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3 years ago

How can naphthalene be separated from a mixture of kbr and sand?

2 answers:

7 0

Put it in a beaker. Use a smaller beaker filled half way with ice and water and place in the larger one. It should be about an inch or two above the mixture. Heat over a Bunsen burner and the naphthalene will deposit on the bottom of smaller beaker.

And in this way, nephthalene be separated from the mixture of KBR and sand.

Fofino [41]3 years ago

7 0

Explanation:

A mixture of naphthalene in KBr and sand can be separated by heating as naphthalene has low boiling point. Hence, its volatility is high due to which it will easily escape out from the mixture.

So, vapors of naphthalene can be collected through sublimation. As a result, naphthalene will be separated out from the mixture.

Now, only KBr and sand is left in the mixture. So, water will be added in to this mixture due to which KBr will dissolve in it. And upon filtration sand will be separated out of this mixture.

Whereas upon heating the mixture of water and KBr, water will evaporate and crystals of KBr will be obtained. As a result, all the components of this mixture will be separated out.

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How many gallon are there in 85.00 L?

DerKrebs [107]

Answer:

22.46

Explanation:

.There are 3.79 liters in one gallon

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3 years ago

A scientist measures the standard enthalpy change for the following reaction to be -17.2 kJ : Ca(OH)2(aq) 2 HCl(aq)CaCl2(s)

elixir [45]

Answer: $\Delta H^{0}=-173.72$ kJ/mol

Explanation: Enthalpy Change is the amount of energy in a reaction - absorption or release - at a constant pressure. So, Standard Enthalpy of Formation is how much energy is necessary to form a substance.

The standard enthalpy of formation of HCl is calculated as:

$\Delta ^{0}=\Sigma H_{products}-\Sigma H_{reactants}$

$Ca(OH)_{2}_{(aq)}+2HCl_{(aq)}$ → $CaCl_{2}_{(s)}+2H_{2}O_{(l)}$

Standard Enthalpy of formation for the other compounds are:

Calcium Hydroxide: $\Delta H^{0}=$ -1002.82 kJ/mol

Calcium chloride: $\Delta H^{0}=$ -795.8 kJ/mol

Water: $\Delta H^{0}=$ -285.83 kJ/mol

Enthalpy is given per mol, which means we have to multiply by the mols in the balanced equation.

Calculating:

$-17.2=[-795.8+2(285.85)]-[-1002.82+2\Delta H]$

$-17.2=-1367.46+1002.82-2\Delta H$

$2\Delta H=17.2-364.64$

$\Delta H=-173.72$

So, the standard enthalpy of formation of HCl is -173.72 kJ/mol

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2 years ago

?cual es el tiempo de onda con 6 oscilaciones.?

Setler79 [48]

Answer:

Hey hi

Explanation:

Can you pls tell me which language is this.... Pls really sorry... I wanna help you

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3 years ago

Part A

den301095 [7]

Answer:

$n_{Cl_2}=0.3molCl_2$

Explanation:

Hello there!

In this case, according to the given chemical reaction whereas the sodium chloride is in a 2:1 mole ratio with chlorine, the required moles of the later are computed as shown below:

$n_{Cl_2}=0.6molNaCl*\frac{1molCl_2}{2molNaCl}$

So we cancel out the moles of NaCl to obtain:

$n_{Cl_2}=0.3molCl_2$

Best regards!

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2 years ago

At 1 atm of pressure and a temperature of 0 degrees celsius, which phases of H2O can exist?

NemiM [27]

B, because water is changing its state from solid to liquid (it's fusion in portuguese, don't know in english), so while it's changing, water has 2 states at the same time.

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3 years ago