Answer:
0.689 mg/L Cu
Explanation:
The equation of the best-fit line is:
<em>y</em> = 0.6136<em>x</em> + 0.0142
Where <em>y</em> is the absorbance and <em>x</em> is the concentration in mg/L.
Now using that equation we <u>calculate </u><u><em>x</em></u> when <em>y</em> is equal to 0.438, 0.434 & 0.439.
1) 0.438 = 0.6136<em>x</em> + 0.0142
x = 0.691 mg/L
2) 0.434 = 0.6136<em>x</em> + 0.0142
x = 0.684 mg/L
3) 0.439 = 0.6136<em>x</em> + 0.0142
x = 0.692 mg/L
Finally we <u>calculate the mean of the three concentrations</u>:
- (0.691 + 0.684 + 0.692)/3 = 0.689 mg/L
<span>Rust forms when 2 atoms of fe reacts with oxygen to form iron oxide as follows.
4Fe2 + 302 ==[]::::::::::::::::> 2Fe2O3.
So basically 4 atoms of oxygen reacts with 3 atoms of oxygen to produce the product. We need to find the number of moles of Fe that reacts with Oxygen. Number of moles is the concentration of iron multiplied by the molarity. So we have 55 * 0.035 = 1.925 moles.
Hence 1.925*4 atoms of iron which gives 7.7 moles will actually react with 3 *1.925 = 5.775 of Oxygen
Since we know the number of moles of oxygen we can solve for its mass. No of moles = mass/molar mass. Mass = no of moles * molar mass = 5.775 * 32 = 184.5</span>
Yes they do. But a very small kinetic energy. They vibrate in fixed positions
Answer:
32.7 L of H₂
Explanation:
We'll begin by calculating the number of mole in 95 g of Zn. This can be obtained as follow:
Mass of Zn = 95 g
Molar mass of Zn = 65 g/mol
Mole of Zn =?
Mole = mass /Molar mass
Mole of Zn = 95/65
Mole of Zn = 1.46 mole
Next, we shall determine the number of mole of H₂ produced by the reaction of 95 g (i.e 1.46 mole) of Zn. This can be obtained as illustrated below:
Zn + H₂SO₄ —> ZnSO₄ + H₂
From the balanced equation above,
1 mole of Zn reacted to produce 1 mole of H₂.
Therefore, 1.46 mole of Zn will also react to produce 1.46 mole of H₂.
Finally, we shall determine the volume of H₂ obtained at STP. This can be obtained as follow:
1 mole of H₂ = 22.4 L at STP.
Therefore,
1.46 mole of H₂ = 1.46 × 22.4
1.46 mole of H₂ = 32.7 L at STP
Thus, 32.7 L of H₂ were obtained from the reaction.
Answer:
Zero-Order
Explanation:
The exothermic decaying of nitrous oxide at 575° C will lead to as follows:
→
<u>Hot platinum wire in the above reaction would function as a catalyst in the zero-order</u>. However, if the reaction is considered in the gaseous phase, it will be more inclined towards second-order.
In the given scenario( → ), <u>the reactant molecules of Nitrous oxide are restricted to the ones which have linked themselves to the catalyst's surface. Once this limited surface is filled, the extra molecules of gas would remain vacant until the previously attached molecules with the surface are decayed entirely</u>.