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kotegsom [21]
3 years ago
13

How could using either more or less of a chemical in a scientific experiment cause a change in results?

Chemistry
1 answer:
MakcuM [25]3 years ago
7 0
More chemicals can cause faster reactions/ results.
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A 28.5 gram piece of iron is added to a graduated cylinder containing 45.5 mL of water. The water in the cylinder rises to the 4
yan [13]

7.91 g/ml is the density of the iron piece of 28.5 gms.

Explanation:

The density of a substance is defined as the volume it occupies.  It tells the matter present in a substance.

The density is mass per unit volume and is denoted by p.

The formula for density is given by:

density (p) = \frac{mass}{volume}

Data given is :

mass= 28.5 grams

V1 = 45.5 ml

V2= 49.1 ml

The initial volume of water was 45.5 ml, when iron piece of 28.5 grams was added the final volume was 49.1 ml.

Putting the values in the equation of density

p = \frac{28.5}{49.1-45.5}

p = 7.91 g/ml

Since iron is a dense material it will occupy less volume

4 0
3 years ago
Can you help me with three please? We’re balancing electrons
Aneli [31]

Answer:

Explanation:

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4 0
2 years ago
An aqueous solution contains 32.7% KCl (wt/wt%). what is the mole fraction of KCl in the solution
inna [77]

The mole fraction of KCl in the solution is 0.1051

calculation

mole fraction of KCl in solution = moles of KCl / total number of moles(moles of KCl +moles of H2O)

moles=mass/molar mass

mass of KCl=32.7g

molar mass of KCl= 39 +35.5

moles of KCl is therefore= 32.7g/74.5 g/mol=0.439 moles

find the moles of H2O= mass of H2O/molar mass

mass of H2O=100-32.7=67.3g

molar mass of H2O=( 1 x2) +16=18 g/mol

moles = 67.3/18 =3.739 moles

total moles=3.739+0.439=4.178 moles

mole fraction is therefore=0.439/4.178=0.1051

5 0
3 years ago
Which one of these statements best describes what a scientist is
son4ous [18]
Which of what statements
3 0
3 years ago
The two balanced equations (1) and (2) are for reactions in which gaseous carbon dioxide is produced from the combustion of (1)
V125BC [204]

Answer:

2.0 mol of oxygen are consumed.

Step-by-step explanation:

You know that you will need a balanced equation with masses, moles, and molar masses, so gather all the information in one place.

M_r:   28.0                 44.0

          CO  + ½O₂ ⟶ CO₂ + 67.6 kcal

m/g:   112

<em>Step 1</em>. Convert grams of CO to moles of CO

1 mol CO = 28.0 g CO

Moles of CO = 112 × 1/28.0

<em>Step 2.</em> Convert moles of CO to moles of CO₂.

The molar ratio is 1 mol CO₂ to 1 mol CO

Moles of CO₂ = 4.000 × 1/1

Moles of CO₂ = 4.00 mol CO₂

Option A is <em>wrong</em>.

<em>Step 3.</em> Calculate the amount of heat generated.

q = ΔH

The conversion factor is 67.6 kcal/1 mol CO₂

q = 4.00 × 67.6

q = 270 kJ

Option B is <em>wrong</em>, because it gives the heat generated by 1 mol of CO.

<em>Step 4. </em>Calculate the moles of O₂ consumed

Moles of O₂ = 2.00 mol O₂

Option C is correct.

<em>Step 5.</em> Calculate the moles of CO₂ formed

Already done in Step 2.

Moles of CO₂ = 4.00 mol CO₂

Option D is <em>wrong. </em>

<em> </em>

<em>Step 6</em>. Calculate the moles of O₂ produced

Already done in Step 4.

Moles of O₂ = 2.00 mol O₂

Option E is <em>wrong. </em>

3 0
3 years ago
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