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3241004551 [841]
3 years ago
13

Consider the reaction of 19.0 g of zinc metal with excess silver nitrate to produce silver metal and zinc nitrate. The reaction

is stopped before all the zinc metal has reacted and 29.0 g of solid metal is present. If 14.6 g of zinc are present in the solid metal, calculate the mass of silver metal present in the mixture.
Chemistry
1 answer:
Alexeev081 [22]3 years ago
4 0

Answer:

14.5 g silver

Explanation:

This is a problem using the stoichiometry of the reaction. First thing we need is the balanced equation:

   Zn + 2 AgNO3 ----------------------- 2 Ag + Zn(NO3)2

We know that 14.6 g of Zn did not reacted, then we can calculate the amount of Zn reacted and do the calculation given the above reaction.

amount Zn reacted: 19.0 -14.6 g Zn = 4.4 g Zn

atomic weight of Zn:  65.37 g/mol

mol Zn reacted: 4.4 g Zn x ( 1 mol Zn/ 65.37 g Zn) = 0.067 mol Zn

We know from the balanced equation that moles of Ag are produced from 1 mol Zn therefore the mol of Ag produced are:

0.067 mol Zn x 2 mol Ag/ 1mol Zn = 0.135 mol Ag

and the mass of silver then will be given by multiplying by the atomic weight of silver:

0.135 mol Ag x  107.9 g/mol = 14.5 g Ag

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Answer:

See explanation.

Explanation:

Hello,

In this case, we say that chemical reactions are governed by the law of conservation of mass, which states that matter cannot be neither created nor destroyed by transformed, for that reason, we need to balance chemical reactions in order to ensure all the atoms to be in the same quantity at both reactants and products.

Moreover, equilibrium is defined as such condition at which the concentration of both reactants and products stop changing over the time so they become constant as well as their null reaction rate.

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N_2(g)+3H_2(g)\rightleftharpoons 2NH_3(g)

In such reaction, we have two nitrogens at both reatants and products and six hydrogens at at both reatants and products for us to obey the law of conservation of mass. Furthermore, as the time goes by, nitrogen reacts with hydrogen, nonetheless, they do not react indefinitely, they have a limit that is equilibrium, so their moles stop being consumed and remain unchanged as well as the produced moles of ammonia.

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1.For the reaction P4 O10(s) + 6H2O(l) → 4H3PO4(aq), what mass of P
Alex17521 [72]
P₄O₁₀ + 6H₂O → 4H₃PO₄
The equation shows us that the molar ratio of
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We also know that one mole of a substance contains 6.02 x 10²³ particles. We can use this to calculate the moles of water.
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3 years ago
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A buffer contains 0.18 mol of propionic acid (C2H5COOH) and 0.26 mol of sodium propionate (C2H5COONa) in 1.20 L. What is the pH
Yuki888 [10]

Answer:

1) pH = 5.05

2) pH = 5.13

3) pH = 4.97

Explanation:

Step 1: Data given

Number of moles of propionic acid = 0.18 moles

Number of moles sodium propionate = 0.26 moles

Volume = 1.20 L

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What is the pH of the buffer after the addition of 0.02 mol of NaOH?

moles acid = 0.18 - 0.02 = 0.16

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What is the pH of the buffer after the addition of 0.02 mol of HI?

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