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Juli2301 [7.4K]
2 years ago
10

65 g of NaOH is dissolved to make 500 mL of solution. Find moles of NaPH and Molarity of solution.

Chemistry
1 answer:
Lisa [10]2 years ago
8 0

Answer:

3.25 M

Explanation:

Number of moles = mass/ molar mass

mass of  NaOH = 65 g

Molar mass of NaOH = 40 g/mol

Number of moles of NaOH = 65g/40 g/mol = 1.625 moles

Let us recall that;

n = CV

n = number of moles of solute

C = concentration of solution

V = volume of solution

C = n/V

n = 1.625 moles

V = 500/1000 L = 0.5 L

C = 1.625 moles/0.5

C = 3.25 M

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Answer: The heat required is 6.88 kJ.

Explanation:

The conversions involved in this process are :

(1):ethanol(s)(-135^0C)\rightarrow ethanol(s)(-114^0C)\\\\(2):ethanol(s)(-114^0C)\rightarrow ethanol(l)(-114^0C)\\\\(3):ethanol(l)(-114^0C)\rightarrow ethanol(l)(-50^0C)

Now we have to calculate the enthalpy change.

\Delta H=[m\times c_{p,s}\times (T_{final}-T_{initial})]+n\times \Delta H_{fusion}+[m\times c_{p,l}\times (T_{final}-T_{initial})]+n\times \Delta H_{vap}+[m\times c_{p,g}\times (T_{final}-T_{initial})]

where,

\Delta H = enthalpy change = ?

m = mass of ethanol = 25.0 g

c_{p,s} = specific heat of solid ethanol= 0.97 J/gK

c_{p,l} = specific heat of liquid ethanol = 2.31 J/gK

n = number of moles of ethanol = \frac{\text{Mass of ethanol}}{\text{Molar mass of ethanol}}=\frac{25.0g}{46g/mole}=0.543mole

\Delta H_{fusion} = enthalpy change for fusion = 5.02 KJ/mole = 5020 J/mole

T_{final}-T_{initial}=\Delta T = change in temperature

The value of change in temperature always same in Kelvin and degree Celsius.

Now put all the given values in the above expression, we get

\Delta H=[25.0 g\times 0.97J/gK\times (-114-(-135)K]+0.534mole\times 5020J/mole+[25.0g\times 2.31J/gK\times (-50-(-114))K]

\Delta H=6885.93J=6.88kJ     (1 KJ = 1000 J)

Therefore, the heat required is 6.88 kJ

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Answer:

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Since we don't have the chemical equation we will have to make one I guess.

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So ratio is 2:1 FeBr3 to Fe2S3

So we need 0.76 moles of Fe2S3

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7 0
3 years ago
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