the mole concept :
a mole (mol) is defined as the amount of substance that contains as many atoms, molecules, icons, electrons or any other elementary entities as there are carbon atoms in exactly 12 gm of. the number of atoms in 12gm of is called Avogadro's number.
I'm not sure about muscular mass sorryyyy
Thermoplastics and thermosetting polymers Examples include: polyethylene (PS) and polyvinyl choline (PVC). Common thermoplastics range from 20,000 to 50,000 amu, while thermosets are assumed to have infinite molecular weight.
Full Question:
Aqueous sulfuric acid H2SO4 will react with solid sodium hydroxide NaOH to produce aqueous sodium sulfate Na2SO4 and liquid water H2O. Suppose 94g of sulfuric acid is mixed with 49.9g of sodium hydroxide. Calculate the minimum mass of sulfuric acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.
Answer:
32.8725g
Explanation:
First thing's first, we write out the balanced chemical equation;
2NaOH + H2SO4 --> Na2SO4 + 2H2O
The question hints that sulphuric acid would be in exess by asking to calculate the minium mass that would be left over.
We proceed by calculatng the amount of sulphuric acid that would react with 49.9g of sodium hydroxide.
From the reaction,
2 moles of NaOH reacts with 1 mole of H2SO4.
Calculate moles of sodium hydroxide:
Molar mass of NaOH= 40.0 g/mol
Mass of NaOH = 53 g
moles = Maass / Molar mass = 1.2475
This means 1.2475 would react with x number of moles;
2 = 1
1.2475 = x
x = 1.2475 / 2 = 0.62375
Mass of Sulphuric acid reacted = moles * molar mass = 0.62375 * 98 = 61.1275g
Mimium mass of left over = 94 - 61.1275g = 32.8725g
Below is the solution. I hope it helps.
CfVf = CiVi
<span>Cf = (CiVi)/ Vf </span>
<span>i. Cf = [ (10^-6 mol / L) (1 mL) (1L / 1000 mL) ] / [ (1kL) (1000L / 1 kL) ] = 1x10^-12 M → use as Ci in next dilution </span>
<span>ii. Cf = 1x10^-19 M → use as Ci in next dilution </span>
<span>iii. Cf = 1x10^-22 M </span>
Answer:
Volume = 13.06 L
Explanation:
We are given: mass of nitrogren gas = 16.34 g
We know: molar mass of nitrogen gas = 28.014 g/mol
: ideal gas law constant = 0.082 L.atm/K.mol
At STP: temperature = 273.15 K
: pressure = 1 atm
We first determine the number of moles of nitrogen gas:
n = m/M
= 16.34/28.014
= 0.58 mol
Using the ideal gas law:
