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3 years ago

Ned help with this question

Chemistry

1 answer:

tia_tia [17]3 years ago

8 0

Answer:

135.6

Explanation:

12 * 11.3 = 135.6

To find the mass you have to multiply the density and volume together

If you already have the mass you divide the mass by either the density or volume

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the solubility of nitrogen gas is 1.90 mL/dL of blood at 1.00 atm. what is the solubility of nitrogen gas in a deepsea divers bl

leonid [27]

The solubility of nitrogen gas in water is 1.90 mL/dL at 1.00 atm and 13.3 mL/dL at 7.00 atm.

We want to relate the solubility of a gas with its partial pressure.

We can do so using Henry's law.

<h3>What does Henry's law state?</h3>

Henry's law states that the amount of dissolved gas in a liquid is proportional to its partial pressure above the liquid.

C = k × P

where,

C is the concentration of a dissolved gas.

k is the Henry's Law constant.

P partial pressure of the gas.

The solubility of nitrogen gas is 1.90 mL/dL of blood at 1.00 atm.

Since the solvent is basically water, we can understand that the concentration of nitrogen gas is 1.90 mL/dL at 1.00 atm.

We can use this information to calculate Henry's Law constant.

k = C/P = (1.90 mL/dL)/1.00 atm = 1.90 mL/dL.atm

We want to calculate the solubility of nitrogen gas at a pressure of 7.00 atm.

We will use Henry's law.

C = k × P = (1.90 mL/dL.atm) × 7.00 atm = 13.3 mL/dL

The solubility of nitrogen gas in water is 1.90 mL/dL at 1.00 atm and 13.3 mL/dL at 7.00 atm.

Learn more about solubility here: brainly.com/question/11963573

6 0

3 years ago

Key terms: Reset ____________ anions are strong nucleophiles that open epoxide rings by an SN2 mechanism. ____________ tautomers

iogann1982 [59]

Answer:

Acetylide , Enol ,aldehydes, tautomers, alkynes , Hydroboration, Keto

Explanation:

Reset Acetylide anions are strong nucleophiles that open epoxide rings by an SN2 mechanism. Enol tautomers have an O-H group bonded to a C=C. aldehydes are formed from terminal alkynes with the addition of water using BH3 then H2O2. tautomers are constitutional isomers that differ in the location of a double bond and a hydrogen and exist in an equilibrium with each other. alkynes are compounds that contain a carbon-carbon triple bond. Hydroboration of a terminal alkyne adds BH₂ to the less substituted, terminal carbon. Keto tautomers have a C=O and an additional C-H bond.

3 0

3 years ago

This lab question is: How can you distinguish a physical change from a chemical change?

geniusboy [140]

Answer:b,and c

Explanation:

4 0

3 years ago

A gas exerts a pressure of 0.62 atm. Convert this to kPa and mmHg. Be sure to show your work.

IRINA_888 [86]

Answer:

The answer to your question is 0.62 atm = 62.82 kPa = 471.2 mmHg

Explanation:

Data

P = 0.62 atm

P = ? kPa

P = ? mmHg

Process

1.- Look for the conversion factor of atm to kPa and mmHg

1 atm = 101.325 kPa

1 atm = 760 mmHg

2.- Do the conversions

1 atm ----------------- 101.325 kPa

0.62 atm ------------ x

x = (0,62 x 101.325) / 1

x = 62.82 kPa

1 atm ------------------ 760 mmHg

0.62 atm ------------ x

x = (0.62 x 760)/1

x = 471.2 mmHg

4 0

3 years ago

112 g of aluminum carbide react with 174 g water to produce methane and aluminum hydroxide in the reaction shown below.

dolphi86 [110]

Answer: 4.999 moles of excess reactant will be left over.

Explanation:

Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.

Excess reagent is defined as the reagent which is left behind after the completion of the reaction.

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

Given mass of aluminium carbide = 112 g

Molar mass of aluminium carbide = 143.96 g/mol

Putting values in equation 1:

$\text{Moles of aluminium carbide}=\frac{112g}{143.96g/mol}=0.778mol$

For the given chemical reaction:

$2Al_4C_3(s)+12H_2O(l)\rightarrow 3CH_4(g)+4Al(OH)_3(s)$

By the stoichiometry of the reaction:

2 moles of aluminium carbide reacts with 12 moles of water

So, 0.778 moles of aluminium carbide will react with = $\frac{12}{2}\times 0.778=4.668 mol$ of water

Given mass of water = 174 g

Molar mass of water = 18 g/mol

Putting values in equation 1:

$\text{Moles of water}=\frac{174g}{18g/mol}=9.667mol$

Moles of excess reactant (water) left = 9.667 - 4.668 = 4.999 moles

Hence, 4.999 moles of excess reactant will be left over.

8 0

3 years ago

Ned help with this question​

Ned help with this question