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Romashka-Z-Leto [24]
3 years ago
15

Two stones resembling diamonds are suspected of being fakes. To determine if the stones might be real, the mass and volume of ea

ch are measured. Both stones have the same volume, 0.15 cm^3. However, stone A has a mass of 0.52 g, and stone B has a mass of 0.42 g.
A) If diamond has a density of 3.5 g/cm^3, could either of the stones be real diamonds? Explain.
Chemistry
1 answer:
Charra [1.4K]3 years ago
4 0

Answer:

Stone A

Explanation:

Measuring density is an easiest way to determine if two similar looking substances are same or not. Here also we need to perform the density test for each stone that is suspected to be fake diamond. We will calculate the density of each stone and compare it with the density of original diamond.

Density is calculated using the formula

Density=\frac{Mass}{Volume}

It has been given in the question that both the substances have same volume of 0.15 cm^3.

Density of stone A = \frac{0.52}{0.15} = 3.47 gcm^-^3 or after rounding off we get 3.5 gcm^-^3

Density of stone B = \frac{0.42}{0.15} = 2.8 gcm^-^3

It is clear from the above calculation that the stone A has same density as the diamond but stone B lacks behind in density.

So, stone A could be the real diamond.

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<span>the balanced equation for the reaction is as follows
Na</span>₂<span>SO</span>₄<span> + BaCl</span>₂<span> ----> 2NaCl + BaSO</span>₄ 
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first we need to find out which the limiting reactant is
limiting reactant is fully used up in the reaction.
                                                                           
number of Na2So4 moles - 0.5 mol number of BaCl2 moles - 60 g / 208 g/mol = 0.288 mol
since molar ratio is 1:1 equal number of moles of both reactants should react with each other
                                                                         
therefore BaCl2 is the limiting reactant and Na2SO4 is in excess. amount of product formed depends on number of limiting reactant present.
stoichiometry of BaCl</span>₂<span> to BaSO</span>₄<span> is 1:1.
                                                                           
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The given question is incomplete, the complete question is:

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete — the lime absorbs CO2 from the air and turns back into hard, durable limestone.

Suppose some calcium carbonate is sealed into a limekiln of volume 850 L and heated to 740.0 C. When the amount of CaCO3 has stopped changing, it is found that 2.05 kg have disappeared.

Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 740.0 C. Round your answer to significant digits.

Answer:

The correct answer is 2.00.

Explanation:

Based on the given information, the pressure equilibrium constant or Kp is equivalent to pressure of carbon dioxide or PCO₂. The reaction taking place in the given case is:  

CaCO₃ (s) ⇄ CaO (s) + CO2 (g)

The molecular weight of CO2 is 44 g/mol and the molecular weight of CaCO₃ is 100 g/mol. The amount of CaCO₃ that got disappeared in the given case is 2.05 Kg or 2050 grams. Therefore, the amount of CO₂ is,  

2050 g CaCO₃ * (44 g CO2/100 g CaCO₃) = 902 g CO2

The pressure of CO2, which is equivalent to Kp can be determined by using the formula,  

P = nRT/V

Here V is the volume, which is 850 L, T is the temperature, which is 740 degree C or 1013 K, R is the rate constant, which is 0.0822 L.atm/K.mole

n is the no. of moles, which is equal to weight/molecular wt,  

n = 902 g/44 g/mol = 20.5 mole

Now putting the values we get,  

P = 20.5 mole * 0.0821 L.atm/K.mole * 1013 K / 850 L

P = 2.00 atm or Kp = 2.00

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Answer:

Deductive reasoning.

Explanation:

Hello,

Deductive reasoning lies on the proposal of a hypothesis and its subsequent substantiation before any observation is carried out since the statement says that "he assumes will apply to all situations" he's proposing something before observing it.

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