A 25.0 mL sample of H2SO4 requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid?

(a) 2 Ag+ (aq) + SO42- (aq) Ag2SO4 is the balanced net ionic equation for the precipitation reaction (s)

(b) To get the mass of the precipitate, we must first determine the number of moles of Ag2SO4 that precipitated. To do this, we must subtract the mass of the dry filter paper (0.88 g) from the mass of the filter paper and precipitate right away upon filtration (4.82 g).

4.82 g of precipitation divided by 0.88 g yields 3.94 g.

The mass of the precipitate can then be converted to moles using the molar mass of Ag2SO4 (311.8 g/mol):

Ag2SO4 moles are equal to 3.94 g/311.8 g/mol, or 0.0126 moles.

(c) We must first figure out how many moles of Ag+ ions were in the original 10.00 mL solution of AgNO3 (aq) in order to compute the concentration of Ag+ there. According to the balanced net ionic equation from (a), 1 mole of AgNO3 (aq) is used for every 2 moles of Ag+ ions that precipitate. Consequently, 0.0126 moles / 2 = 0.00630 moles of Ag+ ions were present in the initial 10.00 mL solution of AgNO3 (aq).

The mass of the original solution may then be determined using the volume (10.00 mL) and density (1.01 g/mL) of the solution:

Volume x Density = 10.00 mL x 1.01 g/mL = 10.1 g Mass of Original Solution

Ag+ concentration is calculated as follows: Ag+ concentration = Ag+ moles / original solution volume (in liters) = 0.00630 moles / 0.01 L = 63.0 mol/L

(d) The mass of the filter paper was not subtracted from the total mass of the filter paper and precipitate, causing the student to overestimate the mass of the precipitate and the number of moles of Ag2SO4 that precipitated. This, in turn, led to an overestimate of the concentration of Ag+ in the original solution.

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The specific heat of the metal can be calculated using calorimetric equation. The specific heat of the metal here is 0.61 J/g °C.

The specific heat capacity of  substance is the heat energy required to raise its temperature by one degree Celsius per one gram  of the substance.

The calorimetric equation connecting the heat energy q, mass m, specific heat c and temperature difference ΔT is:

q = m c  ΔT

Here, the heat released from the metal is equal to the heat absorbed by water.

Therefore,

q metal = q water. Let c  be the specific heat of the metal.

25 g  × ( 99 - 20.15°C) ×c = 50 g  × ( 20.15°C- 14.33) × 4.18 J/g °C

                                         = 1217.5 J

Then c = 1217.5 J/25 g  × ( 99 - 20.15°C)  = 0.61 J/g °C.

Therefore, the specific heat of the metal is 0.61 J/g °C.

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Combustion of a hydrocarbon fuel in air is the reaction that is being studied. Chemicals: The two chemicals utilised in the experiment are the air and the hydrocarbon fuel. Special circumstances: Various pressures

Chemicals are substances with a particular composition and set of characteristics. They can exist as solids, liquids, gases, and even plasma, among other forms. Chemicals are essential to many sectors of the economy, including industry, healthcare, agriculture, and energy. They go into the creation of goods like plastics, fertilisers, medicines, and fuels. Chemicals can be utilised in industrial operations including material cleaning, purification, and treatment. To avoid harming both people and the environment, it's crucial to handle and utilise chemicals carefully. This covers employing personal protective equipment and handling and disposing of chemicals in the right ways. chemicals Chert, limestone, and banded iron

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Answer:

The name of this element is Nitrogen.

The atomic symbol for this element is N.

Nitrogen is a nonmetal.

The atomic number of Nitrogen is 7.

A neutral atom of Nitrogen has 7 protons.

A neutral atom of Nitrogen has 7 electrons.

The average number of neutrons in a neutral atom of Nitrogen is 7.

A neutral atom of Nitrogen has 5 valence electrons.

Assuming the atom is at ground state, or its lowest energy level, it has 2 energy levels in its electron cloud.

A Nitrogen ion is the same size as a neutral Nitrogen atom.

The charge on the monatomic ion of Nitrogen is +3.

There are 7 protons in a monatomic ion of Nitrogen.

There are 10 total electrons in a monatomic ion of Nitrogen.

There are 7 valence electrons in a monatomic ion of Nitrogen.