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What is the molarity of the following solutions?a. 19.5 g NaHCO3 in 460.0 ml solution
b. 26.0 g H2SO4 in 200.0 mL solution
c. 15.0 g NaCl dissolved to make 420.0 mL solution

Answers

Answer 1

Answer:

Answer:

a) NaHCO3 = 0.504 M

b) H2SO4 = 1.325 M

c) NaCl = 0.610 M

Explanation:

Step 1: Data given

Moles = mass / molar mass

Molarity = moles / volume

a. 19.5 g NaHCO3 in 460.0 ml solution

Step 1: Data given

Mass NaHCO3 = 19.5 grams

Volume = 460.0 mL = 0.460 L

Molar mass NaHCO3 = 84.0 g/mol

Step 2: Calculate moles NaHCO3

Moles NaHCO3 = 19.5 grams / 84.0 g/mol

Moles NaHCO3 = 0.232 moles

Step 3: Calculate molarity

Molarity = 0.232 moles / 0.460 L

Molarity = 0.504 M

b. 26.0 g H2SO4 in 200.0 mL solution

Step 1: Data given

Mass H2SO4 = 26.0 grams

Volume = 200.0 mL = 0.200 L

Molar mass H2SO4 = 98.08 g/mol

Step 2: Calculate moles H2SO4

Moles H2SO4 = 26.0 grams / 98.08 g/mol

Moles H2SO4 = 0.265 moles

Step 3: Calculate molarity

Molarity = 0.265 moles / 0.200 L

Molarity =1.325 M

c. 15.0 g NaCl dissolved to make 420.0 mL solution

Step 1: Data given

Mass NaCl = 15.0 grams

Volume = 420.0 mL = 0.420 L

Molar mass NaCl = 58.44 g/mol

Step 2: Calculate moles NaCl

Moles NaCl = 15.0 grams / 58.44 g/mol

Moles NaCl = 0.256 moles

Step 3: Calculate molarity

Molarity = 0.256 moles / 0.420 L

Molarity =0.610 M

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Chlorine (Cl2Cl2) is a strong germicide used to disinfect drinking water and to kill microbes in swimming pools. If the product is Cl−Cl−, was the elemental chlorine oxidized or reduced?

Answers

Answer:

The elemental chlorine was reduced

Explanation: inl the elemental form, the oxidation state of chlorine is =0 on been reduced to Cl-Cl-, the oxidation state reduces to -1

Carbon and oxygen combine to form the molecular compound CO2, while silicon and oxygen combine to form a covalent network solid with the formula unit SiO2. Explain the difference in bonding between the two group 4A elements and oxygen. g

Answers

Answer:

See explanation below.

Explanation:

Both carbon and silicon are members of group 4A(now group 14) i n the periodic table. Carbon is the first member of the group. CO2 is a gas while SiO2 is a solid. In SiO2, there are single bonds between silicon and oxygen and the geometry around the central atom is tetrahedral while in CO2, there are double carbon-oxygen bonds and the geometry around the central atom is linear. CO2 molecules are discrete and contain only weak vanderwaals forces.

Again, silicon bonds to oxygen via its 3p orbital while carbon bonds to oxygen via a 2p orbital. As a result of this, there will be less overlap between the pi orbitals of silicon and that of oxygen. This is why tetrahedral bonds are formed with oxygen leading to a covalent network solid rather than the formation of a silicon-oxygen pi bond. A covalent network solid is known to be made up of a network of atoms of the same or different elements connected to each other continuously throughout the structure by covalent bonds.

In SiO2, each silicon atom is surrounded by four oxygen atoms. Each corner is shared with another tetrahedron. SiO2 forms an infinite three dimensional structure and melts at a very high temperature.

Final answer:

Carbon and oxygen form a molecular compound CO2 with weaker covalent bonds, while silicon and oxygen form a covalent network solid SiO2 with stronger, three-dimensional covalent bonds.

Explanation:

The difference in bonding between carbon and oxygen compared to silicon and oxygen is due to the different nature of their chemical bonds. In the case of carbon and oxygen, they form a molecular compound CO2, where carbon and oxygen atoms share electrons to form covalent bonds. This is because carbon and oxygen have similar electronegativities, so they can share electrons equally. The covalent bonds in CO2 are relatively weak, allowing the compound to exist as a gas at room temperature and pressure.

On the other hand, silicon and oxygen form a covalent network solid with the formula unit SiO2, known as quartz. In this case, silicon and oxygen atoms are covalently bonded in a three-dimensional network structure, where each silicon atom is bonded to four oxygen atoms and each oxygen atom is bonded to two silicon atoms. This network structure gives SiO2 its high melting point and hardness, making it a solid at room temperature and pressure.

In summary, the difference in bonding between carbon and oxygen compared to silicon and oxygen is that carbon and oxygen form a molecular compound with weaker covalent bonds, while silicon and oxygen form a covalent network solid with stronger, three-dimensional covalent bonds.

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Question: Looking at the above visual of "Atmospheres of the Solar System" What are two patternsyou can find? PLEASE HELP DUE TONIGHT!

Answers

Answer:

The first and most obvious pattern I see is that all gas giants have an atmosphere mainly made up of hydrogen

The second thing I notice is that all the rocky planets have a significant amount of Nitrogen in their atmospheres except Mercury.

The third thing I notice is that all planets have one element that makes up 75% or more of its atmosphere except Mercury.

(If this is good, may I have brainliest, please? I'm kinda poor..)

Answer:

It's hard to find patterns in the solar system's atmosphere but I think above found a lot of them.

How many water molecules are in a block of ice containing 1.50 mol of water (H2O)?

Answers

1.50 moles H20(6.02*10^23 molecules/1 mole)
9.03*10^23 molecules

Final answer:

The number of water molecules in a 1.50 mol block of ice is calculated by multiplying the number of moles of water by Avogadro's number. The result is approximately 9.033 x 10^23 water molecules.

Explanation:

In chemistry, the amount of substance in moles is related to the number of particles (atoms, molecules) through Avogadro's number. Avogadro's number, which is 6.022 x 1023 particles/mol, tells us the number of molecules in one mole of a substance.

To calculate the number of water molecules in 1.50 mol of water, you would multiply the number of moles of water by Avogadro's number:

1.50 mol of water x 6.022 x 1023 water molecules/mol of water = 9.033 x 1023 water molecules

Therefore, there are approximately 9.033 x 1023 water molecules in a 1.50 mol block of ice.

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A 3.0 L flask containing helium at 145 mmHg is connected by a closed valve to a 2.0 L flask containing argon at 355 mmHg. When the valve is opened and the gases are allowed to mix equally in the two flasks, what is the total pressure (in mmHg) in the two connected flasks after mixing ?

Answers

Answer:

Assuming that both helium and argon act like ideal gases, the total pressure after mixing would be approximately $229\; \rm mmHg$ .

Explanation:

By the ideal gas equation, $P\cdot V = n \cdot R \cdot T$ , where

$P$ is the pressure of the sample.
$V$ is the volume of the container.

$n$ is the number of moles of gas particles in the sample.
$R$ is the ideal gas constant.
$T$ is the temperature of the sample.

Rewrite to obtain:

$\displaystyle n = (P \cdot V)/(R\cdot T)$ , and
$\displaystyle P = (n \cdot R \cdot T)/(V)$ .

Assume that the two samples have the same temperature, $T$ . Also, assume that mixing the two gases did not affect the temperature.

Apply the equation $\displaystyle n = (P \cdot V)/(R\cdot T)$ to find the number of moles of gas particles in each container:

In the helium container, $V = 3.0\; \rm L$ and $P = \rm 145\; mmHg$ . Hence, $\displaystyle n_1 = (P\cdot V)/(R \cdot T) = \frac{(3.0\; \text{L}) \cdot (145\; \text{mmHg})}{R\cdot T}$ .
In the argon container, $V = 2.0\; \rm L$ and $P = 355\; \rm mmHg$ . Hence, $\displaystyle n_2 = (P\cdot V)/(R \cdot T) = \frac{(2.0\; \text{L}) \cdot (355\; \text{mmHg})}{R\cdot T}$ .

After mixing, $V = 2.0 + 3.0 = 5.0\; \rm L$ . Assuming that temperature $T$ stays the same.

$\displaystyle n_1 + n_2 = \frac{(3.0\; \text{L}) \cdot (145\; \text{mmHg})}{R\cdot T} + \frac{(2.0\; \text{L}) \cdot (355\; \text{mmHg})}{R\cdot T}$ .

Apply the equation $\displaystyle P = (n \cdot R \cdot T)/(V)$ to find the pressure after mixing.

$\begin{aligned}P &= \displaystyle \frac{\displaystyle \displaystyle \left(\frac{(3.0\; \text{L}) \cdot (145\; \text{mmHg})}{R\cdot T} + \frac{(2.0\; \text{L}) \cdot (355\; \text{mmHg})}{R\cdot T}\right) \cdot R \cdot T}{5.0\; \rm L} \n &= (3.0\; \rm L * 145\; \rm mmHg + 2.0\; \rm L * 355\; \rm mmHg)/(5.0\; \rm L) \n &\approx 229\; \rm mmHg\end{aligned}$ .

Answer:

The total pressure is 229 atm

Explanation:

Step 1: Data given

Volume of helium flask = 3.0 L

Pressure helium flask = 145 mm Hg

Volume of argon flask = 2.0 L

Pressure argon flask = 355 mmHg

total volume = 5.0 L

Step 2: Partial pressure helium

pHe = 145 *(3/5) = 87.0 atm

Step 3: Calculate pressure argon

pAr = 355*(2/5) = 142.0 atm

Step 4: Calculate total pressure

Total pressure = 87.0 + 142.0 atm

Total pressure = 229 atm

The total pressure is 229 atm

The movement of which layer of Earth drives the motion of the plates on Earth’s crust? Upper mantle
Lower mantle
Outer core
Inner core

Answers

Final answer:

The movement of the upper mantle and the tectonic plates of the Earth's lithosphere results in the movement of the Earth's crust. The tectonic plates float on the asthenosphere, a semi-fluid part of the upper mantle, and are driven by convection currents.

Explanation:

The movement of Earth's plates is driven by the upper mantle. The Earth's lithosphere, which is the topmost layer consisting of the crust and the rigid upper part of the mantle, is broken up into tectonic plates. These tectonic plates float on the semi-fluid layer of the mantle known as the asthenosphere. Convection currents in the asthenosphere, which is part of the upper mantle, move these plates. Thus, the upper mantle has a significant role in the movement of the Earth's crust.