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3 years ago

How many grams of water are produced if we react 3 moles of hydrogen with 3 moles of oxygen?

Chemistry

1 answer:

Thepotemich [5.8K]3 years ago

4 0

Answer:

About 60 grams

Explanation:

The balanced equation of the reaction is given as;

2H2(g) + O2(g) → 2H2O(l)

From the equation;

2 mol of H2 reacts with 1 mol of O2

3 mol of H2 would require 3/2 mol of O2 (considering the 2:1 ratio)

The limiting reactant is H2 as it would be used up before H2. It determines the amount of product that would be formed.

2 mol of H2 produces 2 mol of H2O

3 mol of H2 would produce 3 mol of H2O (Considering the 1 : 1 ratio)

Converting moles to mass;

Mass = Molar mass * Number of moles

Mass = 18 * 3 = 54 g

The correct option is; About 60 grams

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3 years ago

Calcular la cantidad de NaOH necesaria para preparar medio litro de disolución 2,5 N. (Dato: peso molecular del NaOH = 40 g/mol)

kolbaska11 [484]

Answer:

The amount of NaOH required to prepare a solution of 2.5N NaOH.

The molecular mass of NaOH is 40.0g/mol.

Explanation:

Since,

NaOH has only one replaceable -OH group.

So, its acidity is one.

Hence,

The molecular mass of NaOH =its equivalent mass

Normality formula can be written as: $Normality=\frac{mass of solute NaOH}{its equivalent mass} * \frac{1}{volume of solution in L} \\$

Substitute the given values in this formula to get the mass of NaOH required.

$2.5N=\frac{mass of NaOH}{40g/mol} *\frac{1}{1L} \\mass of NaOH=2.5N*40gmol\\ = 100.0g$

Hence, the mass of NaOH required to prepare 2.5N and 1L. solution is 100g

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3 years ago

Which equation will you use to calculate the volume of a 5.00 liter sample of air at 50°C when it is warmed to 100°C at constant

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3 years ago

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Which of the following methods can be used to completely separate a solution containing alcohol and water?

Alenkinab [10]

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4 years ago

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What mass of metallic silver can form from 1.147 g of copper metal according to equation b?

Arisa [49]

Answer:

$\large\boxed{\large\boxed{3.894g}}$

Explanation:

From similar question, equation (b) is

Molecular Equation:

Cu(s) + 2AgNO₃(aq) → Cu(NO₃)₂(aq) + 2Ag(s)

Net Ionic Equation:

Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

1. Mole ratio:

$\dfrac{2molAg(s)}{1molCu(s)}$

2. Convert 1.147 g of Cu(s) to moles:

Atomic mass of Cu: 63.546g/mol

Number of moles = mass in grams / atomic mass

Number of moles = 1.147 g / 63.546 g/mol = 0.01805 mol Cu(s)

3. Calculate the moles of Ag(s):

$0.01805molCu(s)\times \dfrac{2molAg(s)}{1molCu(s)}=0.03610molAg(s)$

4. Convert 0.03610 mol Ag(s) to grams:

Atomic mass of Ag(s) = 107.868g/mol

Mass = 0.03610mol × 107.868g/mol = 3.894g

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3 years ago