0.5
Explanation:
Given parameters:
Mass of Ca²⁺ = 10g
unknown:
Equivalent weight = ?
Solution:
Equivalent weight that is the amount of electrons which a substance gains or loses per mole.
Ca²⁺ has +3 charge
It lost 2e⁻;
therefore;
In 1 mole of Ca²⁺, we have 2 equivalent weight
1 mol Ca²⁺ = 2eq. wts.
1 mol Ca x (40 g / 1 mol ) x (1 mol / 2 eq.wts.) = 20.0 g = 1 eq.wt.
Therefore;
10.0 g Ca²⁺ x (1 eq.wt. / 20.0 g) = 0.5 eq.wts.
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The answer for four is frequency.
Answer:

Explanation:
2NO₂ ⇌ N₂O₄
E/mol·L⁻¹: 0.058 0.012
K_{\text{eq}} = \dfrac{\text{[N$_{2}$O$_{4}$]}}{\text{[NO$_{2}$]$^{2}$}} = \dfrac{0.012}{0.058^{2}} = \mathbf{3.6}
\\\\
\text{The $K_{\text{eq}}$ value would be $\boxed{\mathbf{3.6}}$}
Answer:
690 g IrI₃
Explanation:
To convert from moles to grams, you have to use the molar mass of the compound. The molar mass of IrI₃ is 572.92 g/mol. You use this as the unit converter in this equation:

Round to the lowest number of significant figures which is 2 to get 690 g IrI₃.
In each mole of carbon dioxide there will be one mole of O₂.
Let us calculate the moles of carbon dioxide gas present first
The conditions are NTP it means , Temperature = 293 K and P = 1 atm
We will use ideal gas equation
PV= nRT
Where
P = Pressure of gas = 1 atm
V= 112mL=0.112L
R= gas constant =0.0821 L atm /mol K
n = moles = ?
Putting values

moles = 0.00466
Thus moles of carbon dioxide will be 0.00466
The moles of O₂ = 0.00466