The balanced equation for the combustion reaction is as follows
4C₂H₅ + 13O₂ --> 8CO₂ + 10H₂O
coefficients for the reactants and products are
C₂H₅ - 4
O₂ - 13
CO₂ - 8
H₂O - 10
According to Bronsted-Lowry acid concept
an acid is a that donate a proton" and a base is a "proton acceptor."so
will look for that molecule to which <span><span>H2</span>O</span> "donates" <span>H+</span>to become <span>O<span>H−</span></span>. so answer will be..
. <span>N<span>H3</span>+<span>H2</span>O→N<span>H+4</span>+O<span>H<span>−
so correct option is NH3
hope it helps</span></span></span>
Answer:
+2
Explanation:
If a compound existed, we would identify the oxidation state of sulfur using the following logic:
- oxygen is more electronegative than sulfur, so it's more electron-withdrawing and it should have a negative oxidation state producing a positive oxidation state for sulfur;
- oxygen typically has an oxidation state of -2;
- we may then apply the fact that SO is expected to be a molecule with a net charge of 0;
- if the net charge is 0 and the oxidation state of oxygen is -2, we may set the oxidation state of S to x;
- write the equation for the net charge of 0 by adding all individual charges of the two atoms: ;
- hence, x = 2.
That said, in this hypothetical compound S would have an oxidation state of +2.
Yes because look in the book dh
Answer:
65°C
Explanation:
Formula for calorimetry is:
Q = C . m . ΔT
Where Q is heat, C is specific heat, m is mass and ΔT is the difference between final T° and initial.
We have all data to replace.
First of all, we convert kJ to J → 4.94 kJ . 1000 J / 1 kJ = 4940 Joules
We made this conversion because the unit of C, is in J
As heat is lost, we have to think in a negative value. Let's replace:
- 4940 J = 4.18 J/ g °C . 35 g . ( Final T° - 98.8°C)
- 4940 J / (4.18 J/ g °C . 35 g) = Final T° - 98.8°C
Final T° = - 4940 J / (4.18 J/ g °C . 35 g) + 98.8°C
Final T° = 65.03 °C
Notice, that this answer has sense because as T° decreased, heat has been lost.