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Charra [1.4K]
3 years ago
9

250 g H 2 SO 4 completely reacted with aluminum?

Chemistry
1 answer:
Rasek [7]3 years ago
3 0

Answer: 290 g of aluminium sulphate is produced.

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of} H_2SO_4=\frac{250g}{98g/mol}=2.55moles

The balanced chemical reaction is:

2Al(s)+3H_2SO_4(aq)\rightarrow Al_2(SO_4)_3(aq)+3H_2(g)

According to stoichiometry :

3 moles of H_2SO_4 produce  = 1 mole of Al_2(SO_4)_3

Thus 2.55 moles of H_2SO_4 will require=\frac{1}{3}\times 2.55=0.85moles  of Al_2(SO_4)_3

Mass of Al_2(SO_4)_3=moles\times {\text {Molar mass}}=0.85moles\times 342g/mol=290g

Thus 290 g of aluminium sulphate is produced.

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Answer:

C) In[reactant] vs. time

Explanation:

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A = A_{0}e^{-kt}

where A(0) = initial concentration of the reactant

A = concentration after time 't'

k = rate constant

Taking ln on both sides gives:

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7 0
3 years ago
Convert 7.1x10^25 molecules of water to moles
ruslelena [56]

Answer:

<h2>117.94 moles</h2>

Explanation:

To find the number of moles in a substance given it's number of entities we use the formula

n =  \frac{N}{L} \\

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

n =  \frac{7.1 \times  {10}^{25} }{6.02 \times  {10}^{23} }  \\  = 117.940199...

We have the final answer as

<h3>117.94 moles</h3>

Hope this helps you

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Explanation:

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