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Radda [10]
3 years ago
13

Figure 1 (Use this figure to answer questions 6,7, and 8. Assume that the height at point

Chemistry
1 answer:
nadezda [96]3 years ago
8 0

Answer:

JWBVH

Explanation:

NWSBWHSBHS

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What elemental classification does oxygen belong to?
Lesechka [4]
The elemental classification for oxygen would be non-metal. It is located in period number 2 and group number 16. It has an atomic number of 8. At room temperature, it exists as a gas. Hope this answers the question. Have a nice day.
6 0
3 years ago
Read 2 more answers
For a second order reaction, the half-life is equal to:_____.
gtnhenbr [62]

Answer:

Half life = 1 / k[Ao]

Explanation:

From:

1/ [A] = kt + 1/ [Ao]

Isolating t on its own, we have:

kt = 1 / [A] - 1 / [Ao]

t = 1 / [Ao] / k

Re-arranging we have:

t = 1 / k [Ao]

The t represents the t=half life of the second order reaction and the formula can be re-written as:

t1/2 = 1 / k [Ao]

This is so because second order reaction decreases at a much faster rate than zero and first order reactions and there slopes decreases to zero at a much faster rate.

4 0
3 years ago
HI PLEASE HELPPPL I NEED THIS DUE VERY SOON
Liono4ka [1.6K]

Answer:

A

Explanation:

I just did this question in class:))

8 0
3 years ago
PLEASE HELP
muminat

Answer:

H2O and CO

Explanation:

they both form covalent bonds because none both of the elements are non-metal. Mgo and NaF both have metals in them so they would form ionic bonds.

Covalent bonds, two non-metal

Ionic bonds, a metal and a non-metal

5 0
3 years ago
Read 2 more answers
The aromatic hydrocarbon cymene (C10H14) is found in nearly 100 spices and fragrances, including coriander, anise, and thyme. Th
andrezito [222]

Answer : The thermal energy produced during the complete combustion of one mole of cymene is -7193 kJ/mole

Explanation :

First we have to calculate the heat released by the combustion.

q=c\times \Delta T

where,

q = heat released = ?

c = specific heat of calorimeter = 3.640kJ/^oC

\Delta T = change in temperature = 19.35^oC

Now put all the given values in the above formula, we get:

q=3.640kJ/^oC\times (19.35)^oC

q=70.43kJ

Thus, the heat released by the combustion = 70.43 kJ

Now we have to calculate the molar enthalpy combustion.

\Delta H=-\frac{q}{n}

where,

\Delta H = molar enthalpy combustion = ?

q = heat released = 70.43 kJ

n = number of moles cymene = \frac{\text{Mass of cymene}}{\text{Molar mass of cymene}}=\frac{1.608g}{164.22g/mol}=0.009792mole

\Delta H=-\frac{70.43kJ}{0.009792mole}=-7193kJ/mole

Therefore, the thermal energy produced during the complete combustion of one mole of cymene is -7193 kJ/mole

4 0
3 years ago
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