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3 years ago

What’s the volume of the solution?

Chemistry

1 answer:

prohojiy [21]3 years ago

8 0

Answer:

60.0 mL

General Formulas and Concepts:

Chemistry - Solutions

Reading a Periodic Table
Using Dimensional Analysis
Molarity = moles of solute / liters of solution

Explanation:

Step 1: Define

6.33 g CuNO₃

0.840 M Solution

Step 2: Identify Conversions

1 L = 1000 mL

Molar Mass of Cu - 63.55 g/mol

Molar Mass of N - 14.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of CuNO₃ - 63.55 + 14.01 + 3(16.00) = 125.56 g/mol

Step 3: Convert

$6.33 \ g \ CuNO_3(\frac{1 \ mol \ CuNO_3}{125.56 \ g \ CuNO_3} )$ = 0.050414 mol CuNO₃

Step 4: Find volume

Substitute: 0.840 M = 0.050414 mol / x L
Multiply x on both sides: (x L)(0.840 M) = 0.050414 mol
Divide M on both sides: x L = 0.060017

Step 5: Convert

$0.060017 \ L(\frac{1000 \ mL}{1 \ L} )$ = 60.0168 mL

Step 6: Check

We are given 3 sig figs. Follow sig fig rules and round.

60.0168 mL ≈ 60.0 mL

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Answer:

Explanation:

No. The demonstration does not violate the conservation of mass.

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In this case, even though the remaining bits of paper weigh 0.5 g while the original paper weighed 2.5 g, the ashes and smoke/gas from the burning will all add up to the lost weight of the paper.

The burned part has been converted into other forms. If the smoke/gas and the ashes are properly captured, they will mark up with the weight of the remaining paper to give the weight of the original paper.

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3 years ago

How many grams of SnO2 are required to produce 1.20x10^21 molecules of water?

Drupady [299]

Answer:

0.150 grams

Explanation:

The balanced chemical reaction to obtain water from SnO₂ is:

SnO₂ + 2H₂ → Sn + 2H₂O

The mole ratio is:

$\dfrac{1molSnO_2}{2molH_2O}$

Find the number of moles equivalent to 1.20× 10²¹ molecules of water, using Avogadro's number:

$1.20\times 10^{21}molecules\times \dfrac{1mol}{6.022\times 10^{23}molecules}=1.9927\times 10^{-3}moles$

From the mole ratio, the number of moles of SnO₂ are half the number of moles of water. That is:

0.0019927 moles / 2 = 0.00099635 moles of SnO₂

Use the molar mass of SnO₂ to convert the number of moles to grams:

molar mass of SnO₂ = 150.71g/mol

mass of SnO₂ = 0.00099635mol × 150.71 g/mol = 0.150 grams.

The answer must be reported with 3 significant figures.

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3 years ago

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4 years ago

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How does the vapor pressure of water at 10°C compared with its vapor pressure at 50°C ?

Sliva [168]

Answer: The vapor pressure of water at 10°C will be less as compared with its vapor pressure at 50°C.

Explanation:

Vapor pressure of a liquid is defined as the pressure exerted by the vapors in equilibrium with the liquid/solution at a particular temperature.

As Kinetic energy is dependent on the absolute temperature of the gas.

$K.E=\frac{3}{2}RT$

where R = gas constant

T = temperature

On increase in temperature, the kinetic energy of the molecules increase and thus more liquid molecules can escape to form vapours and thus will exert more vapor pressure.

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3 years ago

1. Calculate the quantity of glucose needed to prepare (a) 250 mL of a 100 mM of

weeeeeb [17]

Answer:

a. mass of glucose required = 4.50 g

b. mass of glucose required = 0.05 g

c. mass of glucose required = 25g

Explanation:

1a. molar mass of glucose = 180.156 g/mol

volume of solution = 250 mL or 250 mL * 1 L/1000 mL = 0.25 L

concentration of solution = 100 mM or 100mM * 1 M/1000 mM = 0.10 M

amount in moles = mass/ molar mass = concentration * volume

mass in grams = concentration * volume * molar mass

mass = 0.10 * 0.25 * 180.156

mass of glucose required = 4.50 g

b. mass concentration of 0.05 % solution = 0.05 g/100 ml = 0.5 g/L

volume of solution = 100 mL = 0.1 L

mass in grams = mass concentration * volume

mass in grams = 0.5 g/L * 0.1 L

mass of glucose required = 0.05 g

c. mass concentration of solution = 50 mg/ mL = 0.05 g/ 0.001 L = 50 g/L

volume of solution = 500 mL = 0.5 L

mass of solute required = concentration * volume

mass required = 50 g/L * 0.5 L

mass of glucose required = 25g

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3 years ago