Two things
Ferrous Ammonium Sulfate is a pale green or blue-green powder or sand-like solid. It is used in photography, analytical chemistry, and Iron-plating baths.
An FAS-DPD titration is as simple as a test for total alkalinity or calcium hardness. A buffered DPD indicator powder is added to a water sample and reacts with chlorine to produce the pink color characteristic of the standard DPD test.
Hope this it gang
The molarity of HBr solution is 0.239 M
calculation
write the equation for reaction
that is LiOH +HBr → LiBr +H20
find the moles of LiOH used
moles =molarity x volume
=0.205 x 29.15 = 5.976 moles
by use of mole ratio between LiOH :HBr which is 1:1 the moles of HBr is therefore= 5.976 moles
Molarity of HCL= moles /volume
= 5.976/25 = 0.239 M
Answer:
Cooling Steam at 100 C to ice at 0 C
Explanation:
chemical reaction results in the forming or breaking apart of chemical bonds between various elements. These reactions can result in many different outcomes, which can be affected by temperature, pressure and the amount of the reactants. Catalysts can also start a reaction or speed up its rate. However, the catalyst is not involved in the chemical reaction, as it remains unchanged before and after the reaction.
Although the elements and compounds may change form during the reaction, every atom in the reactants is also found in one of the products. In the reaction, individual elements can bond together to form compounds, or compounds can break apart into elements. For instance, when water is exposed to an electrical current, it breaks apart into oxygen and hydrogen gases. Alternatively, when zinc and sulfur react together, the two elements bond together to form zinc sulfide.
Some reactions also result in chemical equilibrium, which occurs when the reactants change into products at the same time as the products change back into the original reactants.
1) Write the chemical equation.
2) List the known and unknown quantities.
Sample: CH4.
Volume: 2.0 L.
Temperature: 30 ºC = 303.15 K.
Pressure: 3.0 atm.
Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1).
Moles: <em>unknown</em>.
3) Moles of CH4.
<em>3.1- Set the equation.</em>
<em>3.2- Plug in the known values and solve for n (moles).</em>
4) Moles of oxygen that reacted.
The molar ratio between CH4 and O2 is 1 mol CH4: 2 mol O2.
5) Volume of oxygen required.
Sample: O2.
Moles: 0.48 mol.
Temperature: 30 ºC = 303.15 K.
Pressure: 3.0 atm.
Ideal gas constant: 0.082057 L * atm * K^(-1) * mol^(-1).
Volume: <em>unknown</em>.
<em>5.1- Set the equation.</em>
<em>5.2- Plug in the known values and solve for V (liters).</em>
3.98 L of O2<em> is required to react with 2.0 L CH4.</em>
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