Answer:
The net ionic equation is as follows:
HCN(aq) + OH-(aq) ----> H20(l) + CN-(aq)
Explanation:
The reaction between Hydrocyanic acid, HCN, and sodium hydroxide is a neutralization reaction between a weak acid and a strong base.
Hydrocyanic acid being a weak acid ionizes only slightly, while sodium hydroxide being a strong base ionizes completely. The equation for the reaction is given below:
A. HCN(aq) + NaOH-(aq) ----> NaCN(aq) + H2O(l)
Since Hydrocyanic acid is written in the aqueous form as it ionizes only slightly and the ionic equation is given below:
HCN(aq) + Na+(aq)+OH-(aq) ----> Na+(aq)+CN-(aq) + H2O(l)
Na+ being a spectator ion is removed from the net ionic equation given below:
HCN(aq) + OH-(aq) ----> H20(l) + CN-(aq)
Answer:
the answer is unsaturated
Explanation:
A saturated solution contains more solute per volume of solvent than an unsaturated solution. The solute has dissolved until no more can, leaving undissolved matter in the solution. ... In a supersaturated solution, there is more dissolved solute than in a saturated solution.
This is true there are many factors that influence the amount of a solute.
Answer:
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Explanation:
Regardless of the value of the y subscript, the number of moles of CO₂ that can be produced from 1 mol of 
is 3 moles: that is so because every molecule of contains 3 atoms of C and every atom of C produces one molecule of CO₂.
Then, you can calculate the number of moles of in 97.0g using the molar mass of the compound:
<u />
<u>1. Molar mass of </u><u> :</u>
- 3 × 12g/mol + y × 1 g/mol = (36 + y)g/mol
<u />
<u>2. Number of moles = mass in grams / molar mass</u>
- Number of moles of =
= 97.0 g / (36 + y)g/mol = 97.0/(36+y) mol
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<u>3. Number of moles of CO₂</u>
As stated above, the number of moles of CO₂ is 3 times the number of moles of :
- Number of moles of CO₂ = 3 × 97.0 / (36 + y) mol = 291 / (36 + y)
For instance, imagine the compound is C₃H₈. How many moles of CO₂ will be produced from 97.0 g of C₃H₈?
You can replace 8 for y:
- 291 / (36 + 8) mol = 291.0 / (44) mol = 6.61 mol
