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ra1l [238]
2 years ago
6

What mass of ni has as many atoms as there are n atoms in 63.0 g of no2?

Chemistry
2 answers:
adoni [48]2 years ago
8 0

Answer : The mass of Ni is, 80.346 g

Solution :

First we have to calculate the number of moles.

\text{Moles of }NO_2=\frac{\text{Mass of }NO_2}{\text{Molar mass of }NO_2}=\frac{63g}{46g/mole}=1.369moles

Now we have to calculate the number of atoms of NO_2

As 1 moles NO_2 contains 6.022\times 10^{23} number of molecules

So, 1.369 moles NO_2 contains 1.369\times 6.022\times 10^{23} number of molecules

One NO_2 molecule has one nitrogen atom then 1.369\times 6.022\times 10^{23} number of molecules of NO_2 will contain 1.369\times 6.022\times 10^{23} number of nitrogen atoms

As per question number of Ni atoms is equal to the number of nitrogen atoms

Number of Ni atoms=1.369\times 6.022\times 10^{23} atoms

Number of moles = \frac{1.369\times 6.022\times 10^{23}}{6.022\times 10^{23}}=1.369moles

Mass of Nickel = Moles\times \text{Molecular mass}}

Molecular mass of Nickel = 58.69 g/mol

Mass of nickel = 1.369mol\times 58.69g/mol=80.346grams

djverab [1.8K]2 years ago
6 0

Answer:

80.42 g

Explanation:

NO2 has molar mass equal to 46 g/mol ( 14 of N + 2x16 of O). So, for 63.0 g of NO2, the number of moles are:

n = mass/molar mass

n = 63/46

n = 1.37 moles

By Avogadro's Law, 1 mol has 6.02x10^{23} atoms, for any substance. So, the substances will have the same number of atoms if they had the same number of moles

Then, n of Ni is 1.37 moles.

The molar mass of Ni is 58.7 g, so:

n = mass (m)/ molar mass

1.37 = m/58.7

m = 1.37x58.7

m = 80.42 g

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There is some info missing. I think this is the original question.

<em>Calculate the percent ionization of nitrous acid in a solution that is 0.249 M in nitrous acid. The acid dissociation constant of nitrous acid is  4.50  ×  10 ⁻⁴.</em>

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Step 1: Given data

Initial concentration of the acid (Ca): 0.249 M

Acid dissociation constant (Ka): 4.50  ×  10 ⁻⁴

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HNO₂(aq) ⇒ H⁺(aq) + NO₂⁻(aq)

Step 3: Calculate the concentration of nitrite in the equilibrium ([A⁻])

We will use the following expression.

[A^{-} ] = \sqrt{Ca \times Ka } = \sqrt{0.249 \times 4.50 \times 10^{-4}  } = 0.0106 M

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We will use the following expression.

\alpha = \frac{[A^{-} ]}{[HA]} \times 100\% = \frac{0.0106M}{0.249} \times 100\% = 4.26\%

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