# When copper reacts with silver nitrate according to the equation, the number of grams of copper required to produce 432 grams of silver is -?

2 months ago

## Solution 1

Guest #4188
2 months ago
Answer is: mass of copper is 127 grams.
Balanced chemical reaction: Cu(s) + 2AgNO₃(aq) → Cu(NO₃)₂(aq) + 2Ag(s).
m(Ag) = 432 g.
n(Ag) = m(Ag) ÷ M(Ag).
n(Ag) = 432 g ÷ 108 g/mol.
n(Ag) = 4 mol.
From chemical reaction: n(Ag) : n(Cu) = 2 : 1.
n(Cu) = 4 mol ÷ 2 = 2 mol.
m(Cu) = n(Cu) · M(Cu).
m(Cu) = 2 mol · 63.5 g/mol.
m(Cu) = 127 g.

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Explanation:
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Gas stoichiometry: what volume of oxygen at 25 degrees celsius and 1.04 atm is needed for the complete combustion of 5.53 grams of propane?
Solution 1
Answer is: volume of oxygen is 14.7 liters.
Balanced chemical reaction: C₃H₈ + 5O₂ → 3CO₂ + 4H₂O.
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C₃H₈-propane) = 5.53 g.
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Question
What volume of O2( g. at 810. mmHg pressure is required to react completely with a 4.50g sample of C(s) at 48°C? 2 C(s) + O2( g. → 2 CO( g.
Solution 1
Answer is: volume of oxygen is 4.63 liters.
Balanced chemical reaction: 2C + O₂ → 2CO.
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n(C) = 4.50 g ÷ 12 g/mol.
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From chemical reaction: n(C) : n(O₂) = 2 : 1.
n(O₂) = 0.1875 mol.
T = 48°C = 321.15 K.
p = 810 mmHg ÷ 760 mmHg/atm= 1.066 atm.
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V(O₂) = n·R·T / p.
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Question
What is the purpose of the catalyst? A. to start the chemical reaction B. to stop the chemical reaction C. to speed up the chemical reaction D. to make the chemical reaction safe to observe
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Question
Ammonia (NH3(g), es001-1.jpgHf = –46.19 kJ/mol) reacts with hydrogen chloride (HCl(g), es001-2.jpgHf = –92.30 kJ/mol) to form ammonium chloride (NH4Cl(s), es001-3.jpgHf = –314.4 kJ/mol) according to this equation: NH3(g) + HCl(g) es001-4.jpg NH4Cl(s) What is es001-5.jpgHrxn for this reaction? kJ
Solution 1
Answer is: enthalpy for this reaction is -175.91 kJ.
Chemical reaction: NH₃ + HCl → NH₄Cl.
ΔrH = ∑ΔfH(products of reaction) - ∑ΔfH(reactants).
ΔrH = ΔfH(NH₄Cl) - (ΔfH(NH₃) + ΔfH(HCl)).
ΔrH = -314.4 kJ/mol · 1 mol - (-46.19 kJ/mol · 1 mol + (-92.30 kJ/mol) · 1 mol).
ΔrH = -314.4 kJ + 138.49 kJ.
ΔrH = -175.91 kJ.
Solution 2

The value of heat of the reaction for the given chemical reaction is equal to -175.91 kJ.

### How do we calculate the change in enthalpy of the reaction?

Change in enthalpy of the reaction is calculated by substracting the total sum of enthalpies of reacatnts from the the total sum of the enthalpies of products.

Given chemical reaction is:

NH₃(g) + HCl(g) → NH₄Cl(s)

According to the equation total enthalpy of the reaction calculated as:

ΔHrxn = ΔfH(NH₄Cl) - [(ΔfH(NH₃) + ΔfH(HCl)]

On putting values from the question to the equation, we get

ΔHrxn = -314.4 kJ/mol - [-46.19 kJ/mol + (-92.30 kJ/mol)]

ΔHrxn = -314.4 kJ + 138.49 kJ.

ΔHrxn = -175.91 kJ

Hence the heat of the reaction is -175.91 kJ.

To know more about total heat of reaction, visit the below link:

brainly.com/question/18721983

Question
How many molecules are in 13.5g of sulfur dioxide, so2?
Solution 1

Taking into account the definition of avogadro's number, 0.21 moles of sulfur dioxide contain 1.26482×10²³ molecules.

Avogadro's Number or Avogadro's Constant is called the number of particles that make up a substance (usually atoms or molecules) and that can be found in the amount of one mole of said substance. Its value is 6.023×10²³ particles per mole. Avogadro's number applies to any substance.

First you must determine the number of moles that 13.5 g of sulfur dioxide contains. For that, I use the molar mass of the compound, which is defined as the amount of mass that a substance contains in one mole.

In this case, the molar mass of sulfur dioxide is 64 g/mole. So the number of moles that 13.5 grams of the compound contain can be calculated as:

0.21 moles

Then you can apply the following rule of three: if 1 mole of sulfur dioxide contains 6.023×10²³ molecules, then 0.21 moles contain how many molecules of sulfur dioxide?

amount of molecules of sulfur dioxide= (6.023×10²³ molecules× 0.21 mole)÷ 1 mole

amount of molecules of sulfur dioxide=1.26482×10²³ molecules

Finally, 0.21 moles of sulfur dioxide contain 1.26482×10²³ molecules.

Solution 2
Answer is: there are 1.27·10²³ molecules of sulfur dioxide.
m(SO₂) = 13.5 g.
n(SO₂) = m(SO₂) ÷ M(SO₂).
n(SO₂) = 13.5 g ÷ 64 g/mol.
n(SO₂) = 0.21 mol.
N(SO₂) = n(SO₂) ·Na.
N(SO₂) = 0.21 mol · 6.022·10²³ 1/mol.
N(SO₂) = 1.27·10²³.
n - amount of substance.
M - molar mass of substance.
Na - Avogadro number.

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