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agasfer [191]
3 years ago
15

A student wants to make a 0.150 M aqueous solution of silver (I) nitrate but only has 11.27 g of AgNO3. What volume of the 0.150

M solution can they make?
Chemistry
1 answer:
Usimov [2.4K]3 years ago
3 0

Answer:

442.3 mL

Explanation:

Remember that Molarity is a measure of concentration in Chemistry and it's defined as the number of moles of the substance divided by liters of the solution:

M=\frac{Moles of substance X}{Volume of the solution}

Then, you can express 11.27 g of AgNO3 as moles of AgNO3 using the molar mass of the compound:

11.27 g AgNO_{3} *\frac{1 mole AgNO_{3}}{169.87 g AgNO_{3}} = 0.06634 moles AgNO_{3}

Then you can solve for the volume of the solution:

Volume of the solution=\frac{Moles of AgNO_{3}}{M} =\frac{0.06634 mol AgNO_{3}}{0.150 M} =0.4423 L = 442.3 mL

Hope it helps!

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Anuta_ua [19.1K]

Answer : The value of activation energy for this reaction is 108.318 kJ/mol

Explanation :

The Arrhenius equation is written as:

K=A\times e^{\frac{-Ea}{RT}}

Taking logarithm on both the sides, we get:

\ln k=-\frac{Ea}{RT}+\ln A             ............(1)

where,

k = rate constant  = 2.95\times 10^{-3}L/mol.s

Ea = activation energy  = ?

T = temperature = 435 K

R = gas constant  = 8.314 J/K.mole

A = pre-exponential factor  = 3.00\times 10^{+10}L/mol.s

Now we have to calculate the value of rate constant by putting the given values in equation 1, we get:

\ln (2.95\times 10^{-3}L/mol.s)=-\frac{Ea}{8.314J/K.mol\times 435K}+\ln (3.00\times 10^{10}L/mol.s)

Ea=108318.365J/mol=108.318kJ/mol

Therefore, the value of activation energy for this reaction is 108.318 kJ/mol

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Natali5045456 [20]

Answer:

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Explanation:

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