Answer:
The metal which reduces the other compound is the one higher in reactivity. So in this case, it is.
Explanation:
<u>Answer:</u> The mass of sulfuric acid present in 60 mL of solution is 34.1 grams
<u>Explanation:</u>
We are given:
44 % (m/m) solution of sulfuric acid. This means that 44 grams of sulfuric acid is present in 100 grams of solution.
To calculate volume of a substance, we use the equation:

Density of solution = 1.343 g/mL
Mass of solution = 100 g
Putting values in above equation, we get:

To calculate the mass of sulfuric acid present in 60 mL of solution, we use unitary method:
In 77.46 mL of solution, mass of sulfuric acid present is 44 g
So, in 60 mL of solution, mass of sulfuric acid present will be = 
Hence, the mass of sulfuric acid present in 60 mL of solution is 34.1 grams
Answer:
both Mg isotopes have same atomic number which is equal to number of protons , and the chemical properties of an element depends upon the the number of protons in its atom . and both Mg 24 12 and Mg 26 12 have same number of protons hence they exhibits similar chemical
okay
Explanation:
i hope it helped you .
Answer : The volume of sodium benzoate and benzoic acid solution mixed to prepare this buffer should be, 29.0 mL and 71 mL respectively.
Explanation :
Let the volume of sodium benzoate (salt) be, x
So, the volume of benzoic acid (acid) will be, (100 - x)
Using Henderson Hesselbach equation :
![pH=pK_a+\log \frac{[Salt]}{[Acid]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5BSalt%5D%7D%7B%5BAcid%5D%7D)
Now put all the given values in this expression, we get:

x = 29.0
The volume of sodium benzoate = x = 29.0 mL
The volume of benzoic acid (acid) = (100 - x) = (100 - 29.0) = 71 mL
Thus, the volume of sodium benzoate and benzoic acid solution mixed to prepare this buffer should be, 29.0 mL and 71 mL respectively.
Answer:
There will be 143,67g CO2 produced
Explanation:
2 C6H6 + 15 O2 → 12 CO2 + 6 H2O
(42,5 g C6H6) / (78.1124 g C6H6/mol) = 0.54408775 mole C6H6
(113.1 g O2) / (31.9989 g O2/mol) = 3.534496 moles O2
0.54408775 mole of C6H6 would react completely with 0.54408775 x (15/2) = 4.080658 mole O2, but there is more O2 present than that, so O2 is in excess and C6H6 is the limiting reactant.
(0.54408775 mol C6H6) x (12/2) x (44.0096 g/mol) = 143.67 g CO2