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3 years ago

How many moles are in 1.93 x 10^24 atoms of gold

Chemistry

2 answers:

Anni [7]3 years ago

6 0

Answer:

We know that 1 mole equals to 6.02 x 10^23 atoms (which is Avogadro's number), so to get to atoms from moles, you would divide the atoms of gold by Avogadro's number

(1.93 x 10^24) / (6.02 x 10^23)

= 3.2 mol of gold (rounded)

pshichka [43]3 years ago

4 0

Answer:

do u still need the answer

Explanation:

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A silver block, initially at 58.4∘C, is submerged into 100.0 g of water at 25.0∘C in an insulated container. The final temperatu

Vlada [557]

Answer:

The mass of the silver block is 95.52 grams.

Explanation:

Heat lost by silver will be equal to heat gained by the water

$-Q_1=Q_2$

Mass of silver= $m_1$

Specific heat capacity of silver = $c_1=0.235 J/g^oC$

Initial temperature of the silver = $T_1=58.4^oC$

Final temperature of a silver = $T_2=T=26.7^oC$ =

$Q_1=m_1c_1\times (T-T_1)$

Mass of water= $m_1=100.0 g$

Specific heat capacity of water= $c_2=4.186 J/g^oC$

Initial temperature of the water = $T_3=25^oC$

Final temperature of water = $T_3=T=26.7^oC$

$Q_2=m_2c_2\times (T-T_3)$

$-Q_1=Q_2$

$-(m_1c_1\times (T-T_1))=m_2c_2\times (T-T_3)$

$-(m_1\times 0.235 J/g^oC\times (26.7^oC-58.4^oC))=100.0 g\times 4.186 J/g^oC\times (26.7^oC-25.0^oC)$

On substituting all values:

we get, $m_1 = 95.52 g$

The mass of the silver block is 95.52 grams.

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