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cricket20 [7]
2 years ago
8

What does a scientific law do ?

Chemistry
1 answer:
baherus [9]2 years ago
3 0

Answer:

Scientific laws or laws of science are statements, based on repeated experiments or observations, that describe or predict a range of natural phenomena.

Explanation:

hope it's help

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For the equilibrium
sleet_krkn [62]

Answer:

\large \boxed{\text{0.091 atm }}

Explanation:

The balanced equation is

I₂(g) + Br₂(g) ⇌ 2IBr(g)

Data:

   Kc = 8.50 × 10⁻³

n(IBr) = 0.0600 mol

     V = 1.0 L

1. Calculate [IBr]

\text{[IBr]} = \dfrac{\text{0.0600 mol}}{\text{1.0 L}} = \text{0.0600 mol/L}

2. Set up an ICE table.

\begin{array}{ccccccc}\rm \text{I}_{2}& + & \text{Br}_{2} & \, \rightleftharpoons \, & \text{2IBr} &  &  \\0 & & 0 & &0.0600 & & \\+x &  & +x &   &- 2x & & \\x &   & x &   & 0.0600 - 2x & & \\\end{array}

3. Calculate [I₂]

\begin{array}{rcl}K_{\text{c}}&=&\dfrac{\text{[IBr]}^{2}} {\text{[I$_{2}$][Br]$_{2}$}}\\\\8.50 \times 10^{-2}&=&{\dfrac{(0.0600 - 2x)^{2}}{x^{2}}}& &\\\\0.2915x & = &{\dfrac{0.0600 - 2x}{x}}& &\\\\0.2915x & = &0.0600 - 2x\\\\2.2915x & = & 0.0600\\x & = & \textbf{0.026 18 mol/L}\\\end{array}\\

4. Convert the temperature to kelvins

T = (150 + 273.15) K = 423.15 K

5. Calculate p(I₂)

\begin{array}{rcl}\\pV & = & nRT\\p & = & cRT\\p & = & \text{0.026 18 mol} \cdot \text{L}^{-1}\times \text{0.082 06 L} \cdot \text{atm} \cdot \text{K}^{-1} \text{mol}^{-1} \times \text{423.15 K}\\& = & \textbf{0.91 atm}\\\end{array}\\\text{The partial pressure of iodine is $\large \boxed{\textbf{0.91 atm}}$}

6 0
2 years ago
In the chemical formula 3nh3, how many atoms of hydrogen (h) are there? 3 6 9 11
ANTONII [103]
Your answer is 3! Hope you get a good grade :)♥
7 0
3 years ago
Read 2 more answers
From the following balanced equation,
ArbitrLikvidat [17]

Answer:

9.72 grams.

Explanation:

From the equation, 4 moles of NH₃ produce 6 moles of  water.

Therefore the reaction to product ratio of  NH₃ to H₂O is 4:6

and 2:3 into its simplest form.

The number of moles of NH₃ in 6.12 g is:

Number of moles=mass/ RMM

=6.12 g/17 G/mol

=0.36 moles.

Therefore the number of moles of H₂O produced is calculated as follows.

(0.36 Moles×3)2 = 0.54 moles

Mass= Number of moles × RMM

=0.54 moles×18g/mol

=9.72 grams.

6 0
3 years ago
Is the electron configuration 1s22s22p5 for Oxygen correct?
joja [24]
No that’s is the electronic configuration for fluorine.
7 0
3 years ago
How many moles of co2 are produced when 5.70 mol of ethane are burned in an excess of oxygen
sweet-ann [11.9K]
I believe the answer is 6
4 0
3 years ago
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