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2 years ago

Convert 9.32x 10 23ª atoms of au to moles of au

Chemistry

1 answer:

7nadin3 [17]2 years ago

5 0

Answer:

$\huge\boxed{\sf no.\ of\ moles = 1.55\ moles }$

Explanation:

<u>Given:</u>

Number of atoms = $9.32 \times 10^{23}$ atoms

Avogadro's Number = $6.023 \times 10^{23}$ atom / mol

<u>Required:</u>

Moles = ?

<u>Formula:</u>

$\displaystyle No.\ of\ moles = \frac{no. \ of \ atoms }{avogadro's \ no.}$

<u>Solution:</u>

$\displaystyle no. \ of \ moles = \frac{9.32\times 10^{23}}{6.023 \times 10^{23}}$

no. of moles = 1.55 moles

$\rule[225]{225}{2}$

Hope this helped!

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$\begin{array}{rcl}\text{Heat lost by metal + heat gained by water} & = & 0\\q_{1} + q_{2} & = & 0\\m_{1}C_{1}\Delta T_{1} + m_{2}C_{2}\Delta T_{2} & = & 0\\\text{125 g}\times 0.900 \text{ J$^{\circ}$C$^{-1}$g$^{-1}$} \times\Delta T_{1} + \text{100 g} \times 4.184 \text{ J$^{\circ}$C$^{-1}$g$^{-1}$}\Delta \times T_{2} & = & 0\\112.5\Delta T_{1} + 418.4\Delta T_{2} & = & 0\\112.5\Delta T_{1} & = & -418.4\Delta T_{2}\\\Delta T_{1} & = & -3.719\Delta T_{2}\\\end{array}$

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