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3 years ago

where will you find maximum rate of evaporation - ocean, pond or an aquarium? Give reason to support your answer.

2 answers:

7 0

the ocean because of the fact that in an aquarium if its indoors the sun wont hit it at al even if its outdoors the ocean is way to huge and its because of the ocean that we have clouds. Pond, same thing the ocean beats it

arsen [322]3 years ago

6 0

The answer is Ocean.
Oceans are larger than ponds and or an aquarium. Hence they possess wider exposed surface with more number of free surface molecules.Greater the number of surface molecules, greater number of molecules may escape from the surface easily..and hence greater will be the rate of evaporation.
The rate of evaporation depends even on the external climatic conditions such as Temperature, Wind, Pressure etc.
Higher the temperature. higher will be the rate of evaporation.

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I need help fast...........

guapka [62]

Answer:

I think its might be 1 because the ionic numbers for CA is +2 and for P its +3

8 0

2 years ago

How many hydrogen atoms are in 89.5 g of<br> C6H6 ?<br> Answer in units of atoms.

Elodia [21]

Solution :

Molar mass of $C_6H_6$ is :

M = 6×12 + 6×1 g

M = 78 g

78 gram of $C_6H_6$ contains $6.022 \times 10^{23}$ molecules.

So, 89.5 gram of $C_6H_6$ contains :

$n = 6.022 \times 10^{23} \times \dfrac{89.5}{78}\\\\n = 6.91 \times 10^{23}$

Now, from the formula we can see that one molecule of $C_6H_6$ contains 2 hydrogen atom . So, number of hydrogen atom are :

$h = 2\times 6.91 \times 10^{23}\\\\h = 1.38 \times 10^{22}\ atoms$

Hence, this is the required solution.

8 0

2 years ago

Determine the rate law, including the values of the orders and rate law constant, for the following reaction using the experimen

olga55 [171]

Answer: Rate law= $k[A]^1[B]^2$ , order with respect to A is 1, order with respect to B is 2 and total order is 3. Rate law constant is $3L^2mol^{-2}s^{-1}$

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$Rate=k[A]^x[B]^y$

k= rate constant

x = order with respect to A

y = order with respect to A

n = x+y = Total order

a) From trial 1: $1.2\times 10^{-2}=k[0.10]^x[0.20]^y$ (1)

From trial 2: $4.8\times 10^{-2}=k[0.10]^x[0.40]^y$ (2)

Dividing 2 by 1 : $\frac{4.8\times 10^{-2}}{1.2\times 10^{-2}}=\frac{k[0.10]^x[0.40]^y}{k[0.10]^x[0.20]^y}$

$4=2^y,2^2=2^y$ therefore y=2.

b) From trial 2: $4.8\times 10^{-2}=k[0.10]^x[0.40]^y$ (3)

From trial 3: $9.6\times 10^{-2}=k[0.20]^x[0.40]^y$ (4)

Dividing 4 by 3: $\frac{9.6\times 10^{-2}}{4.8\times 10^{-2}}=\frac{k[0.20]^x[0.40]^y}{k[0.10]^x[0.40]^y}$

$2=2^x,2=2^1$ , x=1

Thus rate law is $Rate=k[A]^1[B]^2$

Thus order with respect to A is 1 , order with respect to B is 2 and total order is 1+2=3.

c) For calculating k:

Using trial 1: $1.2\times 10^{-2}=k[0.10]^1[0.20]^2$

$k=3 L^2mol^{-2}s^{-1}$ .

6 0

3 years ago

100!!!POINTS PLZ HELP Explain (on the molecular level) what pumping a tire with air will do to

Bas_tet [7]

Answer:

Gases are easily compressed. We can see evidence of this in Table 1 in Thermal Expansion of Solids and Liquids, where you will note that gases have the largest coefficients of volume expansion. The large coefficients mean that gases expand and contract very rapidly with temperature changes. In addition, you will note that most gases expand at the same rate, or have the same β. This raises the question as to why gases should all act in nearly the same way, when liquids and solids have widely varying expansion rates.

The answer lies in the large separation of atoms and molecules in gases, compared to their sizes, as illustrated in Figure 2. Because atoms and molecules have large separations, forces between them can be ignored, except when they collide with each other during collisions. The motion of atoms and molecules (at temperatures well above the boiling temperature) is fast, such that the gas occupies all of the accessible volume and the expansion of gases is rapid. In contrast, in liquids and solids, atoms and molecules are closer together and are quite sensitive to the forces between them.

3 0

3 years ago

I need this answer quick please show work

Ainat [17]

Answer:

The answer to your question is 25.2 g of acetic acid.

Explanation:

Data

[Acetic acid] = 0.839 M

Volume = 0.5 L

Molecular weight = 60.05 g/mol

Process

1.- Calculate the number of moles of acetic acid

Molarity = moles / volume

-Solve for moles

moles = Molarity x volume

-Substitution

moles = (0.839)(0.5)

-Result

moles = 0.4195

2.- Calculate the mass of acetic acid using proportions and cross multiplications

60.05 g ----------------------- 1 mol

x ----------------------- 0.4195 moles

x = (0.4195 x 60.05) / 1

x = 25.19 g

3.- Conclusion

25.2 g are needed to prepare 0.500 L of Acetic acid 0.839M

4 0

3 years ago