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2 years ago

How many moles of KF would need to be added to 2500 ml of water to make 1.2 M solution?

Chemistry

1 answer:

Oduvanchick [21]2 years ago

4 0

The number of moles of KF needed to prepare the solution is 3 moles

<h3>What is molarity?</h3>

Molarity is defined as the mole of solute per unit litre of solution. Mathematically, it can be expressed as:

Molarity = mole / Volume

<h3>How to determine the mole of KF </h3>

Volume = 2500 mL = 2500 / 1000 = 2.5 L
Molarity = 1.2 M
Mole of KF =?

Molarity = mole / Volume

1.2 = mole of KF / 2.5

Cross multiply

Mole of KF = 1.2 × 2.5

Mole of KF = 3 moles

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Cancel out CO because it appears as a reactant in one intermediate reaction and a product in the other intermediate reaction.

Explanation:

The CO appears twice hence in he intermediate reaction it only forms path of the enabling reagents and it further reacts to form the final product. Accounting for the CO in the intermediate reaction that undergoes further reaction will impact on the stoichiometry of the reaction.

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3 years ago

The pendulum has the greatest kinetic energy and no potential energy when it is _____.

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2 years ago

An ionic solid is placed in water. which information is described by the solubility product constant?

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Answer:

$\boxed{\text{C. the equilibrium between the solid and its ions in solution}}$

Explanation:

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It tells us nothing about the amount of precipitate that will form or the temperature at which the equilibrium occurs.

8 0

3 years ago

Read 2 more answers

Consider this reaction: 6 CO2 + 6 H2O + light equation C6H12O6 + 6 O2 If there were 2.38 x 102 g of H2O, 18.6 moles of CO2, and

alisha [4.7K]

H₂O would be the limiting reactant.

Balanced chemical equation:

6CO₂ + 6H₂O + light equation → C₆H₁₂O₆ + 6O₂

The amount of product that can be created is constrained by the reactant that is consumed first in a chemical reaction, commonly referred to as the limiting reactant (or limiting reagent).

Given

No. of moles of CO₂ = 18.6

Mass of H₂O = 2.38 × 10² g = 238g

No. of moles of H₂O = Given mass/ Molar mass

= 238 / 18 = 13.22 moles

Moles of H₂O = 13.22

According to the balanced chemical equation

6 moles of CO₂ react with 6 moles of H₂O

So the reactant that has less number of moles will be consumed first.

As the No. of moles of H₂O < No. of moles of CO₂

So, H₂O is the limiting reactant with 13.22 moles.

Hence, H₂O would be the limiting reactant.

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7 0

2 years ago

What is the pressure inside a 2.0 L bottle filled with 0.25 mol of carbon dioxide gas at 25 °C?

motikmotik

Answer:

3.1atm

Explanation:

Given parameters:

Volume of gas = 2L

Number of moles = 0.25mol

Temperature = 25°C = 25 + 273 = 298K

Unknown:

Pressure of the gas = ?

Solution:

To solve this problem, we use the ideal gas equation.

This is given as;

PV = nRT

P is the pressure

V is the volume

n is the number of moles

R is the gas constant = 0.082atmdm³mol⁻¹K⁻¹

T is the temperature

P = $\frac{nRT}{V}$

Now insert the parameters and solve;

P = $\frac{0.25 x 0.082 x 298}{2}$ = 3.1atm

8 0

3 years ago