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11111nata11111 [884]
3 years ago
10

To help relieve heartburn, a person should take medicine that is

Chemistry
2 answers:
Sav [38]3 years ago
3 0

Prescribed to you by your doctor.

I would use an over the counter antacids for occasional heart burn. If there are symptoms of acid reflux I would suggest a histamine blocker, or H2-Blockers, such as Ranitidine (Zantac) and Famotidine (Pepcid)

miv72 [106K]3 years ago
3 0

Answer:

Explanation:

Over-the-counter (OTC) antacids and acid blockers are the most commonly used medicines for treating heartburn.

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Which statement is TRUE about enzymes?
nikklg [1K]

Answer:

the answer is

c

i guessed btw

Explanation:

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3 years ago
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.65 x 103 at a certain temperature. Find the
Aleks [24]

Answer:

6.97 atm was the equilibrium pressure of HBr .

Explanation:

The value of the equilibrium constant =K_p=1.65\times 10^3

H_2+Br_2\rightleftharpoons 2HBr

Initially:

0             0                 7.10 atm

At equilibrium

x              x                 (7.10-2x)

The expression of equilibrium constant can be written as:

K_p=\frac{p_{HBr}}{p_{H_2}\times p_{Br_2}}

1.65\times10^3=\frac{(7.10-2x)}{x^2}

Solving for x:

x = 0.065

Partial pressure of HBr at equilibrium :(7.10 - 2 × 0.065) atm = 6.97 atm

6.97 atm was the equilibrium pressure of HBr .

7 0
3 years ago
C2H4(g) + H2(g) → C2H6(g) ΔH = –137.5 kJ; ΔS = –120.5 J/K Calculate ΔG at 25 °C and determine whether the reaction is spontaneou
Katen [24]

Answer:-ΔG=-101.5KJ

Explanation:We have to calculate ΔG for the reaction  so using the formula given in the equation we can calculate the \Delta G for the reaction.

We need to convert the unit ofΔS in terms of KJ/Kelvin as its value is given in terms of J/Kelvin

Also we need to convert the temperature in Kelvin as it is given in degree celsius.

\Delta H=-137.5\\ \Delta S=-120J/K\\ \Delta S=-0.120KJ/K\\ T=25^{.C}\\ T=273+25=298 K\\ \Delta G=?\\ \Delta G=\Delta H-T\Delta S\\\Delta G=-137.5KJ-(278\times -0.120)\\ \Delta G=-137.5+35.76\\\Delta G=-101.74\\\Delta G=Negative

After calculating forΔG we found that the value ofΔG is negative and its value is -101.74KJ

 For a  reaction to be spontaneous the value of \Delta G \ must be negative .

As the ΔG for the given reaction is is negative so the reaction will be spontaneous in nature.

In this reaction since the entropy of reaction is positive and hence when we increase the temperature term then the overall term TΔS would become more positive  and hence the value of ΔG would be less negative .

Hence the value of ΔG  would become more positive with the increase in temperature.

So we found the value of ΔG to be -101.74KJ

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