 torr or 9.60 atm

Explanation:

<em>Total pressure = partial pressure of nitrogen + partial pressure of oxygen</em>

The partial pressure due to nitrogen is determined using the equation of Gay-Lussac's law: <em>P₁/T₁=P₂/T₂</em>

P₁ = 760 torr = 1atm, T₁ = 28∘C = (273+28)K = 301k, P₂ = ?, T₂ = 310∘C =(310+273)K = 583K

P₂ = P₁ T₂/ T₁

P₂ = 760 * 583 / 301 = 1472.03 torr

The pressure due to Oxygen gas produced is calculated thus:

Balanced equation of the decomposition of Ag₂O at s.t.p. is as follows;

2Ag₂O ----> 4Ag + O₂(g)

2 moles of Ag₂O produces 1 mole of O₂

molar mass of Ag₂O = (2*108 + 16)g = 232g/mol

molar volume of gas at s.t.p. = 22.4L

2*232g i.e. 464g of Ag₂O produces 22.4L of O₂

5.57g of Ag₂O will produce 5.57g*22.4L/464g = 0.269L or 269mL of O₂

Using the General gas equation  P₁V₁/T₁=P₂V₂/T₂

P₁ = 1atm = 760 torr, V₁ = 269mL, T₁=273K, P₂ = ?, V₂= 75mL, T₂ = 583K

P₂ = P₁V₁T₂/V₂T₁

P₂ = 760*269*583 / 75*273

P₂ = 5821.17 torr

Total pressure = (1472.03 + 5821.17) torr

Total pressure = 7293.2 torr or 9.60 atm

7 0
3 years ago
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