Answer:
your answer should be the bottom
sorry if im wrong
Explanation:
Answer:
The ratio of f at the higher temperature to f at the lower temperature is 5.356
Explanation:
Given;
activation energy, Ea = 185 kJ/mol = 185,000 J/mol
final temperature, T₂ = 525 K
initial temperature, T₁ = 505 k
Apply Arrhenius equation;
![Log(\frac{f_2}{f_1} ) = \frac{E_a}{2.303 \times R} [\frac{1}{T_1} -\frac{1}{T_2} ]](https://tex.z-dn.net/?f=Log%28%5Cfrac%7Bf_2%7D%7Bf_1%7D%20%29%20%3D%20%5Cfrac%7BE_a%7D%7B2.303%20%5Ctimes%20R%7D%20%5B%5Cfrac%7B1%7D%7BT_1%7D%20-%5Cfrac%7B1%7D%7BT_2%7D%20%5D)
Where;
is the ratio of f at the higher temperature to f at the lower temperature
R is gas constant = 8.314 J/mole.K
![Log(\frac{f_2}{f_1} ) = \frac{E_a}{2.303 \times R} [\frac{1}{T_1} -\frac{1}{T_2} ]\\\\Log(\frac{f_2}{f_1} ) = \frac{185,000}{2.303 \times 8.314} [\frac{1}{505} -\frac{1}{525} ]\\\\Log(\frac{f_2}{f_1} ) = 0.7289\\\\\frac{f_2}{f_1} = 10^{0.7289}\\\\\frac{f_2}{f_1} = 5.356](https://tex.z-dn.net/?f=Log%28%5Cfrac%7Bf_2%7D%7Bf_1%7D%20%29%20%3D%20%5Cfrac%7BE_a%7D%7B2.303%20%5Ctimes%20R%7D%20%5B%5Cfrac%7B1%7D%7BT_1%7D%20-%5Cfrac%7B1%7D%7BT_2%7D%20%5D%5C%5C%5C%5CLog%28%5Cfrac%7Bf_2%7D%7Bf_1%7D%20%29%20%3D%20%5Cfrac%7B185%2C000%7D%7B2.303%20%5Ctimes%208.314%7D%20%5B%5Cfrac%7B1%7D%7B505%7D%20-%5Cfrac%7B1%7D%7B525%7D%20%5D%5C%5C%5C%5CLog%28%5Cfrac%7Bf_2%7D%7Bf_1%7D%20%29%20%3D%200.7289%5C%5C%5C%5C%5Cfrac%7Bf_2%7D%7Bf_1%7D%20%20%3D%2010%5E%7B0.7289%7D%5C%5C%5C%5C%5Cfrac%7Bf_2%7D%7Bf_1%7D%20%20%3D%205.356)
Therefore, the ratio of f at the higher temperature to f at the lower temperature is 5.356
When a monovalent cation X binds to a divalent anion Y, a compound with the formula
would be formed.
A monovalent cation is an atom that has lost an electron. Hence, such cation has a single positive charge. A monovalent cation X will, thus, be 
A divalent anion is an atom that has gained two electrons. Such anion has 2 negative charge. Thus, divalent Y would be 
Since Y is a divalent anion, it requires 2 electrons in order to successfully bind with another charged atom, a cation to be specific. Thus, two of
would be required to successfully bind 
+
+
---->
More on the chemical formula can be found here: brainly.com/question/16741890
Answer:
2.9 g
Explanation:
There is some info missing. I think this is the original question.
<em>Ammonium perchlorate is the solid rocket fuel used by the U.S. Space Shuttle. It reacts with itself to produce nitrogen gas, chlorine gas, oxygen gas, water, and a great deal of energy.
</em>
<em>What mass of water is produced by the reaction of </em><em>9.6 g</em><em> of ammonium perchlorate?</em>
<em />
Step 1: Given data
Mass of ammonium perchlorate: 9.6 g
Step 2: Write the balanced equation
2 NH₄ClO₄(s) → N₂(g) + Cl₂(g) + 2 O₂(g) + 4 H₂O(l)
Step 3: Calculate the moles corresponding to 9.6 g of ammonium perchlorate
The molar mass of ammonium perchlorate is 117.49 g/mol.

Step 4: Calculate the moles of water formed from 0.082 moles of ammonium perchlorate
The molar ratio of NH₄ClO₄ to H₂O is 2:4. The moles of water formed are 4/2 × 0.082 mol = 0.16 mol
Step 5: Calculate the mass corresponding to 0.16 moles of water
The molar mass of water is 18.02 g/mol.
