Answer:
92.46 g
Explanation:
The reaction is
I = Current = 19.5 A
t = 4 hours =
F = Faraday constant = 96485.33 C/mol
Molar mass of copper = 63.546 g/mol
Charge is given by
Moles of electrons is given by
Moles of copper is
Mass of copper would be
The mass of copper electroplated is 92.46 g.
Answer:
q = mC∆T
q = (50 g)(4.184 J/g/deg)(10 deg)
q = 2092 J = 2.09x10^3 J
That's how it's done.
Explanation:
Hope this helps! sorry If i didn't simplify enough..
The answer is 9.03 × 10²⁴<span> molecules.
</span><span>Avogadro's number is the number of units (atoms, molecules) in 1 mole of substance.
Make the proportion.
</span><span>6.02 × 10²³ molecules per 1 mol
</span>x per 15 mol
6.02 × 10²³ molecules : 1 mol = x : 15 mol
x = 6.02 × 10²³ molecules * 15 mol * 1 mol
x = 90.3 × 10²³ molecules
x = 9.03 × 10 × 10²³ molecules
x = 9.03 × 10²³⁺¹ molecules
x = 9.03 × 10²⁴ molecules
Answer:
Mass = 185.896 g
Explanation:
Given data:
Mass in gram = ?
Number of moles = 2.00 mol
Solution:
Formula:
Number of moles = mass/molar mass
Molar mass of cobalt (I) hydroxide =92.948 g/mol
by putting the values,
2.00 mol = Mass/92.948 g/mol
Mass = 2.00 mol × 92.948 g/mol
Mass = 185.896 g
The x and y are directly related and k=8 means that the relationship between x and y is y=8x. So x=0.5, y=4; x=1, y=8; x=2, y=16; x=3, y=24.