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3 years ago

A mixture contains 3.64g nacl, 2.87g nh4cl, and 4.13g of sio2. what is the percent by mass of nh4cl

1 answer:

8 0

<span>Total mass = 3.64 + 2.87 + 4.13 = 10.64 g Mass percent of NH4Cl = (mass of NH4Cl/ Total mass) x 100 = (2.87 g/10.64g) x 100 = 27.0 % mass of NH4Cl</span>

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6. How many moles of water would require 92.048 kJ of heat to raise its temperature from 34.0 °C to 100.0 °C? (3 marks)

scoray [572]

Taking into account the definition of calorimetry, 0.0185 moles of water are required.

<h3>Calorimetry</h3>

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).

So, the equation that allows to calculate heat exchanges is:

Q = c× m× ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

<h3>Mass of water required</h3>

In this case, you know:

Heat= 92.048 kJ
Mass of water = ?
Initial temperature of water= 34 ºC
Final temperature of water= 100 ºC
Specific heat of water = 4.186 $\frac{J}{gC}$

Replacing in the expression to calculate heat exchanges:

92.048 kJ = 4.186 $\frac{J}{gC}$ × m× (100 °C -34 °C)

92.048 kJ = 4.186 $\frac{J}{gC}$ × m× 66 °C

m= 92.048 kJ ÷ (4.186 $\frac{J}{gC}$ × 66 °C)

<u><em>m= 0.333 grams</em></u>

<h3>Moles of water required</h3>

Being the molar mass of water 18 $\frac{g}{mole}$ , that is, the amount of mass that a substance contains in one mole, the moles of water required can be calculated as:

$amount of moles=0.333 gramsx\frac{1 mole}{18 grams}$

<u><em>amount of moles= 0.0185 moles</em></u>

Finally, 0.0185 moles of water are required.

Learn more about calorimetry:

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8 0

2 years ago

I need some help!!! Asap

miss Akunina [59]

Answer:

Al2O3 + 6HCl --> 2AlCl3 + 3H2O

Explanation:

Al: 2

O: 3

H: 6

Cl: 6

Balanced on both sides.

8 0

3 years ago

The steps required to prepare 200.0 mL of an aqueous solution of iron (III) chloride, at a concentration of 1.25x10^-2 M. Please

Yanka [14]

Answer:

In order to prepare 200.0 mL of an aqueous solution of iron (III) chloride, at a concentration of 1.25 x 10⁻² M, you need to weight 0.4055 g of FeCl₃ and add to 200.0 mL of water.

Explanation:

Concentration: 1.25 x 10⁻² M

1,25 x 10⁻² mol FeCl₃ ___ 1000 mL

x ___ 200.0 mL

x = 2.5 x 10⁻³ mol FeCl₃

Mass of FeCl₃:

1 mol FeCl₃ _____________ 162.2 g

2.5 x 10⁻³ mol FeCl₃ _______ y

y = 0.4055 g FeCl₃

8 0

3 years ago

What is the molality of a solution made by dissolving 50.00 g of glucose, C6H12O6, in 500.0 g water. Give your answer to 3 signi

hichkok12 [17]

Answer:

m = 0.5556 mol/kg

Explanation:

The molality of any solution is calculated using the following expression:

m = moles solute / kg solvent (1)

So in order to calculate the molality of this solution, we need to calculate the moles of the glucose using the expression:

n = mass / molecular weight (2)

The molecular weight of glucose, can be calculated using the molecular mass of the atoms in the glucose:

C = 12 g/mol; H = 1 g/mol; O = 16 g/mol

the molecular weight is:

MW = (12*6) + (12*1) + (6*16) = 180 g/mol

Then, the moles of glucose:

moles = 50 / 180 = 0.2778 moles

The solvent in this case is water, and 500 g of water is 0.5 kg of water, so the molality is:

m = 0.2778 / 0.5

m = 0.5556 mol/kg

5 0

2 years ago

How do you increase the concentration of a solution wiki?

never [62]

It would be to change the amount of solute or solvent in the solution.

4 0

3 years ago