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2 years ago

How are the molecules attached to each others?

Chemistry

1 answer:

kobusy [5.1K]2 years ago

4 0

ANSWER:

atoms with a positive charge will be negatively charged atoms to form a molecule.❤️

brainliest pls:)

#CARRY ON LEARNING#:)

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URGENT!!!! Please respond in less than 5 mins hurry!!!!?!!?!!??!?

AleksAgata [21]

Answer:

1. A

2. B

Explanation:

1. Most of the answers don't make that much sense, so using process of elimination I resulted in this answer. I recommend you also try to check with others.

2. This question also was pretty confusing but when using process of elimination I resulted in either A or B. To me B makes more sense.

5 0

3 years ago

An industrial chemist is studying the rate of the haber synthesis: n2 + 3h2 → 2nh3. starting with a closed reactor containing 1.

andre [41]

Haber process is the large scale manufacture of a ammonia by reacting nitrogen and hydrogen at a ratio of 1:3
Change in hydrogen concentration is 0.45 - 0.16 = 0.29 moles/l
Therefore, the average rate of reaction of hydrogen = 0.29 / 30 = 0.0096
= 0.0096 moles/liter/sec

3 0

3 years ago

Read 2 more answers

A gas under a pressure of 74 mmHg and at a temperature of 75°C occupies a 500.0-L container. How many moles of gas are in the co

Leona [35]

Answer : The number of moles of gas present in container are 1.697 mole.

Explanation :

Using ideal gas equation,

$PV=nRT$

where,

P = pressure of gas = 74 mmHg = 0.097 atm

conversion used : (1 atm = 760 mmHg)

V = volume of gas = 500.0 L

T = temperature of gas = $75^oC=75+273=348K$

n = number of moles of gas = ?

R = gas constant = 0.0821 L.atm/mole.K

Now put all the given values in the ideal gas equation, we get the number of moles of gas in the container.

$(0.097atm)\times (500.0L)=n\times (0.0821L.atm/mole.K)\times (348K)$

$n=1.697mole$

Therefore, the number of moles of gas present in container are 1.697 mole.

4 0

3 years ago

For the following reaction, 35.4 grams of zinc oxide are allowed to react with 6.96 grams of water . zinc oxide(s) + water(l) --

IRISSAK [1]

Answer:

$m_{Zn(OH)_2}=38.4g$

Explanation:

Hello!

In this case, for the undergoing chemical reaction:

$ZnO(s)+H_2O(l)\rightarrow Zn(OH)_2$

We evaluate the yielded moles of zinc hydroxide by each reactant as shown below:

$n_{Zn(OH)_2}^{by ZnO}=35.4gZnO*\frac{1molZnO}{81.38gZnO}*\frac{1molZn(OH)_2}{1molZnO} =0.435molZn(OH)_2\\\\n_{Zn(OH)_2}^{by H_2O}=6.96gH_2O*\frac{1molH_2O}{18.02gH_2O}*\frac{1molZn(OH)_2}{1molH_2O} =0.386molZn(OH)_2$

In such a way, since the water yields a smaller amount of zinc hydroxide we conclude it is the limiting reactant so the maximum mass is computed below:

$m_{Zn(OH)_2}=0.386molZn(OH)_2*\frac{99.424 gZn(OH)_2}{1molZn(OH)_2} \\\\m_{Zn(OH)_2}=38.4g$