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3 years ago

2AgNO_3 \rightarrow 2Ag + Cu(NO_3)_2" alt="Cu + 2AgNO_3 \rightarrow 2Ag + Cu(NO_3)_2" align="absmiddle" class="latex-formula">
How many grams of \text{Ag} will be produced from 5.00 g of Cu and 1 .00 g of AgNO₃?

Chemistry

1 answer:

il63 [147K]3 years ago

5 0

Answer:

0.635 g

Explanation:

First, we have to find the limiting reagent. Convert Cu and AgNo₃ to moles. You should get 0.0786 moles of Cu and 0.00589 moles of AgNO₃.

AgNO₃ has the least amount of moles making it the limiting reagent.

Then, we use stoichiometry to find how many moles of Ag can be made with our limiting reagent. Based on the chemical equation, for every 2 moles of AgNO₃, you will get 2 moles of Ag.

This means that you should get 0.00589 moles of Ag.

Convert moles to grams. You should get 0.6349958... grams.

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a 50.0 mL sample of KCl requires 22.40 mL of 0.0229 M Pb(NO3)2 in order to completely titrate it. What is the Molarity of the KC

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0.02052M

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First, we need to write a balanced equation for the reaction. This is illustrated below:

2KCl + Pb(NO3)2 → 2KNO3 + PbCl2

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Molarity of Pb(NO3)2 = 0.0229M

Volume of Pb(NO3)2 = 22.40 = 22.4/1000 = 0.0224L

Number of mole of Pb(NO3)2 =?

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Mole = Molarity x Volume

Mole of Pb(NO3)2 = 0.0229x0.0224

Mole of Pb(NO3)2 = 5.13x10^-4mole

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1mole of Pb(NO3)2 required 2moles KCl.

Therefore, 5.13x10^-4mole of Pb(NO3)2 will require = 5.13x10^-4x2 = 1.026x10^-3mole of KCl.

Now we can use this amount (i.e 1.026x10^-3mole) to find the molarity of KCl. This is illustrated below:

Mole of KCl = 1.026x10^-3mole

Volume of KCl = 500mL = 50/1000 = 0.05L

Molarity =?

Molarity = mole /Volume

Molarity of KCl = 1.026x10^-3/0.05

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