Answer:
3.91 L
Explanation:
Using the ideal gas law equation as follows:
PV = nRT
Where:
P = pressure (atm)
V = volume (L)
n = number of moles (mol)
R = gas law constant (0.0821 Latm/molK)
T = temperature (K)
Based on the information given in this question,
P = 5.23 atm
V= ?
n = 0.831 mol
T = 27°C = 27 + 273 = 300K
Using PV = nRT
V = nRT/P
V = (0.831 × 0.0821 × 300) ÷ 5.23
V = 20.47 ÷ 5.23
V = 3.91 L
I can give you four oxygen, selenium, sulfur, talarium hope this helps!
1.53 moles of Fe is your solution hope it helps!
Answer:
Mg
Explanation:
The standard reduction potentials are
<u>E°/V
</u>
Au³⁺(aq ) + 3e⁻ ⟶ Au(s); 1.42
Hg²⁺(aq) + 2e⁻ ⟶ Hg(l); 0.85
Ag⁺(aq) + e⁻ ⟶ Ag(s); 0.80
Cu²⁺(aq) + 2e⁻ ⟶ Cu(s); 0.34
Mg2+(aq) + 2e- ⟶ Mg(s); -2.38
The more negative the standard reduction potential, the stronger the metal is as a reducing agent.
Mg is the only metal with a standard reduction potential lower than that of Cu, so
Only Mg will react spontaneously with Cu²⁺.
