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gtnhenbr [62]
3 years ago
6

A bird could be both a consumer and a producer

Chemistry
1 answer:
Ilia_Sergeevich [38]3 years ago
4 0
False, only Consumers.
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22.17 grams of Mercury (II) Nitrate, Hg(NO3)2, reacts with an excess of Potassium, K.
Svetradugi [14.3K]

Answer:

Mass = 14.0 g

Explanation:

Given data:

Mass of mercury nitrate = 22.17 g

Mass of mercury formed = ?

Solution:

Chemical equation:

Hg(NO₃)₂ + 2K    →    2KNO₃ + Hg

Number of moles of mercury nitrate:

Number of moles = mass/molar mass

Number of moles = 22.17 g / 324.6 g/mol

Number of moles = 0.07 mol

Now we will compare the moles of Hg(NO₃)₂ and mercury.

                Hg(NO₃)₂       :        Hg

                     1                :          1

                  0.07             :       0.07

Mass of mercury:

Mass = number of moles × molar mass

Mass = 0.07 mol × 200.6 g/mol

Mass = 14.0 g

7 0
2 years ago
All minerals on the mohs hardness scale are hard enough to scratch a piece of glass is it true or false
11Alexandr11 [23.1K]
The answer is false
8 0
2 years ago
Read 2 more answers
how many moles of potassium hydroxide are needed to completely react with 1.73 miles of aluminum sulfate according to the follow
Masteriza [31]
<h3><u>Answer; </u></h3>

=10.38  moles KOH  

<h3><u>Explanation</u>;</h3>

The balanced equation.  

6KOH + Al2(SO4)3 --> 3K2SO4 + 2Al(OH)3  

From the equation;

1 mole of aluminum sulfate requires 6 moles of potassium hydroxide.  

Moles of Aluminium sulfate;  1.73 moles

Moles of KOH;

1 mol Al2(SO4)3 : 6 mol KOH = 1.73  mol Al2(SO4)3 : x mol KOH  

Thus; x =  (6 × 1.73)

              <u> =10.38 moles KOH </u>

4 0
3 years ago
Read 2 more answers
Previous Page
algol13
Chechnya. 345. Gcbjshjkfs
3 0
3 years ago
Consider the reaction of peroxydisulfate ion (S2O2−8) with iodide ion (I−) in aqueous solution: S2O2−8(aq)+3I−(aq)→2SO2−4(aq)+I−
kolbaska11 [484]

Answer:

r = 3.61x10^{-6} M/s

Explanation:

The rate of disappearance (r) is given by the multiplication of the concentrations of the reagents, each one raised of the coefficient of the reaction.

r = k.[S2O2^{-8} ]^{x} x [I^{-} ]^{y}

K is the constant of the reaction, and doesn't depends on the concentrations. First, let's find the coefficients x and y. Let's use the first and the second experiments, and lets divide 1º by 2º :

\frac{r1}{r2} = \frac{0.018^{x} x0.036^{y} }{0.027^xx0.036^y}

\frac{2.6x10^{-6}}{3.9x10^{-6}} = (\frac{0.018}{0.027})^xx(\frac{0.036}{0.036})^y

0.67 = 0.67^x

x = 1

Now, to find the coefficient y let's do the same for the experiments 1 and 3:

\frac{r1}{r3} = \frac{0.018x0.036^y}{0.036x0.054^y}

\frac{2.6x10^{-6}}{7.8x10^{-6}} = (\frac{0.018}{0.036})x(\frac{0.036}{0.054})^y

0.33 = 0.5x 0.67^y

0.67 = 0.67^y

y = 1

Now, we need to calculate the constant k in whatever experiment. Using the first :

2.6x10^{-6} = kx0.018x0.036kx6.48x10^{-4} = 2.6x10^{-6}

k = 4.01x10^{-3} M^{-1}s^{-1}[/tex]

Using the data given,

r = 4.01x10^{-3}x1.8x10^{-2}x5.0x10^{-2}

r = 3.61x10^{-6} M/s

7 0
2 years ago
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