Answer:
C combination reaction (synthesis) reaction
Explanation:
two chemicals are combined
Answer:
0.00725 M
Explanation:
Considering for
Mass = 5.66 g
Molar mass of = 80.043 g/mol
Moles = Mass taken / Molar mass
So,
<u>Moles = 5.66 / 80.043 moles = 0.0707 moles</u>
will dissociate as:
Thus 1 mole of yields 1 mole of ammonium ions. So,
<u>Ammonium ions furnished by = 1 × 0.0707 moles = 0.0707 moles</u>
Considering for
Mass = 4.42 g
Molar mass of = 149.09 g/mol
Moles = Mass taken / Molar mass
So,
Moles = 4.42 / 149.09 moles = 0.0296 moles
will dissociate as:
Thus 1 mole of yields 3 moles of ammonium ions. So,
<u>Ammonium ions furnished by = 3 × 0.0296 moles = 0.0888 moles</u>
<u>Total moles of the ammonium ions = 0.0707 + 0.0888 moles = 0.1595 moles</u>
Given that:
Volume = 22.0 L
So, Molarity of the is:
<u>Molarity = Moles / Volume = 0.1595 / 22 M = 0.00725 M</u>
This should help :)
Example 1: A 36.0 g sample of water is initially at 10.0 °C.
How much energy is required to turn it into steam at 200.0 °C? (This
example starts with a temperature change, then a phase change followed
by another temperature change.)
Solution:
<span>q = (36.0 g) (90.0 °C) (4.184 J g¯1 °C¯1) = 13,556 J = 13.556 kJ
q = (40.7 kJ/mol) (36.0 g / 18.0 g/mol) = 81.4 kJ
q = (36.0 g) (100.0 °C) (2.02 J g¯1 °C¯1) = 7272 J = 7.272 kJ
q = 102 kJ (rounded to the appropriate number of significant figures)
</span>
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.
It’s some apps that come in handy for this sorry if I didn’t help