1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
lara [203]
3 years ago
15

A sample of oxygen is collected over water at a total pressure of 692.2 mmHg at 17°C. The vapor pressure of water at 17°C is 14.

5 mmHg. The partial pressure of the O2
Chemistry
1 answer:
frutty [35]3 years ago
5 0

Answer:

677.7 mmHg

Explanation:

The first empirical study on the behaviour of a mixture of gases was carried out by John Dalton. He established the effects of mixing gases at different pressures in the same vessel.

Dalton's law states that,the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the individual gases present in the mixture of gases. When a gas is collected over water, the gas also contains some water vapour. The partial pressure of the gas will now be given as; total pressure of gas mixture - saturated vapour pressure of water (SVP) at that temperature.

Given that;

Total pressure of gas mixture = 692.2 mmHg

SVP of water at 17°C = 14.5 mmHg

Therefore, partial pressure of oxygen = 692.2-14.5

Partial pressure of oxygen = 677.7 mmHg

You might be interested in
Cuales son las fórmulas de la velocidad
AnnZ [28]

Answer:

s = d÷ t

Explanation:

Where s means speed, d means distance and t means time

7 0
3 years ago
The theoretical yield of NaBr from
Dvinal [7]

the percent yield of the reaction is 100%.

The percent yield is calculated as the experimental yield divided by the theoretical yield x 100%:

% yield = actual yield / theoretical yield * 100%

% yield of a reaction in this case Rate

In this case, the molar mass of NaBr is 102.9 g / mol, as you know:

444 actual yield = 7.08 mol x 102.9 g / mol = 728.532 g

theoretical yield = 7.08 mol x 102.9 g / mol = 728.532 g

, Replaced by the definition of percent yield:

percent yield = 728.532 grams / 728.532 grams * 100%

percent yield = 100%

Finally, the percent yield of the reaction is 100%.

<h3 />

FeBr3 is iron bromide. Also known as iron bromide. Iron bromide is an ionic compound in which iron is in a +3 oxidation state.

Learn more about % yield here:brainly.com/question/27979178

#SPJ10

5 0
2 years ago
The development of a nuclear power plant at an ocean site is expected to produce an enormous amount of electric power for a larg
Oksanka [162]

Answer:

B. The effects of warmed water on aquatic life

Explanation:

quizizz

8 0
3 years ago
Read 2 more answers
Hydrogen cyanide, HCN, can be made by a two-step process. First, ammonia reacts with O2 to give nitric oxide, NO.
stealth61 [152]

Answer:

The mass of HCN is 79.65 g.

The mass of reactant which remain at the end of both reactions is 88.5 g.

Explanation:

Given that,

Mass of ammonia = 50.2 g

Mass of methane = 48.4 g

Hydrogen cyanide, HCN, can be made by a two-step process

Ammonia reacts with O₂ to give nitric oxide NO.

The reaction is,

4NH_{3}+5O_{2}\Rightarrow 4NO+6H_{2}O

We need to calculate the mole of NO

Using given data,

2.25 g NH_{3}=\dfrac{50.2}{17}= 2.95\ mole\ NH_{3} [/tex]

4\ mole NH_{3}\ glose 4\ mol NO

2.95 mol NH₃ will produced 2.95 mol NO

Then nitric oxide reacts with methane,

The reaction is,

2NO+2CH_{4}\Rightarrow 2HCN+2H_{2}O+H_{2}

We need to calculate the mole of methane

Using given data,

mole\ of\ methane=\dfrac{48.4}{16}

mole\ of\ methane = 3.03\ moles

2 mole NO produced 2 mole HCN

2.95 mol NO will produced \dfrac{2.95\times3.03}{3.03}= 2.95 mol HCN

We need to calculate the mass of HCN

Using formula of mass

m=N\times M

Where, N = number of mole

M = molecular mass

Put the value into the formula

m=2.95\times27

m= 79.65\ g

The mass of HCN is 79.65 g.

We need to calculate the mass of NO

Using formula of mass

m=N\times M

Where, N = number of mole

M = molecular mass

Put the value into the formula

m=2.95\times30

m= 88.5\ g

Hence, The mass of HCN is 79.65 g.

The mass of reactant which remain at the end of both reactions is 88.5 g.

4 0
3 years ago
KClO3 (s) KCl (s) + 02 (g)​<br><br><br>How do you balance this equation
Vitek1552 [10]

Answer:

2KCl(s) + 6O3O2

Explanation:

I think it's correct

7 0
3 years ago
Other questions:
  • How many grams nh3 are equivalent to 9.3 x 1023 molecules nh3?
    12·1 answer
  • What is a isotope ?
    15·2 answers
  • One lap of an engineered hamster track measures 255 cm. To run 10. meters, how many laps should the hamster run? Report your ans
    10·1 answer
  • You spot a friend walking on a moving walkway in an airport. You are not on the walkway and you want to keep up with her.
    13·1 answer
  • Match each organ or function with its body system.
    10·2 answers
  • Dumbledore decides to gives a surprise demonstration. He starts with a hydrate of Na2CO3 which has a mass of 4.31 g before heati
    12·1 answer
  • Classify the following as an element, compound, homogeneous mixture, or heterogeneous mixture:
    5·1 answer
  • Covalent compounds are formed when
    8·1 answer
  • Which supports the idea that birds and butterflies both have wings but they do not have a common ancestor with wings?
    14·2 answers
  • Why are scientists worried that climate change will cause these toxic algae blooms to become more frequent?
    8·2 answers
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!