The equation that we will use to solve this question is:
M1*V1 = M2*V2
where:
M1 is the initial concentration = 9.13*10^-2 M
V1 is the initial volume = 80 ml
M2 is the final concentration = 1.6*10^-2 M
V2 in the final volume that we need to find
Substitute with the values given in the equation to calculate the final volume as follows:
(9.13*10^-2*80) = (1.6*10^-2) * V2
V2 = 456.5 ml
17. not sure
18. not sure
19. movement of rock from one place to another
20. deposition
21. Urbanization
22. sedimentary
23. ease of traffic movement
24. absolute dating
25. fracture
26. increased farm land producing food for people
Answer:
1.17 L of H₂
Explanation:
We'll begin by calculating the number of mole in 2.3 g of Mg. This can be obtained as follow:
Mass of Mg = 2.3 g
Molar mass of Mg = 24 g/mol
Mole of Mg =?
Mole = mass /molar mass
Mole of Mg = 2.3 / 24
Mole of Mg = 0.096 mole
Next, we shall determine the number of mole of H₂ produced by the reaction of 2.3 g (i.e 0.096 mole) of Mg. This can be obtained as follow:
Mg + 2HCl —> MgCl₂ + H₂
From the balanced equation above,
1 mole of Mg reacted to 1 mole of H₂.
Therefore, 0.096 mole of Mg will also react to produce 0.096 mole of H₂.
Finally, we shall determine volume of H₂ produced from the reaction. This can be obtained as follow:
Number of mole (n) of H₂ = 0.096 mole
Pressure (P) = 2 atm
Temperature (T) = 298 K
Gas constant (R) = 0.0821 atm.L/Kmol
Volume (V) of H₂ =?
PV = nRT
2 × V = 0.096 × 0.0821 × 298
Divide both side by 2
V = (0.096 × 0.0821 × 298) /2
V = 1.17 L
Therefore, 1.17 L of H₂ were obtained from the reaction.
The answer is Decomposition.
An example of a nuisance, oxygen reacts with iron to form rust.
This reaction involves the addition of oxygen, which is not needed.
2Fe(s) + 2H2O(l) + O2 (g)---> 2Fe^+2 (aq) + 4OH- (aq)