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Bingel [31]
3 years ago
13

A sample compound contains 9.11 g Ni and 5.89g F. What is the empirical formula of this compound?

Chemistry
2 answers:
Alexxx [7]3 years ago
8 0

The empirical formula of the compound is C. NiF₂.

<em>Step 1</em>. Calculate the <em>moles of each element</em>

The empirical formula is the simplest whole-number ratio of atoms in a compound.

The ratio of atoms is the same as the ratio of moles.

So, our job is to calculate the molar ratio of Ni to F.

Moles of Ni = 9.11 g Ni × (1 mol Ni /(58.69 g Ni) = 0.1552 mol Ni

Moles of F = 5.89 g F × (1 mol F/19.00 g F) = 0.3100 mol F

<em>Step 2</em>. Calculate the <em>molar ratio</em> of the elements

Divide each number by the smallest number of moles

Ni:F = 0.1552:0.3100 = 1:1.997 ≈ 1:2

<em>Step 3</em>: Write the <em>empirical formula</em>

EF = NiF₂

Novay_Z [31]3 years ago
3 0

Answer:

C

Explanation:

Edg2020

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If the wavelength of purple light is 400 x 10^-9 m, what is the frequency?
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The frequency : a) 7.5 x 10¹⁴ /s

<h3>Further explanation</h3>

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The energy in one photon can be formulated as

\large{\boxed{\bold{E\:=\:h\:.\:f}}}

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λ = wavelength

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\tt f=\dfrac{c}{\lambda}\\\\f=\dfrac{3.10^8~m/s}{4.10^{-7}m}\\\\f=\boxed{\bold{7.5.10^{14}}/s}

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Ierofanga [76]

Answer:

0.417 J/gºC

Explanation:

From the question given above, the following data were obtained:

Heat (Q) absorbed = 2500 J

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Final temperature (T2) = 70 °C

Specific heat capacity (C) =?

Next, we shall determine the change in temperature (ΔT). This can be obtained as follow:

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Final temperature (T2) = 70 °C

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