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3 years ago

The rate law of a reaction is rate = k[D][X]. The units of the rate constant are ________.

Chemistry

1 answer:

bogdanovich [222]3 years ago

8 0

Answer:

Explanation:

Hello!

Since the rate must have the following units: mol/(L*s), the suitable units for k, considering that the term [D] [X] leads to mol^2/(L^2) (it means a second order kinetic law), are L/(mol*s), nevertheless, that answer isn't in the given options.

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The half-life of cobalt-60 is 5.3 years. after __________ years, 1/4 of the original amount of cobalt-60 will remain.

cestrela7 [59]

The number of years required for 1/4 cobalt-60 to remain after decay is calculated as follows

after one half life 1/2 of the original mass isotope remains

after another half life 1/4 mass of original mass remains

therefore if one half life is 5.3 years then the years required

= 2 x 5.3years = 10.6 years

4 0

3 years ago

Read 2 more answers

Use the following equation to answer the questions and please show all work.

DIA [1.3K]

Answer:

a.36 g of water is produced.

b.64 g of $O_{2}$ is consumed.

Explanation:

The reaction is $2H_{2} + O_{2}$ ⇒ $2H_{2}O$

Given,

Weight of $H_{2}$ reacted = 4g

Weight of 1 mole of $H_{2}$ = 2 $\times$ 1 = 2g

Therefore no. of moles of $H_{2}$ reacted = $\frac{4}{2}$ = 2 moles;

Also given,

Weight of $O_{2}$ reacted = 32 g

Weight of 1 mole of $O_{2}$ = 2 $\times$ 16 = 32 g

Therefore no. of moles of $O_{2}$ reacted = $\frac{32}{32}$ = 1

We know that 2 moles of Hydrogen reacts with 1 mole of Oxygen to give 2 moles of water,

As we took 2 moles of Hydrogen and 1 mole of Oxygen,

Directly,from the equation we can tell 2moles of water will be produced.

Therefore no. of moles of $H_{2} O$ produced = 2

Weight of 1 mole of water = $2\times 1+16$ = 18

Therefore weight of $H_{2}O$ produced = $2\times 18$ = 36gm

Given ,

72 g of $H_{2}O$ is produced.

So,

no. of moles of $H_{2}O$ produced = $\frac{72}{18}$ = 4 moles

From equation For every 2 moles of water formed , 1 mole of oxygen must be required.

So for producing 4 moles of water,

No. of moles of Oxygen required = 2 moles.

Therefore weight of $O_{2}$ reacted = $2\times32$ = 64 g

Method 2:

Given,

8 g of $H_{2}$ has reacted.

So,

no. of moles of $H_{2}$ reacted = $\frac{8}{2}$ = 4 moles.

From equation , we know that For every 2 moles of $H_{2}$ reacted,1 mole of $O_{2}$ will react.

Therefore,

No. of moles of $O_{2}$ that reacts with 4 moles of $H_{2}$ = $2\times1$ = 2 moles

Therefore the weight of $O_{2}$ reacted = $2\times 32$ = 64 g

6 0

3 years ago

Concentration of Cl ion of 72.24g NaCl in .862 L solution

Nady [450]

Answer:

$Molarity_{Cl^-}=1.434\ M$

Explanation:

Moles of NaCl :

Given, Mass of NaCl = 72.24 g

Molar mass of NaCl = 58.44 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{72.24\ g}{58.44\ g/mol}$

$Moles\ of\ NaCl= 1.2361\ mol$

NaCl is a strong salt. So, moles of chloride ion = 1.2361 moles

Volume = 0.862 L

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

$Molarity_{Cl^-}=\frac{1.2361}{0.862}$

$Molarity_{Cl^-}=1.434\ M$

7 0

3 years ago

Which of the following is an oxidation-reduction reaction? Which of the following is an oxidation-reduction reaction? Ba(C2H3O2)

DochEvi [55]

Answer:

The only oxidation- reduction reaction is Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2

Explanation:

An oxidation-reduction reaction is a chemical reaction that involves an electron transfer between two species. This will lead to a change in oxidation number of a molecule, atom, or ion changes by gaining or losing an electron.

Some atoms have different possible oxidation numbers.

H has oxidation number +1

O has oxidation number -2

The oxidation number of an individual atom is 0.

The total oxidation number of all atoms in: a neutral species is 0 and in an ion is equal to the ion charge.

⇒ Ba(C2H3O2)2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaC2H3O2

(C2H3O2)2 has an oxidation number of -2. So Ba has an oxidation number of +2

In BaSO4 has SO4 an oxidation number of -2 and Ba has an oxidation number of +2

This means Ba doesn't change its oxidation number.

In Na2SO4 Na has an oxidation of +1; in NaC2H3O2 Na has an oxidation of +1

This means Na doesn't change its oxidation number.

⇒ Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2

Cu has an oxidation number of 0

In Cu(NO3)2, NO3 has an oxidation number of -1 so Cu has an oxidation number of +2

In 2AgNO3, NO3 has an oxidation number of -1 so Ag has an oxidation number of +1

Ag has an oxidation number of 0

⇒ HCl (aq) + NaOH (aq) → H2O (l) + NaCl

The oxidation number of Cl and Na do not change

⇒ AgNO3 (aq) + HCl (aq) → AgCl (s) + HNO3

In AgNO3 Ag has an oxidation number of +1

In AgCl Ag has an oxidation number of +1

In HCl Cl has an oxidation number of -1

In AgCl Cl has an oxidation number of +1

The oxidation number of Cl and Ag do not change

⇒ H2CO3 (aq) + Ca(NO3)2 (aq) → 2HNO3 (aq) + CaCO3 (s)

In Ca(NO3)2 Ca has an oxidation number of +2

In CaCO3 Ca has an oxidation number of +2

In Ca(NO3)2 N has an oxidation number of +5

In HNO3 N has an oxidation number of +5

In H2CO3 C has an oxidation number of +4

In CaCO3 C has an oxidation number of +4

The only oxidation- reduction reaction is Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2

Oxidizing agent: Ag ; Reducing agent: Cu

4 0

3 years ago

Choose the true statement.

Svetradugi [14.3K]

Answer:

1. The solubility of a gas in water increases with an increase in pressure

Explanation:

6 0

2 years ago