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3 years ago

What is the mass of HCL is consumed by the reaction of 1.5 mole of magnesium

Chemistry

1 answer:

photoshop1234 [79]3 years ago

3 0

Answer: 109.5g

Explanation:

Mg + 2HCl —> MgCl2 + H2

From the equation,

1mole of Mg required 2moles of HCl

Therefore 1.5moles of Mg will require = 1.5 x 2 = 3 moles of HCl.

Molar Mass of HCl = 1+35.5 =36.5g/mol

Mass conc. Of HCl = 3 x 36.5 = 109.5g

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A chunk of tin weighing 18.5 grams and originally at 97.38 °C is dropped into an insulated cup containing 75.7 grams of water at

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Answer:

The final temperature of the water is 22.44°C.

Explanation:

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

$-q_1=q_2$

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Specific heat capacity of tin = $c_1=0.21 J/g^oC$

Initial temperature of the tin = $T_1=97.38^oC$

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Initial temperature of the water = $T_3=21.52^oC$

Final temperature of water = $T_2$ =T

$q_2=m_2c_2\times (T-T_3)$

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$-(m_1\times c_1\times (T-T_1))=m_2\times c_2\times (T-T_3)$

On substituting all values:

$-(18.5 g\times 0.21 J/g^oC\times (T-97.38^oC))=75.7 g\times 4.184 J/g^oC\times (T-21.52 ^oC)$

we get, T = 22.44°C

The final temperature of the water is 22.44°C.

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