CaO + H2O → Ca(OH)2
the number of O atom on the left side is 1 and on the right side 2 so,
we put 2H2O instead of H2O
CaO + 2H2O → Ca(OH)2
now we have to put 2Ca(OH)2 instead of Ca(OH)2 to make H atoms equal on both sides 4
CaO + 2H2O → 2Ca(OH)2
now we have to put 2CaO instead of CaO to make Ca atoms equal on both sides 2 atoms.
∴ the final balanced equation is:
2CaO + 2H2O → 2 Ca(OH)2
∴ the coefficients are 2 2 2
Answer:
False
Explanation:
The statement ; Regardless of any concentration of ammonium solution the precipitate of unknown halide after 0.1M AgNO3 will remain is FALSE
This is Because the remaining concentration of AgNO3 is dependent on the solubility of Ag⁺
Answer:
A. LiCl
Explanation:
Lithium chloride is an ionic compound but it also has some covalent character due to the very small size of lithium metal.
Answer:
Methyl Alcohol.
Acetate
Heptane
Dioxane
Explanation:
The boiling point of liquids are measure by observing the gas pressure or vapors temperature. There are few liquids whose boiling point is difficult to measure. The gas pressure differs for every liquid. It is important to observe the vapor pressure also to identify the boiling point. The most difficult boiling point identification is for Methyl alcohol as it has ability to absorb different level of pressure.
<span>1. A gas occupies 4.31 litres at a pressure of 0.755atm. Determine the volume if the pressure is increased to 1.25 atm.
method: </span>Boyles Law<span>: P1/V1 = P2/V2
</span>P1/V1 = P2/V2 implies V2= P2 V1/ P1
V2=1.25x4.31 / 17=7.13L
<span>
2. 600 mL of a gas is at a pressure of 8.00atm. What is the Volume of the gas at 2 atm?
</span>method: Boyles Law: P1/V1 = P2/V2
P1/V1 = P2/V2 implies V2= P2 V1/ P1,
V1=2.6mL=0.026L
V2= P2 V1/ P1= 0.00065 L
<span>3. How hot will a 2.3 L balloon have to get to expand to a volume of 400 L? Assume that the initial temperature of the balloon is 25 degrees Celsius.
</span><span>Method: Charles Law: V1/T1 =V2/T2 Degrees Celcius + 273 = Kelvin
</span>
25 degrees Celsius=25+273=298K=T1
V1=2.3L, V2=400L
V1/T1 =V2/T2 implies T2=V2T1/V1=(400x298) /2.3=51826 K
<span>4. A gas takes up a volume of 17 litres, has a pressure of 2.3atm, and a temperature of 299K. If I raise the temperature to 350K and lower the pressure to 1.5atm, what is the new volume of the gas?
</span>
<span>Combined gas Law: (P1)(V1) = (P2)(V2)
(T1) (T2)</span>
V1=17L
P1=2.3 atm
T1= 299K
P2=1.5 atm
T2=350 K
V2=?
(P1)(V1) / T1= (P2)(V2)/ T2
so V2= (P1)(V1) T2 / P2 T1
V2=17x2.3x350 /1.5 x 299= 30.51L
