What is the atomic mass of 3NaCl

Copper sulfate is a blue solid that is used to control algae growth. Solutions of copper sulfate that come in contact with the s

True [87]

Answer:

185.49 grams of Zinc would react with 454g (1lb) of copper sulfate

Explanation:

Yo know the following balanced reaction:

CuSO₄(aq)+ Zn(s) →Cu(s) + ZnSO₄(aq)

You can see that by stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of reagents and products are part of the reaction:

CuSO₄: 1 mole
Zn: 1 mole
Cu: 1 mole
ZnSO₄: 1 mole

Being:

Cu: 63.54 g/mole
S: 32 g/mole
O: 16 g/mole
Zn: 65.37 g/mole

the molar mass of the compounds participating in the reaction is:

CuSO₄:63.54 g/mole + 32 g/mole + 4*16 g/mole= 159.54 g/mole ≅ 160 g/mole
Zn: 65.37 g/mole
Cu: 63.54 g/mole
ZnSO₄: 65.37 g/mole + 32 g/mole + 4*16 g/mole= 161.37 g/mole

Then, by stoichiometry of the reaction, the following amounts of mass of reagent and product participate in the reaction:

CuSO₄: 1 moles* 160 g/mole= 160 g
Zn: 1 mole* 65.37 g/mole= 65.37 g
Cu: 1 mole* 63.54 g/mole= 63.54 g
ZnSO₄: 1 mole* 161.37 g/mole= 161.37 g

Now you can apply the following rule of three: if 160 grams of CuSO₄ react with 65.37 grams of Zn by this reaction stoichiometry, 454 grams of CuSO₄ with how much mass of Zn will it react?

$mass of Zn=\frac{454 grams of CuSO_{4} *65.37 grams of Zn}{160 grams of CuSO_{4}}$

mass of Zn= 185.49 grams

185.49 grams of Zinc would react with 454g (1lb) of copper sulfate

4 0

3 years ago

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Ira Lisetskai [31]

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8 0

2 years ago

At-57 °C and 1 atm, carbon dioxide is in which phase? View Available Hint(s) Phase diagrams for water (Figure 1)and carbon dioxi

goblinko [34]

Answer:

Gas

Increase the pressure

Explanation:

Let's refer to the attached phase diagram for CO₂ (not to scale).

At -57 °C and 1 atm, carbon dioxide is in which phase?

If we look at the intersection between -57°C and 1 atm, we can see that CO₂ is in the gas phase.

At 10°C and 2 atm carbon dioxide is in the gas phase. From these conditions, how could the gaseous CO₂ be converted into liquid CO₂?

Since at 10°C and 2 atm carbon dioxide is below the triple point, the only way to convert it into liquid is by increasing the pressure (moving up in the vertical direction).