Answer:
Answer is: Keq = [CO₂].
Explanation:
Balanced chemical reaction: CaCO3(s) ⇄ CaO(s) + CO₂(g).
The equilibrium constant (Keq) is a ratio of the concentration of the products to the concentration of the reactants.
Pure liquids (shown in chemical reactions by appending (l) to the chemical formula) and solids (shown in chemical equations by appending (s) to the chemical formula) not go in to he equilibrium constant expression, only gas state (shown in chemical reactions by appending (g) to the chemical formula) reactants and products go in to the equilibrium constant expression
I mole of water has an Avogadro number of molecules.
1 mole = 6.02 * 10^ 23 molecules.
6.02 * 10^ 23 molecules = 1 mole of water
1 molecule = 1/(6.02 * 10^23) mole of water
2.0 * 10^22 molecules would have = (2*10^22) * 1/(6.02*10^23)
= 0.033
2* 10 ^22 molecules of water would have 0.033 moles of water.
It indicates that there is only one oxygen molecule
Answer:
Your question is not complete, but use this answer as a guide for your solution.
Question: A chemistry student weighs out 0.112g of acetic acid (HCH₃CO₂) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1600 <em>M</em> NaOH solution. Calculate the volume of solution the student will need to add to reach the equivalence point. Be sure your answer has the correct number of significant digits.
Answer: Volume of NaOH is 11.6 mL
Explanation:
The reaction of acetic acid with NaOH is as follows:
CH3COOH + NaOH -----> CH3COONa + H2O
M1V1 = M2V2
Here M1 V1 are molarity and volume of acetic acid.
M2, V2 are molarity and volume of NaOH.
Number of moles of acetic acid:
0.112 g CH3COOH × (1 mol / 60.05 g) = 0.001865 mol
Molarity = moles of solute / Liters of solution
Molarity = 0.001865 mol / 0.250 L = 0.00746 M
Hence,
M1 = 0.00746 M
V1 = 250 mL
M2 = 0.160 M
V2 = ?
V2 = M1V1 / M2
V2 = 0.00746 M × 250 mL / 0.160 M
V2 = 11.6 mL
Hence the volume of NaOH is 11.6 mL
Usually, percent yield is lower than 100% because the actual yield is often less than the theoretical value. Reasons for this can include incomplete or competing reactions and loss of sample during recovery. Percent yield is always a positive value. I hope this can help you
