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3 years ago

Chlorine gas reacts with aluminum metal producing aluminum chloride. What mass of chlorine reacts with 9.00g of Al to form AlCl3

1 answer:

6 0

The mass of chlorine that react with 9.00 g of Al to form AlCl3 is 35.465 grams

Explanation
write the equation for reaction
that is
2 Al + 3 Cl2 = 2 Al CL3
find the moles of Al reacted

moles = mass/molar mass

9 g/ 27 g/mol = 0.333 moles of Al

by use of mole ratio between Al to Cl2 which is 2:3 find the moles of Cl2

mole of cl2 = 0.333 x3/2 = 0.4995 moles

mass of Cl2 is therefore = moles x molar mass

= 0.4995 x71 = 35.465 moles

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2 years ago

What is the mass of 0.28 mole of iron?

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3 years ago

A 32.2 g iron rod, initially at 21.9 C, is submerged into an unknown mass of water at 63.5 C. in an insulated container. The fin

lorasvet [3.4K]

Answer : The mass of the water in two significant figures is, $3.0\times 10^1g$

Explanation :

In this case the heat given by the hot body is equal to the heat taken by the cold body.

$q_1=-q_2$

$m_1\times c_1\times (T_f-T_1)=-m_2\times c_2\times (T_f-T_2)$

where,

$c_1$ = specific heat of iron metal = $0.45J/g^oC$

$c_2$ = specific heat of water = $4.18J/g^oC$

$m_1$ = mass of iron metal = 32.3 g

$m_2$ = mass of water = ?

$T_f$ = final temperature of mixture = $59.2^oC$

$T_1$ = initial temperature of iron metal = $21.9^oC$

$T_2$ = initial temperature of water = $63.5^oC$

Now put all the given values in the above formula, we get

$32.3g\times 0.45J/g^oC\times (59.2-21.9)^oC=-m_2\times 4.18J/g^oC\times (59.2-63.5)^oC$

$m_2=30.16g\approx 3.0\times 10^1g$

Therefore, the mass of the water in two significant figures is, $3.0\times 10^1g$

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3 years ago

Which element is oxidized in the reaction below? fe(co)5 (l) + 2hi (g) fe(co)4i2 (s) + co (g) + h2 (g)?

DanielleElmas [232]

Oxidation state of I is (-1) and for CO it is zero. Let's assume that the oxidation state of Fe in Fe(CO)₄I₂<span> (s) is x. For whole compound, the charge is zero.

Sum of oxidation numbers in all elements = Charge of the compound.

Here we have 1Fe , 4CO and 2I
hence we can find the oxidation state as;
x + 4*0 + 2*(-1) = 0
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Hence the oxidation state of Fe in product </span>Fe(CO)₄I₂ (s) is +2.

Same as we can find the oxidation state (y) of Fe in Fe(CO)₅(s).
y + 5*0 = 0
y = 0

Since oxidation state of Fe increased from 0 to +2, the oxidized element is Fe in the given reaction.

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3 years ago