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2 years ago

Physical science:verification on newton's second law

Chemistry

1 answer:

mezya [45]2 years ago

6 0

Explanation:

finally I have given you answer hope it will help you successfully

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The vapor pressure of water is 23.76 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in water is sucrose. Calculate

MrRissso [65]

Answer : The vapor pressure of solution is 23.67 mmHg.

Solution:

As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

$\frac{p^o-p_s}{p^o}=\frac{w_2M_1}{w_1M_2}$

where,

$p^o$ = vapor pressure of pure solvent (water) = 23.76 mmHg

$p_s$ = vapor pressure of solution= ?

$w_2$ = mass of solute (sucrose) = 12.25 g

$w_1$ = mass of solvent (water) = 176.3 g

$M_1$ = molar mass of solvent (water) = 18.02 g/mole

$M_2$ = molar mass of solute (sucrose) = 342.3 g/mole

Now put all the given values in this formula ,we get the vapor pressure of the solution.

$\frac{23.76-p_s}{23.76}=\frac{12.25\times 18.02}{176.3\times 342.3}$

$p_s=23.67mmHg$

Therefore, the vapor pressure of solution is 23.67 mmHg.

7 0

3 years ago

Calculate the volume of 1.00 x 10^-2M KOH solution containing 3.00 x 10^-1 mol of solute?

ioda

Volume = ?

Molarity (M) = 1.00 x 10⁻² M

moles (n) = 3.00 x 10⁻¹ mol

V = n / M

V = 3.00 x 10⁻¹ / 1.00 x 10⁻²

V = 30 L

7 0

4 years ago

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(I

ale4655 [162]

Answer:

The answer is "6.52 kg and 13.1 kg"

Explanation:

For point a:

$Actual\ yield = 6.52 \ kg\\\\Percent \ yield= 66\%\\\\Percent \ yield = \frac{Actual \ yield}{Theoretical\ yield} \times 100 \%\\\\Theoretical\ yield \ of \ MnO_2 = \frac{Actual \ yield}{Percent \ yield} \times 100\%\\\\=\frac{6.52 \ kg}{66 \%} \times 100\% =9.88 \ kg\\\\$

Equation:

$3MnCO_3 +O_2 \longrightarrow 2MnO_2 + 2CO_2\\\\$

Calculating the amount of $MnCO_3$

$= 9.88 \ kg \times \frac{1000 \ g}{1 \ kg} \times \frac{1 \ mol \ MnO_2}{86.94 \ g} \times \frac{2 \ Mol \ MnCO_3}{2 \ mol \ MnO_2} \times \frac{114.95\ g}{1 \ mol \ MnCO_3 }\times \frac{1\ kg}{1000\ g}\\\\= 13.1 \ kg$

For point b:

$Actual\ yield = 4.0 \ kg\\\\Percent\ yield=97.0\%\\\\Percent \ yield = \frac{Actual \ yield}{Theoretical \ yield} \times 100 \% \\\\Theoretical \ yield\ of\ Mn = \frac{Actual \ yield}{Percent \ yield} \times 100\%\\\\$

$=\frac{4.0 \ kg}{97.0\%} \times 100\% =4.12 \ kg$

Equation:

$3MnO_2 +4AL \longrightarrow 3Mn + 2AL_2O_3\\\\$

Calculating the amount of $MnO_2:$

$= 4.12 \ kg \times \frac{1000 \ g}{1 \ kg} \times \frac{1 \ mol \ Mn}{54.94 \ g} \times \frac{3 \ Mol \ MnO_2}{3 \ mol \ Mn} \times \frac{86.94 \ g}{1 \ mol \ MnO_2 }\\\\= 6516 \ g \\\\=6.52 \ kg\\\\$

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3 years ago

Is the cause of rapid oxidation explosion

melamori03 [73]

Rapid oxidation results in burning of a material or even an explosion. It happens rapidly and produces light and noticeable heat. Combustion or burning is rapid oxidation. But combustion can also refer to rapid burning where oxygen is not involved

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3 years ago

The less blank, the more carbon monoxide will be produced

chubhunter [2.5K]

FUELS,GAS,HEATERS, AND FIRES cause carbon monoxide

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3 years ago