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Alexandra [31]
3 years ago
15

In the rate law, k is a universal constant. True or False? ( I have more questions on profile)

Chemistry
1 answer:
OverLord2011 [107]3 years ago
7 0
False information.....
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2 years ago
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kifflom [539]

Answer:

See explanation

Explanation:

A net ionic equation shows only the chemical species that are involved in a reaction, while a complete ionic equation also includes the spectator ions(Khan Academy).

From the species shown in the image we can write the molecular equation, ionic equation and net ionic equation and also identify the spectator ions.

Chemical equation: KX + BY --------> BX + AY

Ionic Equation; X^- + A^+ + B^+ + Y^- -----> BX + A^+ + Y^-

Spectator ions;  A^+ and Y^-

Net Ionic Equation; X^- + B^+ ------> BX

7 0
2 years ago
Which type of bond is MOST LIKELY formed in nitrous oxide?
arsen [322]
The type of bond most likely formed in nitrous oxide would be a covalent bond..
8 0
3 years ago
Read 2 more answers
4. Nitrogen and oxygen gases react to form dinitrogen monoxide gas (N2O). What volume of O, is
solmaris [256]

Answer:

no be t ha t s had ice

Explanation:

uah an

8 0
3 years ago
A sample compound with a molar mass of 34.00g/mol is found to consist of 0.44g H and 6.92g O. Calculate both empirical and molec
balu736 [363]

Answer:

E.F= OH

M.F=O_{2} H_{2}

Explanation:

Empirical Formula

Step 1: Calculate mols of each element

0.44gH(1 mol H/ 1.008g H)= 0.4365 mol H

*note leave extra sig figs for calculations

6.92gO(1 mol O/ 16 g O)=0.4325 mol O

Step 2: Identify which is the smallest mol

*in this case 0.4365 mol H> 0.4325 mol O so we will use 0.4325 mol O

Step 3: Divide above calculations by the smallest mol

0.4325 mol O/0.4325= 1

0.4365 mol H/0.4325= 1.009 *rounds to 1

Step 4: use calculations as subscripts

Oxygen = 1 so the subscript will 1 (O)

Hydrogen = 1 so the subscript will 1 (H)

making E.F= OH

Molecular Formula:

Step 1: identify  molecular mass and mass from the E.F

the molecular mass is given 34.00g/mol

the mass of the E.F is

(oxygen mass from periodic table)+(hydrogen mass from periodic table)

16+1.008= 17.008

Step 2:Divide the molecular mass by the mass given by the emipirical formula.

\frac{34.00}{17.008}= 1.999 round to 2

Step 3:Multiply the empirical formula (the subscripts) by this number to get the molecular formula.  ANSWER: M.F=2(OH)- O_{2} H_{2}

3 0
3 years ago
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