Filling in the blanks, the full sentence is: Robert Boyle made the biggest impact on science by <span>writing out the scientific method for all of science.
</span><span>
The scientific method is the standard method of knowledge pursuit.</span><span> It involves careful observations,</span><span> formulating </span>hypotheses<span> (based on observations); preparation of </span>experimental<span> testing, and the measurement and interpretation of results</span>.
Answer:
ive been there before but im not from there
Explanation:
Answer:
![\boxed{\text{Q1. 3.6 g; Q2. 0.2 A}}](https://tex.z-dn.net/?f=%5Cboxed%7B%5Ctext%7BQ1.%203.6%20g%3B%20Q2.%200.2%20A%7D%7D)
Explanation:
Q1. Mass of Cu
(a) Write the equation for the half-reaction.
Cu²⁺ + 2e⁻ ⟶ Cu
The number of electrons transferred (z) is 2 mol per mole of Cu.
(b) Calculate the number of coulombs
q = It
![\text{t} = \text{1.0 h} \times \dfrac{\text{3600 s}}{\text{1 h}} = \text{3600 s}\\\\q = \text{3 C/s} \times \text{ 3600 s} = \textbf{10 800 C}](https://tex.z-dn.net/?f=%5Ctext%7Bt%7D%20%3D%20%5Ctext%7B1.0%20h%7D%20%5Ctimes%20%5Cdfrac%7B%5Ctext%7B3600%20s%7D%7D%7B%5Ctext%7B1%20h%7D%7D%20%3D%20%5Ctext%7B3600%20s%7D%5C%5C%5C%5Cq%20%3D%20%5Ctext%7B3%20C%2Fs%7D%20%5Ctimes%20%5Ctext%7B%203600%20s%7D%20%3D%20%5Ctextbf%7B10%20800%20C%7D)
(c) Mass of Cu
We can summarize Faraday's laws of electrolysis as
![\begin{array}{rcl}m &=& \dfrac{qM}{zF}\\\\& = &\dfrac{10 800 \times 63.55}{2 \times 96 485}\\\\& = & \textbf{3.6 g}\\\end{array}\\\text{The mass of Cu produced is $\boxed{\textbf{3.6 g}}$}](https://tex.z-dn.net/?f=%5Cbegin%7Barray%7D%7Brcl%7Dm%20%26%3D%26%20%5Cdfrac%7BqM%7D%7BzF%7D%5C%5C%5C%5C%26%20%3D%20%26%5Cdfrac%7B10%20800%20%5Ctimes%2063.55%7D%7B2%20%5Ctimes%2096%20485%7D%5C%5C%5C%5C%26%20%3D%20%26%20%5Ctextbf%7B3.6%20g%7D%5C%5C%5Cend%7Barray%7D%5C%5C%5Ctext%7BThe%20mass%20of%20Cu%20produced%20is%20%24%5Cboxed%7B%5Ctextbf%7B3.6%20g%7D%7D%24%7D)
Note: The answer can have only two significant figures because that is all you gave for the time.
Q2. Current used
(a) Write the equation for the half-reaction.
Ag⁺ + e⁻ ⟶ Ag
The number of electrons transferred (z) is 1 mol per mole of Ag.
(a) Calculate q
![\begin{array}{rcl}m &=& \dfrac{qM}{zF}\\\\2.00& = &\dfrac{q \times 107.87}{1 \times 96 485}\\\\q &=& \dfrac{2.00 \times 96485}{107.87}\\\\& = & \textbf{1789 C}\\\end{array}](https://tex.z-dn.net/?f=%5Cbegin%7Barray%7D%7Brcl%7Dm%20%26%3D%26%20%5Cdfrac%7BqM%7D%7BzF%7D%5C%5C%5C%5C2.00%26%20%3D%20%26%5Cdfrac%7Bq%20%5Ctimes%20107.87%7D%7B1%20%5Ctimes%2096%20485%7D%5C%5C%5C%5Cq%20%26%3D%26%20%5Cdfrac%7B2.00%20%5Ctimes%2096485%7D%7B107.87%7D%5C%5C%5C%5C%26%20%3D%20%26%20%5Ctextbf%7B1789%20C%7D%5C%5C%5Cend%7Barray%7D)
(b) Calculate the current
t = 3 h = 3 × 3600 s = 10 800 s
![\begin{array}{rcl}q&=& It\\1789 & = & I \times 10800\\I & = & \dfrac{1789}{10800}\\\\& = & \textbf{0.2 A}\\\end{array}\\\text{The current used was $\large \boxed{\textbf{0.2 A}}$}](https://tex.z-dn.net/?f=%5Cbegin%7Barray%7D%7Brcl%7Dq%26%3D%26%20It%5C%5C1789%20%26%20%3D%20%26%20I%20%5Ctimes%2010800%5C%5CI%20%26%20%3D%20%26%20%5Cdfrac%7B1789%7D%7B10800%7D%5C%5C%5C%5C%26%20%3D%20%26%20%5Ctextbf%7B0.2%20A%7D%5C%5C%5Cend%7Barray%7D%5C%5C%5Ctext%7BThe%20current%20used%20was%20%24%5Clarge%20%5Cboxed%7B%5Ctextbf%7B0.2%20A%7D%7D%24%7D)
Note: The answer can have only one significant figure because that is all you gave for the time.
I think the answer is e? That's if o is -2 if not it will be a
Answer:
at the temperature of the experiment is 0.56.
Explanation:
Moles of
= 0.35 mole
Moles of
= 0.40 mole
Volume of solution = 1.00 L
Initial concentration of
=
Initial concentration of
= ![\frac{0.40mol}{1.00L}=0.40M](https://tex.z-dn.net/?f=%5Cfrac%7B0.40mol%7D%7B1.00L%7D%3D0.40M)
Equilibrium concentration of
=
The given balanced equilibrium reaction is,
Initial conc. 0.35 M 0.40 M 0 M 0M
At eqm. conc. (0.35-x) M (0.40-x) M (x) M (x) M
Given: (0.35-x) = 0.19
x= 0.16 M
The expression for equilibrium constant for this reaction will be,
Now put all the given values in this expression, we get :
![K_{eq}=\frac{0.16\times 0.16}{(0.19)\times (0.24)}=0.56](https://tex.z-dn.net/?f=K_%7Beq%7D%3D%5Cfrac%7B0.16%5Ctimes%200.16%7D%7B%280.19%29%5Ctimes%20%280.24%29%7D%3D0.56)
Thus
at the temperature of the experiment is 0.56.