The statement that best describes the variables in a controlled experiment is independent variable while all other conditions are unchanged.
<h3>What is an experiment?</h3>
An experiment is a scientific research, findings or investigation about a subject matter with the aim of validating a claim and establishing theories.
A controlled experiment refers to an experiment in which the variables involved and the control factor are kept in the same group except for one variable which can be changed.
Therefore, The statement that best describes the variables in a controlled experiment is independent variable while all other conditions are unchanged.
Learn more about experiment below.
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Answer:
Average amu is 6.52556
Explanation:
Average the numbers
Add the two masses together.
6.01512+ 7.01600= 13.03112
Then divide by 2, we divide by 2 because that is how many #'s we are given.
13.03112/ 2= 6.52556
I believe the correct answer from the choices listed above is the third option. It would be chromium (Cr) that is a transition metal. The 38 elements in groups 3 through 12 of the periodic table are called "transition metals<span>". Hope this answers the question. Have a nice day.</span>
Answer:
2.4 g
Explanation:
Step 1: Given data
- Initial pressure (P₁): 755 torr
- Final pressure (P₂): 1.87 atm
Step 2: Convert "P₁" to atm
We will use the conversion factor 1 atm = 760 torr.
755 torr × 1 atm/760 torr = 0.993 atm
Step 3: Convert "T" to K
We will use the following expression.
K = °C + 273.15
K = 25°C + 273.15 = 298 K
Step 4: Calculate the initial number of moles of He
We will use the ideal gas equation.
P₁ × V = n₁ × R × T
n₁ = P₁ × V/R × T
n₁ = 0.993 atm × 16.8 L/(0.0821 atm.L/mol.K) × 298 K
n₁ = 0.682 mol
Step 5: Calculate the final number of moles of He
We will use the ideal gas equation.
P₂ × V = n₂ × R × T
n₂ = P₂ × V/R × T
n₂ = 1.87 atm × 16.8 L/(0.0821 atm.L/mol.K) × 298 K
n₂ = 1.28 mol
Step 6: Calculate the moles of He added
n = n₂ - n₁
n = 1.28 mol - 0.682 mol
n = 0.60 mol
Step 7: Convert "n" to mass
The molar mass of He is 4.00 g/mol
0.60 mol × 4.00 g/mol = 2.4 g
