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beks73 [17]
3 years ago
15

Carbon dioxide and water react to form bicarbonate ion and hydronium ion. Hyperventilation (rapid breathing) causes more carbon

dioxide to be exhaled than normal. How will hyperventilation affect the pH of blood?
this is about a unit on shifting equilibrium and the common-ion effect so try to connect the explanation to those ideas please!
Chemistry
1 answer:
Juliette [100K]3 years ago
4 0
Hyperventilation<span> will blow off carbon dioxide which reduces the alkaline component of the </span>blood<span>, resulting in acidosis and a lower </span>blood pH<span>. (See Andromeda Strain). This is why re-breathing into a bag to increase carbon dioxide in your </span>blood will make you feel less faint. Basically <span>It increases the pH ... you can look at CO2 as an acid ... and when reduced ... alkalinization of the pH occurs</span> 
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If you have a substance, would it have the same density no matter what mass of the substance you have?
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Which change will cause more CO2 to form in a closed container?​
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Option C Removing Na₂CO₃

Option E Heating the container.

Explanation:

The equation for the reaction is given below:

2NaHCO₃ (s) <=> Na₂CO₃ (s) + CO₂ (g) + H₂O (g)

Enthalpy change (ΔH) = 136 KJ

To obtain more CO₂ do the following:

1. Add more NaHCO₃

From chemical equilibrium, adding more NaHCO₃ means the reactant has increase. Thus, it (the reactant) will react to form more product (CO₂)

2. Removing any of the products. Removing any of the products implies that more reactants are in the reaction vessel than the product. Thus, the reactants will react to produce more products (CO₂)

3. Heating the container. Heating the container will lead to an increase in the temperature of the reaction. Since the enthalpy change (ΔH) is positive it means the reaction is endothermic. Thus, heating the container i.e increasing the temperature will favours the forward reaction i.e more products will be obtained.

NOTE: Pressure has no effect in the reaction system since there is no gaseous reactants.

Considering the options given above, C and E gives the correct answer to the question.

8 0
2 years ago
How many grams of AgCl will be produced from 5.00 g of NaCl and 103 g of AgNO3?<br> grams
lapo4ka [179]

Answer:

12.3 g.

Explanation:

Whenever a similar problem is involved, we need to write the chemical reaction representing the net change, as well as due to the fact that we need to know the stoichiometry involved.

Sodium chloride reacts with silver nitrate in a double displacement reaction to produce a cation exchange, that is, we produce silver chloride and sodium nitrate given by the following balanced chemical equation:

AgNO_3 (aq)+NaCl(aq)\rightarrow AgCl(s)+NaNO_3 (aq)

According to the balanced chemical equation, the molar stoichiometry of silver nitrate to sodium chloride is 1 : 1.

Let's find moles of each substance to determine the limiting reactant. To do this, divide mass of each component by its molar mass:

n_{NaCl}=\frac{5.00 g}{58.44 \frac{g}{mol} }= 0.08556 mol\\n_{AgNO_3}=\frac{103 g}{169.87 \frac{g}{mol}}= 0.6063 mol

Since the stoichiometry of this reaction is 1 : 1, we can compare the moles directly. Notice that the number of moles of NaCl is lower than the number of moles of silver nitrate. This means NaCl is the limiting reactant.

According to the balanced chemical equation, 1 mole of NaCl produces 1 mole of AgCl, so the amount of AgCl would be:

n_{AgCl}=n_{NaCl}=0.08556 mol

In order to convert this into mass, let's multiply by the molar mass of AgCl:

m_{AgCl}=0.08556 mol\cdot143.32 \frac{g}{mol}=12.3 g

5 0
3 years ago
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