Explanation:
Molar mass of is 114.23 g/mol. Therefore, its number of moles are calculated as follows.
No. of moles =
=
= 0.043 mol
So, 0.043 moles are releasing 239.5 kcal of heat. Hence, heat released by 1.54 mol will be calculated as follows.
= 8577.44 kcal
Thus, we can conclude that 8577.44 kcal heat is released by the combustion of 1.54 mol of .
Answer:
<em>C</em> H2SO4 = 9.79 M
Explanation:
- molarity (M) ≡ # dissolved species / V sln
- H2SO4 ↔ H3O+ + SO4-
∴ %w/w H2SO4 = 960% = g H2SO4 / g sln * 100
⇒ 9.6 = g H2SO4 / g sln
calculation base: 1000 g sln
⇒ g H2SO4 = 9600g
⇒<em> </em>mol<em> </em>H2SO4 =<em> </em>9600 g H2SO4 * ( mol H2SO4/ 980g H2SO4 ) = 9.796 mol H2SO4
⇒ V sln = 1000g sln / 1000g/L = 1 L sln
∴ ρ H20 ≅ 1000 Kg/m³ = 1000 g/L
⇒ <em>C</em> H2SO4 = 9.796 mol H2SO4 / 1 L sln
⇒ <em>C</em> H2SO4 = 9.796 M
Answer:
a property ( colour,hardness and boiling point)
Answer:
A. Students made a measurement error, because ending with more products is impossible.
Explanation:
The law of conversation of matter tells us that in a chemical reaction, matter is never created or destroyed, it's simply converted from one form to another. So the mass of reactants should always equal the mass of the products in a chemical reaction. If there is excess mass in the product, the students have made an error of some kind.