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andrey2020 [161]

3 years ago

5

Formular for calculating weight

2 answers:

ahrayia [7]3 years ago

6 0

W = mg

Weight of object = mass of object × acceleration of gravity

Natasha2012 [34]3 years ago

4 0

The weight of an object is defined as the force of gravity on the object and may be calculated as the mass times the acceleration of gravity, w = mg. Since the weight is a force, its SI unit is the newton.

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At a certain temperature, the equilibrium constant, K c , for this reaction is 53.3. H 2 ( g ) + I 2 ( g ) − ⇀ ↽ − 2 HI ( g ) K

swat32

Answer:

$[HI]_{eq}=0.942M$

Explanation:

Hello,

In this case, the initial concentrations of hydrogen and iodine are the same:

$[H_2]_0=[I_2]_0=0.600M$

Thus, considering the given undergoing chemical reaction, one states the law of mass action in terms of the change $x$ due to the chemical change as shown below:

$Kc=\frac{(2x)^2}{(0.600M-x)(0.600M-x)}=53.3$

Therefore, solving for $x$ by quadratic equation one obtains:

$x_1=0.471M;x_2=0.826M$

Nevertheless, the feasible result is the first one as the second one results in negative concentrations, thus, the hydroiodic acid equilibrium concentration turns out:

$[HI]_{eq}=2*0.471M=0.942M$

Best regards.

8 0

3 years ago

Read 2 more answers

Calculate the Kc for the following reaction if an initial reaction mixture of 0.500 mole of CO and 1.500 mole of H2 in a 5.00 li

Lera25 [3.4K]

Answer:

4.41

Explanation:

Step 1: Write the balanced equation

CO(g) + 3 H₂(g) = CH₄(g) + H₂O(g)

Step 2: Calculate the respective concentrations

$[CO]_i = \frac{0.500mol}{5.00L} = 0.100M$

$[H_2]_i = \frac{1.500mol}{5.00L} = 0.300M$

$[H_2O]_{eq} = \frac{0.198mol}{5.00L} = 0.0396M$

Step 3: Make an ICE chart

CO(g) + 3 H₂(g) = CH₄(g) + H₂O(g)

I 0.100 0.300 0 0

C -x -3x +x +x

E 0.100-x 0.300-3x x x

Step 4: Find the value of x

Since the concentration at equilibrium of water is 0.0396 M, x = 0.0396

Step 5: Find the concentrations at equilibrium

[CO] = 0.100-x = 0.100-0.0396 = 0.060 M

[H₂] = 0.300-3x = 0.300-3(0.0396) = 0.181 M

[CH₄] = x = 0.0396 M

[H₂O] = x = 0.0396 M

Step 6: Calculate the equilibrium constant (Kc)

$Kc = \frac{[CH_4] \times [H_2O] }{[CO] \times [H_2]^{3} } = \frac{0.0396 \times 0.0396 }{0.060 \times 0.181^{3} } = 4.41$

3 0

4 years ago

Please help meee!!!!

Alchen [17]

The cork is less dense than the water

3 0

4 years ago

I have exams coming up for science.

Archy [21]

Answer:

flashcards, if its the periodic table write out the elements in order

just read the material over and over again

Explanation:

7 0

3 years ago

Read 2 more answers

• When a mechanism has been investigated in detail, it can be understood on many levels of differing detail. • An additional det

Nataly [62]

Complete Question

The complete question is shown on the first uploaded image

Answer:

The kinetic order in HI is x= 2

Explanation:

Generally the slow step in a reaction mechanism is the rate determining step

Now with this knowledge at the back of our minds we can see that the number of moles of HI i s 2 which implies that the order of HI is 2m

So we can represent the rate law as

$Rate = k [CH_3 CHCH_2][HI]^2$

hence

x = 2

7 0

4 years ago