What is the main intermolecular force in H2CO?(dipole dipole, hydrogen bond, London dispersion,polar/nonpolar)

The right response is that, Using the 0.200 M KBr solution, about 43.31 mL should be mixed with water to create a 0.0495 M solution with a volume of 175.0 mL.

175.0 mL is the final volume needed for a 0.0495 M solution. To achieve this, we can use the dilution formula and calculate the amount of 0.200 M KBr solution necessary.

V2C2 is equivalent to V1C1, as depicted by the formula C1V1 = C2V2.

Where:

Starting at 0.200 M, C1 indicates the concentration of the solution.

Unknown is the designation for the volume of the first solution that will be used.

The diluted solution's final volume is V2, and its ultimate concentration is marked as C2 (0.0495 M).

To determine V1, rewrite the equation as V1 = (C2 * V2) / C1.

Based on these values:

V2 is 175.0 mL, C1 is 0.200 M, and C2 is 0.0495 M.

Enter the corresponding values to establish V1:

= (0.0495 * 175.0) / 0.200 V1 = 43.3125 mL

You would need around 43.31 mL of the 0.200 M KBr solution to make a 0.0495 M solution (rounded to two decimal places) when diluted to 175.0 mL with water.

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Final answer:

To prepare a 0.0495 M solution of KBr by dilution to 175.0 mL with water, you would need 2.744 mL of 0.200 M KBr solution.

Explanation:

When diluting a solution, the equation M1V1 = M2V2 holds true, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume. In this case, the final concentration (M2) is 0.0495 M, and the final volume (V2) is 175.0 mL.

Rearranging the equation to solve for V1, the initial volume of the concentrated solution needed, we have:

V1 = (M2 * V2) / M1

Substituting the given values:

V1 = (0.0495 M * 175.0 mL) / 0.200 M

V1 ≈ 43.3125 mL

This means you need 43.3125 mL of the 0.200 M KBr solution to achieve a concentration of 0.0495 M. However, since you have the concentrated solution at 0.200 M, you can dilute it further. The volume you take from the concentrated solution (V1) and the volume of water you add (V_water) should sum up to the final volume of 175.0 mL:

V1 + V_water = 175.0 mL

Rearranging to find V_water:

V_water = 175.0 mL - V1

V_water ≈ 175.0 mL - 43.3125 mL

V_water ≈ 131.6875 mL

So, you would take 43.3125 mL of the 0.200 M KBr solution and dilute it with approximately 131.6875 mL of water to get a total volume of 175.0 mL, resulting in a final concentration of 0.0495 M.

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The answer is has a Moh's hardness of 1.

The amount of heat that is released by the chemical reaction of 25.0 g of with water is -20.223 Joules.

Given the following data:

• Mass of  = 25.0 grams

• Enthalpy of combustion = -126 kJ/mol

To find the amount of heat that is released by the chemical reaction of 25.0 g of with water:

First of all, we would determine the number of moles of  in this chemical reaction:

                ------>

Substituting the values into the formula, we have;

Number of moles () = 0.321 moles.

Now, we can find the quantity of heat released when reacts with water:

2 mole of   = -126 kJ/mol

0.321 mole of   = X kJ/mol

Cross-multiplying, we have:

×

X = -20.223 Joules.

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Answer : The amount of heat released by the reaction is, 20.2 kJ

Explanation :

First we have to calculate the number of moles of .

Molar mass of = 77.98 g/mole

Now we have to calculate the heat released during the reaction.

The balanced chemical reaction is:

From the reaction we conclude that,

As, 2 moles of releases heat = 126 kJ

So, 0.320 moles of releases heat =

Therefore, the amount of heat released by the reaction is, 20.2 kJ

Final answer:

A balanced chemical equation shows that mass is not lost or gained in a chemical reaction by ensuring the number of atoms and overall charge on both the reactants and products side are equal, adhering to the law of conservation of mass.

Explanation:

A balanced chemical equation is one where the number of each type of atom in the reactants side is equivalent to the number of the same type of atoms in the products side. In chemical reactions, matter cannot be created or destroyed, a principle called the law of conservation of mass. This means that all the atoms present in the reactants will be accounted for in the products, ensuring that mass is never lost or gained during the reaction process.

For instance, if we take the simple chemical reaction of hydrogen and oxygen forming water (2H2 + O2 → 2H2O), you'll see that there are four hydrogen atoms and two oxygen atoms both before and after the reaction, thus demonstrating mass conservation. Additionally, in balanced chemical equations, not only should atoms be balanced, but also charges to ensure charge conservation which is necessary when dealing with ionic substances. The mass balance and charge balance are both instrumental in maintaining the law of conservation of mass in chemical reactions.

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Answer:The answer is "It has five valence electrons available for bonding". An element's group number is equivalent to the number of valence electrons that it has. This means that since phosphorus is found on group number 5, it has 5 valence electrons that participate in bonding. It also means that it needs 3 more electrons to complete its valency.

Final answer:

There are approximately 1.0545 x 10^24 atoms in 1.75 mole of CHCl3.

Explanation:

To calculate the number of atoms in 1.75 mole of CHCl3, we need to use Avogadro's number, which is 6.02 x 10^23 atoms per mole. The atomic mass of CHCl3 can be calculated by adding up the atomic masses of its constituent atoms. Carbon has an atomic mass of 12.01 g/mol, hydrogen has 1.01 g/mol, chlorine has 35.45 g/mol, and there are 3 chlorine atoms in CHCl3. So, the total atomic mass of CHCl3 is 12.01 + (1.01 x 3) + 35.45 = 119.48 g/mol. Therefore, 1.75 mole of CHCl3 contains (1.75 mol) x (6.02 x 10^23 atoms/mol) = 1.0545 x 10^24 atoms.

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Final answer:

To find the number of atoms in 1.75 moles of CHCl3, multiply 1.75 moles by Avogadro's number, then by the number of atoms per CHCl3 molecule to get approximately 5.26925 × 10^24 atoms.

Explanation:

To calculate the number of atoms in 1.75 moles of CHCl3, we'll follow a few simple steps. First, remember that 1 mole of any substance contains Avogadro's number of particles, which is 6.022 × 10^23 particles/mole. The formula CHCl3 consists of 1 atom of carbon, 1 atom of hydrogen, and 3 atoms of chlorine for a total of 5 atoms per molecule.

So, if we have 1.75 moles of CHCl3, we can multiply this by Avogadro's number to find the number of molecules:

1.75 moles × 6.022 × 102^3 molecules/mole = 1.05385 × 10^24 molecules of CHCl3

Then, we multiply the total number of molecules by the number of atoms per molecule:

1.05385 × 10^24 molecules × 5 atoms/molecule =

5.26925 × 10^24 atoms

Therefore, there are approximately 5.26925 × 10^24 atoms in 1.75 moles of CHCl3.

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