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2 years ago

Afirmar que el h20 es la formula que corresponde al agua, esto es una teoría, idea, ley, hipotesis o experimentación

Chemistry

1 answer:

frozen [14]2 years ago

6 0

Answer:

Ley.

Explanation:

En la teoría de la ciencia, la regularidad de los procesos en la naturaleza se denomina ley de la naturaleza. Las leyes naturales se diferencian de otras leyes en que los seres humanos no pueden ponerlas en vigor ni anularlas a su discreción. En tal sentido, la composición química del agua es indudablemente una ley natural, en tanto el hombre no puede modificarla sin modificar las características inherentes del agua como tal.

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The amount of heat absorbed when 5.5g of aluminum is heated from 25.0c to 95.0c the specific heat of aluminum is 0.897J/(gc)

NemiM [27]

Answer:

Q=21.99 kJ

Explanation:

4 0

2 years ago

When a 0.245-g sample of benzoic acid is combusted in a bomb calorimeter, the temperature rises 1.643 ∘C . When a 0.260-g sample

sveticcg [70]

Answer:

The heat of combustion per moles of caffeine is 4220 kJ/mol

Explanation:

Step 1: Data given

⇒ When benzoic acid sample of 0.245 grams is burned the temperature rise is 1.643 °C

⇒ When 0.260 gram of caffeine is burned, the temperature rise is 1.436 °C

⇒ Heat of combustion of benzoic acid = 26.38 kJ/g

Step 2: Calculate the heat released: for combustion of benzoic acid

0.245 g benzoic acid * 26.38 kJ/g = 6.4631 kJ

Step 3: Calculate the heat capacity of the calorimeter:

c = Q/ΔT

Q = 6.4631 kJ / 1.643°C = 3.934 kJ/ °C

Step 4: Calculate moles of a 0.260 g sample of caffeine:

Moles caffeine = Mass caffeine / Molar mass caffeine

0.260 grams/ 194.19 g/mol = 0.0013389 moles

Step 5: Calculate heat released: for combustion of caffeine

Q = c * ΔT

Q = 3.934 kJ/°C * 1.436 °C = 5.65 kJ

Step 6: Calculate the heat of combustion per mole of caffeine

5.65 kJ / 0.0013389 moles = 4219.9 kJ/mol ≈ 4220 kJ/mol

The heat of combustion per moles of caffeine is 4220 kJ/mol

4 0

3 years ago

Which compound contains both sigma and pi bonds

Misha Larkins [42]

Any compound with multiple covalent bonds

6 0

2 years ago

Read 2 more answers

Borax (na2b4o7Â·10h2o; fw = 381.372 g/mol; density = 1.73 g/ml), a primary standard, was used to standardize a solution of hno3.

SashulF [63]

0.06355391 mol The balanced equation for the reaction is Na2B4O7*10H2O + 2 HNO3 = 2 NaNO3 + 4 H3BO3 + 5 H2O So for each mole of Borax to neutralize, it takes 2 moles of HNO3. Calculate number of moles of Borax 0.2619 g / 381.372 g/mol = 0.0006867 mol Moles of HNO3 used = 0.0006867 mol * 2 = 0.0013734 mol Molarity is defined as moles per liter so divide the number of moles used by the volume in liters. So 0.0013734 / 0.02161 = 0.06355391 mol

3 0

3 years ago

21. The formation of an ionic bond involves the a transfer of electrons. b. transfer of neutrons. c. transfer of protons. d. sha

iren2701 [21]

Answer:

I think its C but if its not try A then

Explanation:

7 0

2 years ago