1) divide each percentage by the relative atomic mass of the element
2) divide all results by the smallest number
3)multiply by a whole number to get the simplest whole number ratio (if necessary)
that is to say:
Na S O
32.37÷23 22.58÷32 45.05÷16
= 1.407 = 0.7056 = 2.816 (to 4 significant figures)
the smallest number here is 0.7056 so:
1.407÷0.7056 0.7056÷0.7056 2.816÷0.7056
=1.99 approx.2 = 1 3.99 approx. 4
here there is no need to carry out step 3 as ratio obtained is already a simplest whole number ratio
so empirical formula is: Na₂SO₄
Answer:
The correct answer is pOH= 11
Explanation:
From the aqueous acid-base equilibrium we know that
pH + pOH = 14
If we know pH, we can calculate pOH as follows:
pOH = 14 - pH
In this problem, the solution has a pH of 3, so:
pOH = 14 - 3 = 11
They share four electrons, two from each oxygen atom
2HNO3 + Ca(OH)2 --> 2HOH + Ca(NO3)2
Answer: The final temperature is 
Explanation:

As we know that,

.................(1)
where,
q = heat absorbed or released
= mass of lead = 50 g
= mass of water = 75 g
= final temperature = ?
= temperature of lead = 
= temperature of water = 
= specific heat of lead = 
= specific heat of water= 
Now put all the given values in equation (1), we get
![50\times 0.11\times (T_{final}-373)=-[75\times 1.0\times (T_{final}-273)]](https://tex.z-dn.net/?f=50%5Ctimes%200.11%5Ctimes%20%28T_%7Bfinal%7D-373%29%3D-%5B75%5Ctimes%201.0%5Ctimes%20%28T_%7Bfinal%7D-273%29%5D)

Therefore, the final temperature of the mixture will be 279.8 K.