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3 years ago

Someone help me with this plz due in 10 minutes ILl give brainly!!!

Chemistry

1 answer:

user100 [1]3 years ago

7 0

Answer:

which one do u want help with?

Explanation:

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Calculate the number of moles of solute present and the number of grams

nekit [7.7K]

Answer:

The answer is: 18 moles and 1341, 72 grams of KCl

Explanation:

The molarity is defined as the moles of solute ( in this case KCl) in 1 liter of solution:

1L solution-----3 moles of KCl

6L solution-----x= (6L solutionx 3 moles of KCl)/1 L solution= 18 moles of KCl

We calculate the weight of 1 mol of KCl:

Weight 1 mol KCl= Weight K + Weight Cl= 39,09 g + 35, 45 g=74, 54 g/mol

1 mol KCl----- 74, 54 g

18 mol KCl----x= (18 mol KCl x 74, 54 g)/1 mol KCl=1341, 72 g

6 0

4 years ago

Iron has a density of 7.86 g/cm3 (1 cm3=1 mL). Calculate the volume (in dL) of a piece of iron having a mass of 4.84 kg . Note t

Marrrta [24]

1 kg ---------- 1000 g
4.84 kg ------ ?

4.84 x 1000 / 1 => 4840 g

D = m / V

7.86 =4840 / V

V = 4840 / 7.86

V = 615.77 cm³

1 cm³ ------------ 0.01 dL
615.77 ----- ?

615.77 x 0.01 / 1

= 6.1577 dL

6 0

4 years ago

3. KMnO4 name compound

dimaraw [331]

Potassium Peramanganate .

The equation is followed as

$\\ \ast\sf\hookrightarrow {K\atop Potassium}+{MnO_4\atop Manganeese\:Oxide}\longrightarrow {KMnO_4\atop Potassium\:Peramanganete}$

5 0

3 years ago

Ammonia is a? Base Acid Ketone Ester

BaLLatris [955]

Answer:

it is a base

Explanation:

8 0

3 years ago

A 23.0-mL volume of O2, collected over water at 752 torr and 22Â°C, is produced from the thermal decomposition of KClO3. The vap

arsen [322]

Answer:

$9.14\times 10^{-4}$ moles

Explanation:

We are given:

Vapor pressure of water = 19.8 torr

Total vapor pressure = 752 torr

Vapor pressure of oxygen gas = Total vapor pressure - Vapor pressure of water = (752 - 19.8) torr = 732.2 torr

To calculate the amount of oxygen gas collected, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 732.2 torr

The conversion of P(torr) to P(atm) is shown below:

$P(torr)=\frac {1}{760}\times P(atm)$

So,

Pressure = 732.2 / 760 atm = 0.9634 atm

V = Volume of the gas = 23 mL = 0.023 L

T = Temperature of the gas = $22^oC=[22+273]K=295K$

R = Gas constant = $0.0821 L.atm/K.mol$

n = number of moles of oxygen gas = ?

Applying the equation as:

0.9634 atm × 0.023 L = n × 0.0821 L.atm/K.mol × 295.15 K

⇒n = $9.14\times 10^{-4}$ moles

3 0

4 years ago