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jasenka [17]
3 years ago
11

During an experiment, 104 grams of calcium carbonate reacted with an excess amount of hydrochloric acid. If the percent yield of

the reaction was 80.15%, what was the actual amount of calcium chloride formed? CaCO3 + HCl → CaCl2 + CO2 + H2O 90.1 grams 92.4 grams 109.2 grams 115.3 grams
Chemistry
1 answer:
postnew [5]3 years ago
7 0

Answer:

92.4 grams.

Explanation:

  • From the balanced reaction:

<em>CaCO₃ + 2HCl → CaCl₂ + CO₂ + H₂O,</em>

1.0 mole of CaCO₃ reacts with 2.0 moles of HCl to produce 1.0 mole of CaCl₂, 1.0 mole of CO₂, and 1.0 mole of H₂O.

  • We need to calculate the no. of moles of (104 g) of CaCO₃:

<em>no. of moles of CaCO₃ = mass/molar mass</em> = (104 g)/(100.08 g/mol) = <em>1.039 mol.</em>

<u><em>Using cross multiplication:</em></u>

1.0 mole of CaCO₃ produce → 1.0 mole of CaCl₂.

∴ 1.039 mole of CaCO₃ produce → 1.039 mole of CaCl₂.

∴ The amount of CaCl₂ produced = no. of moles x molar mass = (1.039 mol)(110.98 g/mol) = 114.3 g.

∵ percent yield of the reaction = [(actual yield)/(theoretical yield)] x 100.

Percent yield of the reaction = 80.15%, theoretical yield = 115.3 g.

<em>∴ actual yield = [(percent yield of the reaction)(theoretical yield)]/100 </em>= [(80.15%)/(115.3 g)] / 100 = <em>92.42 g ≅ 92.4 g.</em>

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stellarik [79]

Answer:

The percent by mass of water in this crystal is:

  • <u>21.4%</u>

Explanation:

This exercise can be easily solved using a simple rule of three where the initial weight of the hydrated crystal (6,235 g) is taken into account as 100% of the mass, and the percentage to which the mass of 4.90 g corresponds (after getting warm). First, the values and unknown variable are established:

  • 6,235 g = 100%
  • 4.90 g = X

And the value of the variable X is found:

  • X = (4.90 g * 100%) / 6,235 g
  • X = approximately 78.6%.

The calculated value is not yet the percentage of the water, since the water after heating the glass has evaporated, therefore, the remaining percentage must be taken, which can be calculated by subtraction:

  • Water percentage = Total percentage - Percentage after heating.
  • <u>Water percentage = 100% - 78.6% = 21.4%</u>
4 0
3 years ago
Read 2 more answers
how much heat, in terms in q, would it take to produce the change in temperature indicated in the picture? what is your reasonin
STALIN [3.7K]

Answer:

1. q.

2. 2q.

3. 3q.

4. 6q.

Explanation:

We'll begin by calculating the specific heat capacity of the liquid. This can be obtained as follow:

Mass (m) = 25 g

Change in temperature (ΔT) = 20 °C

Heat (Q) = q

Specific heat capacity (C) =?

Q = MCΔT

q = 25 × C × 20

q = 500C

Divide both side by 500

C = q/500

C = 2×10¯³ qg°C

Therefore, the specific heat capacity of liquid is 2×10¯³ qg°C

Now, we shall determine the heat required to produce the various change in temperature as follow:

2. Mass (m) = 50 g

Change in temperature (ΔT) = 20 °C

Specific heat capacity (C) = 2×10¯³ qg°C

Heat (Q) =?

Q = MCΔT

Q = 50 × 2×10¯³ × 20

Q = 2q.

Therefore, the heat required is 2q.

3. Mass (m) = 25 g

Change in temperature (ΔT) = 60 °C

Specific heat capacity (C) = 2×10¯³ qg°C

Heat (Q) =?

Q = MCΔT

Q = 25 × 2×10¯³ × 60

Q = 3q.

Therefore, the heat required is 3q.

4. Mass (m) = 50 g

Change in temperature (ΔT) = 60 °C

Specific heat capacity (C) = 2×10¯³ qg°C

Heat (Q) =?

Q = MCΔT

Q = 50 × 2×10¯³ × 60

Q = 6q.

Therefore, the heat required is 6q.

4 0
3 years ago
Calculate the [oh] for 0.46 Hcl
Bad White [126]

Answer:

2.17 e -14

Explanation:

A strong acid like HCl ionize 100 % in water so [H3O+] = 0.46 M

[OH-] = Kw /  [H3O+]

        =  1.0 e -14 / 0.46

         = 2.17 e -14

3 0
3 years ago
PLEASE HELPPPP???!!!!!!
sertanlavr [38]
Mass of molecule (g) = Mr of substance over avarogado constant
5 0
3 years ago
Which of the following is not an example of a polymer?
Nady [450]
I believe the correct answer from the choices listed above is the third option. It is amino acid that is not an example of a polymer. It <span> is a large molecule, or macromolecule, composed of many repeated subunits. Hope this answers the question.</span>
7 0
3 years ago
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