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11111nata11111 [884]
3 years ago
14

40 POINTS!! If all of the water is removed from a one-mole sample of Ba(OH)2·8H2O, by how many grams will the mass of the sample

be reduced?
Chemistry
1 answer:
yarga [219]3 years ago
5 0

Answer:

8H2O x 100.

Explanation:

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What is the molarity of an aqueous solution containing 1.5 moles of calcium chloride in 2.75 L of solution? A. 0.004 M B. 0.55 M
kondor19780726 [428]

Answer:

B. 0.55 M

Explanation:

Step 1: Given data

  • Moles of calcium chloride (solute): 1.5 mol
  • Volume of solution: 2.75 M

Step 2: Calculate the molarity of the aqueous solution

The molarity is a way to express the concentration of a solution. It is equal to the quotient between the moles of solute and the liters of solution.

M = moles of solute / liters of solution

M = 1.5 mol / 2.75 L = 0.55 mol/L = 0.55 M

6 0
2 years ago
To satisfy the octet rule in an ionic reaction, selenium must:
4vir4ik [10]

Answer:

Answer A

Explanation:

because it had 6 electrons in the last shell so it needs two electrons to reach 8

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2 years ago
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Using a graduated cylinder, fill a 600 mL beaker with 100 mL of water.
fomenos

Answer:

Temperature of water: 3

Reaction time: 138.5

Explanation:

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3 years ago
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What types of predictions can be made using the Periodic Table?
Andrej [43]
Periodic trends are specific patterns that are present in the periodic table that illustrate different aspects of a certain element, including its size and its electronic properties. Major periodic trends include: electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. Periodic trends, arising from the arrangement of the periodic table, provide chemists with an invaluable tool to quickly predict an element's properties. These trends exist because of the similar atomic structure of the elements within their respective group families or periods, and because of the periodic nature of the elements.
8 0
3 years ago
Determine the mass of CO2 produced by burning enough of methane to produce 1.50×102kJ of heat. CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rx
MArishka [77]

<u>Answer:</u> The mass of CO_2 produced will be 8.228 g.

<u>Explanation:</u>

We need to find the mass of carbon dioxide produced when 150 kJ of heat is released.

For the given chemical reaction:

CH_4(g)+2O_2(g)\rightarrow CO_2(g)+2H_2O(g);\Delta H^o_{rxn}=-802.3kJ

By Stoichiometry of the reaction:

802.3 kJ of energy is released when 1 mole of carbon dioxide is produced.

So, 150 kJ of energy will be release when = \frac{1}{802.3}\times 150=0.187mol of carbon dioxide is produced.

To calculate the mass of carbon dioxide, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of carbon dioxide gas = 0.187 mol

Molar mass of carbon dioxide gas = 44 g/mol

Putting values in above equation, we get:

0.187mol=\frac{\text{Mass of carbon dioxide gas}}{44g/mol}\\\\\text{Mass of carbon dioxide gas}=8.228g

Hence, the mass of CO_2 produced will be 8.228 g.

8 0
3 years ago
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