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3 years ago

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A graduate cylinder was filled to 25.0 mL with a liquid. A solid object weighting 39.7 g was immersed in the liquid, raising the

liquid level to 33.6 mL. Calculate the density of the solid object.

1 answer:

ELEN [110]3 years ago

5 0

Answer:

184478 qreo si si es es hola

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Acid

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A 6.13 g sample of an unknown salt (MM = 116.82

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Answer:

-3.19x10³ J

Explanation:

Since the surroundings absorbed 3.19 × 10³ J (or 3190 J) of heat, the system, or the dissolution reaction, must have lost the same amount of heat. The heat for the system, then, is -3.19 × 10³ J (or -3190 J). We know this is true because of the first law of thermodynamics, "heat is a form of energy, and thermodynamic processes are therefore subject to the principle of conservation of energy".

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Consider 4.60 L of a gas at 365 mmHg and 20 C . If the container is compressed to 2.60 L and the temperature is increased to 36

BaLLatris [955]

Explanation:

The given data is as follows.

$V_{1}$ = 4.60 L, $P_{1}$ = 365 mm Hg

$V_{2}$ = 2.60 L, $P_{2}$ = ?

$T_{1}$ = (20 + 273) K = 293 K, $T_{2}$ = (36 + 273) K = 309 K

Since, number of moles of gas are equal so, according to ideal gas equation:

$\frac{P_{1}V_{1}}{T_{1}}$ = $\frac{P_{2}V_{2}}{T_{2}}$

$\frac{365 mm Hg \times 4.60 L}{293 K}$ = $\frac{P_{2} \times 2.60 L}{309 K}$

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Thus, we can conclude that new pressure $P_{2}$ is 681.03 mm Hg.

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3 years ago

A compound that contains only carbon, hydrogen, and oxygen is 58.8% C and 9.87% H by mass. What is the empirical formula of this

Dmitry [639]

<u>Answer:</u> The empirical formula of the compound becomes $C_5H_{10}O_2$

<u>Explanation:</u>

The empirical formula is the chemical formula of the simplest ratio of the number of atoms of each element present in a compound.

Let the mass of the compound be 100 g

Given values:

% of C = 58.8%

% of H = 9.87%

% of O = [100 - 58.8 - 9.87] = 31.33%

Mass of C = 58.8 g

Mass of H = 9.87 g

Mass of O = 31.33 g

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ......(1)

To formulate the empirical formula, we need to follow some steps:

<u>Step 1:</u> Converting the given masses into moles.

Molar mass of C = 12 g/mol

Molar mass of H = 1 g/mol

Molar mass of O = 16 g/mol

Putting values in equation 1, we get:

$\text{Moles of C}=\frac{58.8g}{12g/mol}=4.9 mol$

$\text{Moles of H}=\frac{9.87g}{1g/mol}=9.87 mol$

$\text{Moles of O}=\frac{31.33g}{16g/mol}=1.96mol$

<u>Step 2:</u> Calculating the mole ratio of the given elements.

Calculating the mole fraction of each element by dividing the calculated moles by the least calculated number of moles that is 1.96 moles

$\text{Mole fraction of C}=\frac{4.9}{1.96}=2.5$

$\text{Mole fraction of H}=\frac{9.87}{1.96}=5.03\approx 5$

$\text{Mole fraction of O}=\frac{1.96}{1.96}=1$

Converting the mole fraction into whole numbers by multiplying them with 2.

$\text{Mole fraction of C}=2.5\times 2=5$

$\text{Mole fraction of H}=5\times 2=10$

$\text{Mole fraction of O}=1\times 2=2$

<u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of C : H : O = 5 : 10 : 2

Hence, the empirical formula of the compound becomes $C_5H_{10}O_2$

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3 years ago

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Answer:

Balanced equation

CS2(l) + 3O2(g)------> CO2(g) + 2SO2(g)

Explanation:

For a chemical equation to be balanced, the number of atoms of each element on the left Hans side of the reaction equation must equal the number of atoms of that element on the right hand side of the reaction equation.

Atoms of oxygen are six on both sides of the reaction equation. Atoms of sulphur are two while there is only one atom of carbon on both sides of the reaction equation.

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