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3 years ago

Identify the type of chemical reaction. H2CO3 H2O + CO2

Chemistry

2 answers:

Triss [41]3 years ago

3 0

The type of chemical reaction in

H2CO3 → H2O+ CO2 is decomposition reaction

Decomposition reaction is a reaction which involve the breakdown of a single compound into two or more elements or compounds. The reaction above is a decomposition reaction because H2CO3 decomposes to yield CO2 and H2O

stepladder [879]3 years ago

3 0

<span>We have the reaction: CO2 + H2O (yield arrow)> H2CO3. It means that carbon dioxide + water makes H2CO3 or Carbonic Acid. This reaction is also reversible, so H2CO3 (yield arrow)> CO2 + H2O. This reversible reaction gives a name to reaction: Carbonic anhydrase. It means that it removes the water molecul from Carbonic Acid. Answer: This is a reversible reaction : Carbonic anhydrase.</span>

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Dafna11 [192]

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3 years ago

Which option is a valid hypothesis in the correct format?

Rashid [163]

Answer:

4. If cotton plants need a consistent amount of water to grow steadily, then a cotton plant that displays steady growth will receieve 100 mL of water every day.

Explanation:

Hypotheses are written in the format of "If... then...". It should include information on both variables to arrive at a conclusion point.

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2 years ago

If a negatively charged object is brought near a neutrally charged sphere, what will happen?

Verizon [17]

Answer:

the protons will jump to the negatively charged object making it negatively charged

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2 years ago

Identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid and the conjugate base for each of the following r

Vlad1618 [11]

Answer:

Acids → H₂CO₃ from equilibrium 1 and water, from equilibrium 2.

Bases → Water from equilibrium 1 and ammonia from equilibrium 2.

In 1st equilibrium, H₃O⁺ is the conjugate acid and HCO₃⁻ the conjugate base.

In 2nd equilibrium, NH₄⁺ is the conjugate acid, and OH⁻, the conjugate base.

Explanation:

By the Bronsted-Lowry you know that acids are the one that release protons and base are the ones that catch them.

For the first equilibrium:

H₂CO₃(aq) + H₂O(l) ⇄ H₃O⁺(aq) + HCO₃⁻(aq)

Carbonic acid is the acid → It donates the proton to water, so the water becomes the base. As H₂CO₃ is the acid, the bicarbonate is the conjugate base (it can accept the proton from water to become carbonic acid, again) and the hydronium is the conjugate acid (it would release the proton to become water).

For the second equilibrium:

NH₃(aq) + H₂O(l) ⇄ NH₄⁺ (aq) + OH⁻(aq)

This is the opposite situation → Water relase the proton to ammonia, that's why water is the acid and NH₃, the base (it accepted to become ammonium). The NH₄⁺ is the conjugate acid (it can release the H⁺ to become ammonia) and the OH⁻ is the conjugate base (It can accept the proton to become water, again).

5 0

3 years ago

The following questions pertain to a system contains 122 g CO(g) in a 0.400 L container at -71.2 degrees C.

7nadin3 [17]

Answer:

a. P = 182 atm

Explanation:

Data Given:

amount of CO = 122g

Volume of CO = .400 L

Temperature of CO = -71.2°C

Convert the temperature to Kelvin

T = °C + 273

T = -71.2 + 273

T = 201.8 K

a. Calculate the pressure exerted by the CO(g) in this system using the ideal gas equation (P) = ?

Solution:

To calculate Pressure by using ideal gas formula

PV = nRT

Rearrange the equation for Pressure

P = nRT / V . . . . . . . . . (1)

where

P = pressure

V = Volume

T= Temperature

n = Number of moles

R = ideal gas constant = 0.08206 L.atm / mol. K

For this we have to know the mole of the gas and the following formula will be used

no. of moles = mass in grams / molar mass . . . . . . (2)

Molar mass of CO = 12 + 16 = 28 g/mol

Put values in equation 2

no. of moles = 122 g / 28 g/mol

no. of moles = 4.4 mol

Now put the value in formula (1) to calculate Pressure for CO

P = 4.4 x 201.8 K x 0.08206 (L.atm/mol. K) / 0.400 L

P = 182 atm

So the pressure will be 182 atm

__________

b. Data Given:

Actual pressure exerted by CO = 145 atm

expected pressure exerted by CO = 182 atm

why the actual pressure is less than what would be expected = ?

Explanation:

This is because of the deviation from ideal behavior of real gases.

The real gases approach to ideal behavior under very high temperature and very low pressure.

But CO deviate from ideal behavior to give expected value for pressure, because it behave at high pressure and low temperature.

This non-ideal behavior is due to two postulate of ideal behavior

gas molecules have negligible volume
Gas molecules have negligible inter-molecular interaction

but these postulates not obeyed under real condition. so we calculated the pressure using ideal condition values for gas and obtained the expected value for pressure but the actual pressure value was detected under normal condition.

8 0

3 years ago