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trapecia [35]
3 years ago
14

Describe the law of conservation of mass and how it applies to chemical reactions.

Chemistry
1 answer:
Lera25 [3.4K]3 years ago
7 0

Answer:

the law of conservation of mass is whatever goes into a reaction comes out nothing is lost or gianed.

Explanation:

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How much heat, in kJ, will be absorbed by a 25.0 g piece of aluminum (specific heat = 0.930 J/g・°C) as it changes temperature fr
faust18 [17]

Answer:

quantity of heat=mc*theta

=25*0.930(76-25)

=25*0.930*51

=1185.75J

=11.9kJ

4 0
2 years ago
An impure sample of table salt that weighed 0.8421 g, when dissolved in water and treated with excess AgNO3, formed 2.044 g of A
Lilit [14]

Answer:

99.24%.

Explanation:

  • NaCl reacted with AgNO₃ as in the balanced equation:

<em>NaCl + AgNO₃ → AgCl(↓) + NaNO₃,</em>

1.0 mol of NaCl reacts with 1.0 mol of AgNO₃ to produce 1.0 mol of AgCl and 1.0 mol of NaNO₃.

  • We need to calculate the no. of moles of AgCl produced:

no. of moles of AgCl = mass/molar mass = (2.044 g)/(143.32 g/mol) = 0.0143 mol.

  • Now, we can calculate the no. of moles of NaCl that can precipitated as AgCl (0.0143 mol), these moles represents the no. of moles of pure NaCl in the sample:

<em>using cross multiplication:</em>

1.0 mol of NaCl produce → 1.0 mol of AgCl, from the stichiometry.

∴ 0.0143 mol of NaCl produce → 0.0143 mol of AgCl.

  • Now, we can get the mass of puree NaCl in the sample:

mass of pure NaCl = (no. of moles of pure NaCl)(molar mass of NaCl) = (0.0143 mol)(58.44 g/mol) = 0.8357 g.

∴ The percentage of NaCl in the impure sample = [(mass of pure NaCl)/(mass of the impure sample)] x 100 = [(0.8357 g)/(0.8421 g)] x 100 = 99.24%.

4 0
3 years ago
To prepare the cooling system for an ice cream freezer, the chef adds 59.7 g of salt (NaCl) to 1433.3 g of ice. Predict the lowe
nordsb [41]

Answer: The entire water/ice solution is at the melting/freezing point, 32°F (0°C). Adding rock salt — or any substance that dissolves in water — disrupts this equilibrium.

Explanation: Hope this helps! Have a great day :)

7 0
3 years ago
An aqueous solution of HNO2 is poured onto a solid pile of SrCO3. Identify the net ionic equation for this reaction.
Eddi Din [679]

Answer:

D) SrCO3(s) + 2 HNO2(aq) → Sr(NO2)2 + H2O + CO2(g)

Explanation:

When an acid react with carbonate, it produces nitrate, carbon-dioxide gas and water molecule. When nitrous acid react with Strontium carbonate, three products are formed i. e. Strontium nitrate, carbon-dioxide gas and water. In the reaction, both nitrous acid and Strontium carbonate exchange their partners with each other and forming a different products.

6 0
3 years ago
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Acetone, the solvent in nail polish remover, has a density of 0.761 g/ml What is the volume of 25.0g of acetone
Jlenok [28]

Answer: 100.0g

Explanation:

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1 year ago
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