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3 years ago

- Reaction without catalyst

Chemistry

1 answer:

Amanda [17]3 years ago

6 0

Answer: The reaction has a lower activation energy with the catalyst present than it has without it.

Explanation:

If you project both curves on the Y axis, which represents the amount of energy required for activating the reaction, you can see that the red curve has a lower value than the black curve. This makes perfect sense, since the purpose of a catalyst is of lowering the energy required for activating a reaction.

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Using the phase diagram for CO2, what phase is carbon dioxide in at -60C and 1 atm pressure? A. Solid B. Gas C. At the melting p

ANTONII [103]

Answer:

B. Gas.

Explanation:

Kindly, see the attached image of CO₂ phase diagram.

Extrapolating the T from - 60.0°C and P from 1.0 atm, you will find that CO₂ is in the gas phase.

So, the right choice is: B. Gas.

7 0

3 years ago

Read 2 more answers

A sample of CaCO3(s) is introduced into a sealed container of volume 0.638 L and heated to 1000 K until equilibrium is reached.

JulsSmile [24]

Answer:

the mass of CaO present at equilibrium is, 0.01652g

Explanation:

$K_p = [CO_2]$ = 3.8×10⁻²

Now we have to calculate the moles of CO₂

Using ideal gas equation,

PV =nRT

P = pressure of gas = 3.8×10⁻²

T = temperature of gas = 1000 K

V = volume of gas = 0.638 L

n = number of moles of gas = ?

R = gas constant = 0.0821 L.atm/mole.k

$\frac{3.8 * 10^2 * 0.638}{0.0821 * 1000} \\= 2.95 * 10^-^4$

Now we have to calculate the mass of CaO

mass = 2.95 * 10 ⁻⁴ × 56

= 0.01652g

Therefore,

the mass of CaO present at equilibrium is, 0.01652g

7 0

3 years ago

Which of the following are examples of a physical property of matter? Select all that apply.

NemiM [27]

Answer:

what are the options i cant see em

Explanation:

6 0

3 years ago

The reaction 2 A + B2 2 AB follows this mechanism:

Vlada [557]

This is too hard to answer

8 0

3 years ago

11. if the ph of a solution increases from 2.0 to 4.0, the h3o^ ion concentration o a decreases by a factor of 2. b. decreases b

Wittaler [7]

Option (B) is the right answer.

Hydronium ion ( $H_{3}O^{+}$ ) concentration decreases by the <u>factor of 100</u>, if the pH of a solution increases from 2.0 to 4.0.

The hydrogen ion concentration in water is expressed by pH. Specific to aqueous solutions, pH is the <u>negative logarithm</u> of the hydrogen ion (H+) concentration (mol/L) : $pH = -log_{10}[H_{3}O^{+} ]$

Acidic solutions are those with a pH under 7, and basic solutions are those with a pH over 7. At this temperature, solutions with a pH of 7 are neutral (e.g.<u> pure water</u>). The pH neutrality <u>relies on temperature, falling below 7 if the temperature rises above 25 °C</u>.

<h3>Given: </h3>

pH1( initial pH) = 2.0

pH2( initial pH) = 4.0

[H3O+] = initial hydronium concentration

[H3O+]* = final hydronium concentration

<h3>Formula used : </h3>

$pH = -log_{10}[H_{3}O^{+}]$

<h3>Solution: </h3>

$pH = - log_{10}[H_{3}O^{+}] \\\\= > 10^{-pH} = [H_{3}O^{+}] \\\\similarly, \\\\10^{-pH} = [H_{3}O^{+}]*\\\\ = > 10^{-4} = [H_{3}O^{+}]*\\\\Now, \frac{[H_{3}O^{+}]*}{[H_{3}O^{+}]} = 10^{-2}$

Thus , the concentration of hydronium ion decreases by 100.

To learn more about pH :

brainly.com/question/15289741

#SPJ4

8 0

2 years ago