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navik [9.2K]
3 years ago
13

Why is a changing ocean temperature of only one or 2 degrees so concerning?

Chemistry
1 answer:
gregori [183]3 years ago
7 0
<span>One degree Celsius indicates the same temperature change as one </span>
You might be interested in
What mass of hydrogen is produced when 49.0 grams of sodium reacts with 30.0 grams of water
nekit [7.7K]

Answer:

the mass of the products must equal the mass of reactants. which means the total mass is 10 grams.

Explanation:

4 0
3 years ago
Gastric juice is made up of substances secreted from parietal cells, chief cells, and mucous-secreting cells. The cells secrete
neonofarm [45]

Answer:

The amount of energy required to transport hydrogen ions from a cell into the stomach is 37.26KJ/mol.

Explanation:

The free change for the process can be written in terms of its equilibrium constant as:

ΔG° = -RTInK_(eq)

where:

R= universal gas constant

T= temperature

K_eq= equilibrum constant for the process

Similarly, free energy change and cell potentia; are related to each other as follows;

ΔG= -nFE°

from above;

F = faraday's constant

n = number of electrons exchanged in the process; and  

E = standard cell potential

∴ The amount of energy required for transport of hydrogen ions from a cell into stomach lumen can be calculated as:

ΔG° = -RTInK_(eq)

where;

[texK_eq[/tex]=\frac{[H^+]_(cell)}{[H^+(stomach lumen)]}

For transport of ions to an internal pH of 7.4, the transport taking place can be given as:

H^+_{inside} ⇒ H^+_{outside}

Equilibrum constant for the transport is given as:

K_{eq}=\frac{[H^+]_{outside}}{[H^+]_{inside}}

=\frac{[H^+]_{cell}}{[H^+]_{stomach lumen}}

[H^+]_{cell}= 10⁻⁷⁴

=3.98 * 10⁻⁸M

[H^+]_{stomach lumen} = 10⁻²¹

=7.94 * 10⁻³M

Hence;

K_{eq}=\frac{[H^+]_{cell}}{[H^+]_{stomachlumen}}

=\frac{3.98*10^{-8}}{7.94*10{-3}}

= 5.012 × 10⁻⁶

Furthermore, free energy change for this reaction is related to the equilibrium concentration given as:

ΔG° = -RTInK_(eq)

If temperature T= 37° C ; in kelvin

=37° C + 273.15K

=310.15K; and

R-= 8.314 j/mol/k

substituting the values into the equation we have;

ΔG₁ = -(8.314J/mol/K)(310.15)TIn(5.0126*10^{-6})

= 31467.93Jmol⁻¹

≅ 31.47KJmol⁻¹

If the potential difference across the cell membrane= 60.0mV.

Energy required to cross the cell membrane will be:

ΔG₂ = -nFE°_{membrane}

ΔG₂ = -(1 mol)(96.5KJ/mol/V)(60*10^{-3})

= 5.79KJ

Therefore, for one mole of electron transfer across the membrane; the energy required is 5.79KJmol⁻¹

Now, we  can calculate the total amount of energyy required to transport H⁺ ions across the membrane:

Δ G_{total} = G_{1}+G_{2}

= (31.47+5.79) KJmol⁻¹

= 37.26KJmol⁻¹

We can therefore conclude that;

   The amount of energy required to transport ions from cell to stomach lumen is 37.26KJmol⁻¹

5 0
3 years ago
Problem PageQuestion Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceutica
Feliz [49]

The question is incomplete, here is the complete question:

Sulfuric acid is essential to dozens of important industries from steel making to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial chemical, and world production exceeds  2.0×10¹¹ kg per year.

The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces 1.8 kg of solid sulfur and 10.0 atm of oxygen gas at 650°C  into an evacuated 50.0 L tank. The engineer believes Kp = 0.099 for the reaction at this temperature.

Calculate the mass of solid sulfur he expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits.

<u>Answer:</u> The mass of solid sulfur that will be consumed is 19. grams

<u>Explanation:</u>

The chemical equation for the formation of sulfur dioxide gas follows:

                    S(s)+O_2\rightarrow SO_2(g)

<u>Initial:</u>                   10.0

<u>At eqllm:</u>              10-x         x

The expression of K_p for above equation follows:

K_p=\frac{p_{SO_2}}{p_{O_2}}

We are given:

K_p=0.099

Putting values in above expression, we get:

0.099=\frac{x}{10-x}\\\\x=0.901atm

Partial pressure of sulfur dioxide = x = 0.901 atm

To calculate the number of moles, we use the equation given by ideal gas which follows:

PV=nRT

where,

P = pressure of the sulfur dioxide gas = 0.901 atm

V = Volume of the gas = 50.0 L

T = Temperature of the gas = 650^oC=[650+273]K=923K

R = Gas constant = 0.0821\text{ L. atm }mol^{-1}K^{-1}

n = number of moles of sulfur dioxide gas = ?

Putting values in above equation, we get:

0.901atm\times 50.0L=n\times 0.0821\text{ L. atm}mol^{-1}K^{-1}\times 923K\\\\n=\frac{0.901\times 50.0}{0.0821\times 923}=0.594mol

By stoichiometry of the reaction:

1 mole of sulfur dioxide gas is produced from 1 mole of sulfur

So, 0.594 moles of sulfur dioxide gas will be produced from = \frac{1}{1}\times 0.594=0.594mol of sulfur

  • To calculate the number of moles, we use the equation:

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

Moles of sulfur = 0.594 moles

Molar mass of sulfur = 32 g/mol

Putting values in above equation, we get:

0.594mol=\frac{\text{Mass of sulfur}}{32g/mol}\\\\\text{Mass of sulfur}=(0.594mol\times 32g/mol)=19.008g

Hence, the mass of solid sulfur that will be consumed is 19. grams

8 0
3 years ago
What is the best explanation for the frequency of eclipses?
Katarina [22]

Answer:A

Explanation:

7 0
3 years ago
if 0.40 mol of h2 and .15 mol of o2 were to reat as completely as possible to produce h20, what mass of the reactant would remai
Sveta_85 [38]

Answer:

0.2g

Explanation:

Given parameters:

Number of moles of H₂  = 0.4mol

Number of moles of O₂  = 0.15mol

Unknown:

Mass of reactant that would remain = ?

Solution:

To solve this problem, we need to know the limiting reactant which is the one in short supply in the given reaction.

  The expression of the reaction is :

                2H₂  + O₂  →   2H₂O

                    2 mole of H₂ will combine with 1 mole of O₂

But given;    0.4 mole of H₂ we will require \frac{0.4}{2}  = 0.2mole of O₂

The given number of oxygen gas is 0.15mole and it is the limiting reactant.

Hydrogen gas is in excess;

       1 mole of oxygen gas will combine with 2 mole of hydrogen gas

    0.15 mole of oxygen gas will require 0.15 x 2  = 0.3mole of hydrogen gas

Now, the excess mole of hydrogen gas  = 0.4 mole  - 0.3 mole  = 0.1mole

  Mass of hydrogen gas  = number of mole x molar mass

  Molar mass of hydrogen gas  = 2(1) = 2g/mol

   Mass of hydrogen gas  = 0.1 x 2 = 0.2g

8 0
3 years ago
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