Answer:
Explanation:
The balanced equation is
I₂(g) + Br₂(g) ⇌ 2IBr(g)
Data:
Kc = 8.50 × 10⁻³
n(IBr) = 0.0600 mol
V = 1.0 L
1. Calculate [IBr]
![\text{[IBr]} = \dfrac{\text{0.0600 mol}}{\text{1.0 L}} = \text{0.0600 mol/L}](https://tex.z-dn.net/?f=%5Ctext%7B%5BIBr%5D%7D%20%3D%20%5Cdfrac%7B%5Ctext%7B0.0600%20mol%7D%7D%7B%5Ctext%7B1.0%20L%7D%7D%20%3D%20%5Ctext%7B0.0600%20mol%2FL%7D)
2. Set up an ICE table.
3. Calculate [I₂]
![\begin{array}{rcl}K_{\text{c}}&=&\dfrac{\text{[IBr]}^{2}} {\text{[I$_{2}$][Br]$_{2}$}}\\\\8.50 \times 10^{-2}&=&{\dfrac{(0.0600 - 2x)^{2}}{x^{2}}}& &\\\\0.2915x & = &{\dfrac{0.0600 - 2x}{x}}& &\\\\0.2915x & = &0.0600 - 2x\\\\2.2915x & = & 0.0600\\x & = & \textbf{0.026 18 mol/L}\\\end{array}\\](https://tex.z-dn.net/?f=%5Cbegin%7Barray%7D%7Brcl%7DK_%7B%5Ctext%7Bc%7D%7D%26%3D%26%5Cdfrac%7B%5Ctext%7B%5BIBr%5D%7D%5E%7B2%7D%7D%20%7B%5Ctext%7B%5BI%24_%7B2%7D%24%5D%5BBr%5D%24_%7B2%7D%24%7D%7D%5C%5C%5C%5C8.50%20%5Ctimes%2010%5E%7B-2%7D%26%3D%26%7B%5Cdfrac%7B%280.0600%20-%202x%29%5E%7B2%7D%7D%7Bx%5E%7B2%7D%7D%7D%26%20%26%5C%5C%5C%5C0.2915x%20%26%20%3D%20%26%7B%5Cdfrac%7B0.0600%20-%202x%7D%7Bx%7D%7D%26%20%26%5C%5C%5C%5C0.2915x%20%26%20%3D%20%260.0600%20-%202x%5C%5C%5C%5C2.2915x%20%26%20%3D%20%26%200.0600%5C%5Cx%20%26%20%3D%20%26%20%5Ctextbf%7B0.026%2018%20mol%2FL%7D%5C%5C%5Cend%7Barray%7D%5C%5C)
4. Convert the temperature to kelvins
T = (150 + 273.15) K = 423.15 K
5. Calculate p(I₂)
Answer:
carbon nitrogen and oxygen
The answer it the function
Idk I’m sorry. I just need points lol
Answer:
9.0 moles of CaO
Explanation:
We have the reaction equation as follows;
Fe2O3 + Ca3(PO4)2 -------> 2FePO4 + 3CaO
Now we know from the equation that;
1 mole of iron III oxide yields 3 moles of CaO
Therefore;
3 moles of iron III oxide yields 3 * 3/1
= 9.0 moles of CaO
