The solution for the problem is:
First, use the concentration of the volume of the thing you
know to compute for the moles of that substance. Then, use the coefficient in
the balanced equation to relay moles of that to moles of anything else in the
chemical equation. Lastly, translate moles into mass by means of its molar
mass, or into a concentration using the volume.
Applying what I have said earlier:
0.0133 L X 1.68 mol/L = 0.0223 mol KMnO4 X (1 mol H2O2 / 2
mol KMnO4) = 0.0112 mol H2O2
Mass H2O2 = 0.0112 mol H2O2 X 34.0 g/mol = 0.380 grams H2O2
Answer:
Molarity = 0.01 M
Explanation:
Molarity is used to measure the concentration of a solution. It will be same for the whole solution or a small amount of solution if the solution is homogeneous.
So, <u>Molarity of 200 mL of solution = Molarity of 50 mL of solution</u>
given mass of aspirin = 360 mg = 0.36 g
molar mass of aspirin = 180 g
Volume of solution = 200 mL = 0.2 L
Therefore, Molarity = 0.01 M
The rules of IUPAC followed for hydrocarbon are
a) We will first find out the longest chain of carbon in the given organic compound including triple bond
the root name will be "hex" as number of carbon atoms in longest chain is six.
b) The triple bond will be assigned minimum number locant. the locant will be 2 .
The primary suffix will be "yne"
hence
hex-2-yne
c) we will give locant number to methyl group (present as substituent)
it will be "4"
Thus the completer IUPAC name will be
4-methylhex-2-yne or 4-methyl-2-hexyne [as given in the options]
Answer:
27.025 g of H₂O
Explanation:
The Balance chemical equation is
2 H₂ + O₂ = 2 H₂O
Step 1: Calculate Limiting Reagent
Moles of H₂
Mole = 16 g / 2.02 g/mol = 7.937 mol
Moles of O₂
Mole = 24 g / 32.00 g/mol = 0.750 mol
Mole ratio of H₂ : O₂ is 2 : 1. Hence, 7.937 mol of H₂ will need 3.9685 mol of O₂. This means O₂ is limiting reagent.
Step 2: Calculate Moles of H₂O
0.750 mol of O₂ will produce 1.50 mol of H₂O because the mole ratio of O₂ : H₂O is 1 : 2.
Step 3: Calculate mass of H₂O
Mass = 1.50 mol × 18.02 g/mol = 27.025 g of H₂O
Answer:
Oxygen is composed of three isotopes: oxygen-16, oxygen-17 and oxygen-18 and has an average atomic mass of 15.9980 amu. Oxygen-17 has a mass of 16.992 amu and makes up 0.035% of oxygen. Oxygen-16 has a mass of 15.982 amu and Oxygen-18 has a mass of 17.984 amu.
