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Debora [2.8K]
3 years ago
12

If a solution contains 3.00 moles of NaCl in 8.00 liters of water, what is the molarity?

Chemistry
1 answer:
ExtremeBDS [4]3 years ago
8 0

Answer:

0.375 M

Explanation:

molarity = number of moles of solute/ number of L solution = 3.00 mol/8.00 L=

= 0.375 mol/L = 0.375 M

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Name the following alkyne:
Lady bird [3.3K]

Answer:

There isn't any picture for me to see

have a good day :)

Explanation:

3 0
3 years ago
A 10-ft moving truck has a volume capacity of 402 cubic feet, which is equivalent to 1.138 x 10⁷ milliliters. What mass of silve
steposvetlana [31]

Answer:

The mass of silver is 1.19\times 10^{14}\ Mg

Explanation:

Given that,

The volume of the truck is 402 cubic feet or 1.138 x 10⁷ mm.

The density of silver is 10.49 g/mL.

We need to find the mass of silver that will fit in this moving truck. Density equals mass divided by volume. So,

d=\dfrac{m}{V}\\\\\text{where m is mass}\\\\m=d\times V\\\\m=10.49\ g/mL\times 1.138 \times 10^7\ mL\\\\m=119376200\ g

1 gram = 10⁻⁶ Megagram

119376200=1.19\times 10^{14}\ Mg

Hence, the mass of silver is 1.19\times 10^{14}\ Mg

4 0
3 years ago
Select the correct answer
amm1812

Answer:

  C  The experiment shows that the red substance experienced a chemical change.

Explanation:

Apparently, adding heat caused the red substance to decompose into a gas and a metallic liquid. If it were simply a phase change, the original red substance could be expected to return when the temperature cooled. Because the substance apparently decomposed, it is clearly not an element. At no point in the experiment is there any evidence of a plasma being formed.

The observed decomposition is a chemical change.

8 0
3 years ago
Calcium hydride (cah2) reacts with water to form hydrogen gas: cah2(s) + 2h2o(l) → ca(oh)2(aq) + 2h2(g) how many grams of cah2 a
andreev551 [17]
Using the ideal gas law equation, we can find the number of H₂ moles produced.
PV = nRT
Where P - pressure - 0.811 atm x 101 325 Pa/atm = 82 175 Pa
V - volume - 58.0 x 10⁻³ m³
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature - 32 °C + 273 = 305 K
substituting these values in the equation,
82 175 Pa x 58.0 x 10⁻³ m³ = n x 8.314 Jmol⁻¹K⁻¹ x 305 K
n = 1.88 mol 

The balanced equation for the reaction is as follows;
CaH₂(s) + 2H₂O(l) --> Ca(OH)₂(aq) + 2H₂(g)
stoichiometry of CaH₂ to H₂ is 1:2
When 1.88 mol of H₂ is formed , number of CaH₂ moles reacted = 1.88/2 mol
therefore number of CaH₂ moles reacted = 0.94 mol
Mass of CaH₂ reacted - 0.94 mol x 42 g/mol  = 39.48 g of CaH₂ are needed
3 0
3 years ago
A sample of chlorine gas fills a vessel at a temperature of 37oC. The vessel has a volume of 3L and experiences a pressure of 3a
Iteru [2.4K]

Answer:

25.1 g is the mass of chlorine in the sample

Explanation:

P . V = n . R . T

We apply the Ideal Gases Law to solve the excersise.

We need to convert the T°C to T°K → 37°C + 273 = 310K

We replace data: 3 atm . 3L = n . 0.082 L.atm /mol.K . 310K

9 atm.L / (0.082 L.atm /mol.K . 310K) = n → 0.354 moles

We convert the moles to mass, to reach the answer

0.345 mol . 70.9g / 1mol = 25.1 g

7 0
3 years ago
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