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2 years ago

What front involves three air masses? Please don't guess, give an accurate answer

Chemistry

1 answer:

dmitriy555 [2]2 years ago

3 0

Answer:

It is an Occluded front

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The gas in a balloon has a volume of 2 Lat a temperature of 301 K. What will be the final temperature (in K) when the volume exp

Blizzard [7]

Answer:

Final temperature = 1279.25 K

Explanation:

We can solve this using the formula for Charles law since we are given volume and temperature.

From Charles law, we know that;

V1/T1 = V2/T2

Where;

T1 is the initial temperature

V1 is the initial volume

T2 is the final temperature

V2 is the final volume

We are given;

V1 = 2 L

T1 = 301 K

V2 = 8.5 L

Thus, making T2 the subject, we have;

T2 = V2•T1/V1

Plugging in the relevant values;

T2 = 8.5 × 301/2

T2 = 1279.25 K

4 0

3 years ago

Mass in mg salt sugar chalk sand water

STALIN [3.7K]

Its 470mg k dude or dudette

6 0

3 years ago

The Second Law of Thermodynamics states that: Select one:

lianna [129]

Answer:

In the total entropy of an isolated system, the thermal energy per unit temperature that is unavailable for doing useful work can never decrease.

8 0

2 years ago

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl4(g) + (1/2)O

madam [21]

The question is incomplete, here is the complete question:

Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine.

$CCl_4(g)+\frac{1}{2}O_2(g)\rightleftharpoons COCl_2(g)+Cl_2(g);K_c=4.4\times 10^9$ at 1,000 K

Calculate Kc for the reaction $2CCl_4(g)+O_2(g)\rightleftharpoons 2COCl_2(g)+2Cl_2(g)$

Answer: The value of $K_c'$ for the final reaction is $1.936\times 10^{19}$

Explanation:

The given chemical equations follows:

$CCl_4(g)+\frac{1}{2}O_2(g)\rightleftharpoons COCl_2(g)+Cl_2(g);K_c$

We need to calculate the equilibrium constant for the equation, which is:

$2CCl_4(g)+O_2(g)\rightleftharpoons 2COCl_2(g)+2Cl_2(g)$

As, the final reaction is the twice of the initial equation. So, the equilibrium constant for the final reaction will be the square of the initial equilibrium constant.

The value of equilibrium constant for net reaction is:

$K_c'=(K_c)^2$

We are given:

$K_c=4.4\times 10^9$

Putting values in above equation, we get:

$K_c'=(4.4\times 10^9)^2=1.936\times 10^{19}$

Hence, the value of $K_c'$ for the final reaction is $1.936\times 10^{19}$

3 0

3 years ago

Ionic character of lih

adoni [48]

I believe LiH becomes HF

8 0

3 years ago