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igor_vitrenko [27]
2 years ago
6

Nevermind i got it dont need help thanks

Chemistry
1 answer:
OverLord2011 [107]2 years ago
4 0

Answer:

Ok then...

Explanation:

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Mention 10 products made from crude oil​
garri49 [273]

Answer:

"After crude oil is removed from the ground, it is sent to a refinery where different parts of the crude oil are separated into useable petroleum products. These petroleum products include gasoline, distillates such as diesel fuel and heating oil, jet fuel, petrochemical feedstocks, waxes, lubricating oils, and asphalt.

A U.S 42-gallon barrel of crude oil yields about 45 gallons of petroleum products in U.S. refineries because of refinery processing gain. This increase in volume is similar to what happens to popcorn when it is popped."

"What are petroleum products, and what is petroleum used for?

Petroleum products include transportation fuels, fuel oils for heating and electricity generation, asphalt and road oil, and feedstocks for making the chemicals, plastics, and synthetic materials that are in nearly everything we use. Of the approximately 7.21 billion barrels of total U.S. petroleum consumption in 2016, 47% was motor gasoline (includes ethanol), 20% was distillate fuel (heating oil and diesel fuel), and 8% was jet fuel."

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4 0
2 years ago
A student performs an acid-base titration experiment to determine the amount of ascorbic acid in different brands of juice. Whic
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Answer:

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8 0
2 years ago
How many kilograms of oseltamivir would be needed to treat all the people in a city with a population of 400000 people if each p
madam [21]

Answer:

300 kg

Explanation:

The number of people in the city, p = 400,000

The number of capsules of oseltamivir each person consumes per day, n = 2 capsules

The number of days each person consumes the oseltamivir capsules, t = 5 days

The mass of oseltamivir in each capsule, m = 75 mg

The mass of oseltamivir needed to treat all the people in the city, <em>M</em>, is given as follows;

M = n·t·m·p

∴ M (in milligrams) = (2 × 5 × 75 × 400,000) mg = 300,000,000 mg

1,000,000 mg = 1 kg

∴ 300,000,000 mg = 300 kg

The mass of oseltamivir needed to treat all the people in the city, <em>M</em> = 300 kg

3 0
3 years ago
How many moles of O2 are required to react with 6.6 moles of H2?
Bingel [31]

<u>Answer: </u>

<u>For 1:</u> 3.3 moles of oxygen gas is required.

<u>For 2:</u> 14 moles of hydrogen gas is required.

<u>For 3:</u> 1.5 moles of oxygen gas is required.

<u>Explanation:</u>

The chemical reaction of oxygen and hydrogen to form water follows:

O_2+2H_2\rightarrow 2H_2O

  • <u>For 1:</u> When 6.6 moles of H_2 is reacted.

By Stoichiometry of the above reaction:

2 moles of hydrogen gas reacts with 1 mole of oxygen gas.

So, 6.6 moles of hydrogen gas will react with = \frac{1}{2}\times 6.6=3.3mol of oxygen gas.

Hence, 3.3 moles of oxygen gas is required.

  • <u>For 2:</u> When 7.0 moles of O_2 is reacted.

By Stoichiometry of the above reaction:

1 mole of oxygen gas reacts with 2 moles of hydrogen gas.

So, 7 moles of oxygen gas will react with = \frac{2}{1}\times 7=14mol of hydrogen gas.

Hence, 14 moles of hydrogen gas is required.

  • <u>For 3:</u> When 3.0 moles of H_2O is formed.

By Stoichiometry of the above reaction:

2 moles of water is formed from 1 mole of oxygen gas.

So, 3.0 moles of water will be formed from = \frac{1}{2}\times 3.0=1.5mol of oxygen gas.

Hence, 1.5 moles of oxygen gas is required.

7 0
2 years ago
If 150 g dimethylhydrazine reacts with excess dinitrogen tetroxide and the product gases are collected at 127oC in an evacuated
zhuklara [117]

Answer : The the partial pressure of the nitrogen gas is 0.981 atm.

The total pressure in the tank is 2.94 atm.

Explanation :

The balanced chemical reaction will be:

(CH_3)_2N_2H_2(l)+2N_4O_4(l)\rightarrow 3N_2(g)+4H_2O(g)+2CO_2(g)

First we have to calculate the moles of dimethylhydrazine.

Mass of dimethylhydrazine = 150 g

Molar mass of dimethylhydrazine =60.104 g/mole

\text{Moles of dimethylhydrazine}=\frac{\text{Mass of dimethylhydrazine}}{\text{Molar mass of dimethylhydrazine}}

\text{Moles of dimethylhydrazine}=\frac{150g}{60.104g/mole}=2.49mole

Now we have to calculate the moles of N_2 gas.

From the balanced chemical reaction we conclude that,

As, 1 mole of (CH_3)_2N_2H_2 react to give 3 moles of N_2 gas

So, 2.49 mole of (CH_3)_2N_2H_2 react to give 2.49\times 3=7.47 moles of N_2 gas

Now we have to calculate the partial pressure of nitrogen gas.

Using ideal gas equation :

PV=nRT\\\\P_{N_2}=\frac{nRT}{V}

where,

P = Pressure of N_2 gas = ?

V = Volume of N_2 gas = 250 L

n = number of moles  N_2 gas = 7.47 mole

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of N_2 gas = 127^oC=273+127=400K

Putting values in above equation, we get:

P_{N_2}=\frac{(7.47mole)\times (0.0821L.atm/mol.K)\times 400K}{250L}=0.981atm

Thus, the partial pressure of the nitrogen gas is 0.981 atm.

Now we have to calculate the total pressure in the tank.

Formula used :

P_{N_2}=X_{N_2}\times P_T

P_T=\frac{1}{X_{N_2}}\times P_{N_2}

P_T=\frac{1}{(\frac{n_{N_2}}{n_T})}\times P_{N_2}

P_T=\frac{n_{T}}{n_{N_2}}\times P_{N_2}

where,

P_T = total pressure = ?

P_{N_2} = partial pressure of nitrogen gas = 0.981 atm

n_{N_2} = moles of nitrogen gas = 3 mole  (from the reaction)

n_{T} = total moles of gas = (3+4+2) = 9 mole  (from the reaction)

Now put all the given values in the above formula, we get:

P_T=\frac{9mole}{3mole}\times 0.981atm=2.94atm

Thus, the total pressure in the tank is 2.94 atm.

8 0
2 years ago
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