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Alexeev081 [22]

3 years ago

11

The graph above shows the progress of a chemical reaction. Based on the graph, which of the following is true?

2 answers:

rusak2 [61]3 years ago

4 0

In the given graph, it can be seen that the energy consumed by Reaction B is much lower compared to Reaction A during which both of the reaction reached the peak. This now suggest that because the reaction energy required for B is lowered, then the answer to this item is the second option.

algol [13]3 years ago

3 0

Answer: Reaction A is not enzyme-catalyzed, while reaction B is enzyme-catalyzed

Explanation:

The minimum energy required by the reactants to cross the energy barrier is called as activation energy. The use of enzyme lowers the activation energy as it takes the reaction through a different pathway which is lower in energy. Thus a enzyme catalyzed reaction has low activation energy as compared to a non catalyzed reaction.

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Explain what causes air pressure:

Sidana [21]

Gravity pulling the mass of the atmosphere toward the center of the earth. Atmosphere includes air, water vapor, etc.

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3 years ago

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The density of liquid oxygen at its boiling point is 1.14 kg/L , and its heat of vaporization is 213 kJ/kg . How much energy in

-Dominant- [34]

<span>2.28 kg x 213 kJ/kg = 486 kJ = 4.86E+05 J</span>

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3 years ago

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vladimir2022 [97]

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Explanation:

7 0

2 years ago

**PLEASE SHOW YOUR WORK**Calculate how much energy would be necessary to convert 250.0 grams of ice at -30°C to steam at 145°C.

garri49 [273]

Answer:

Q= mc∆T(ice) + mLF(ice) + mc∆T(water) + mLV(water) + mc∆T(steam)

m=250 g = 0.25 kg = ¼ kg c(ice)= 2100 J/kg.K c(water)= 4200 J/kg.K LF(ice)= 333.7 kJ/kg LV(water)= 2256 kJ/kg c(steam)= 2080 J/kg.K

Explanation:

Q= ¼ × 2100 × (0°-(-30°)) + ¼ × 333700 + ¼ × 4200 × (100°-0°) + ¼ × 2256000 + ¼ × 2080 × (145°-100°)

Q= 15750 + 83425 + 105000 + 564000 + 23400

Q= 791575 J

7 0

2 years ago

If you have 730 moles of a gas at 304 Kelvin in a 4.50 Liter container what

vova2212 [387]

Answer:

4046atm

Explanation:

For this question you can use the ideal gas law,

<em /> $PV=nRT$ <em />

Where P is pressure, V is volume, n is moles of substance, R is the constant, and T is the temperature.

Because of the units given, R will equal .08026 $P=4046 atm$

<h3>Rearrange the equation to solve for pressure:</h3>

$P=\frac{nRT}{V}$

Then, plug in the values (I'll be excluding units for simplicity, but they all cancel out for pressure in atm):

$P=\frac{(730)(.08206)(304)}{4.5}$

This will give you:

$P=4046atm$

3 0

2 years ago