How do I find the number of moles and molar mass of Gas A and Gas B with the information provided?

Sắp xếp các hợp chất: HF, HI, HBr, HCl theo chiều giảm dần tính axit.

mixer [17]

I don’t know what to answer

6 0

2 years ago

____ is converted to carbohydrate by plants during photosynthesis.

Ratling [72]

Carbon dioxide
Have a great day:)

5 0

4 years ago

Read 2 more answers

A mixture of gases is analyzed and found to have the following composition in mol %: CO2 12.0 CO 6.0 CH4 27.3 H2 9.9 N2 44.8 a)

vichka [17]

Answer:

a) CO₂: 21,9%; CO: 7,0%; CH₄: 18,2%; H₂: 0,8%; N₂: 52,1%

b) 24,09 g/mol

Explanation:

a) It is posible to obtain the composition of the gas mixture in weight% using molecular mass of each compound, thus:

12% CO₂× $\frac{44,01g}{1mol}$ = 528,1 g

6% CO× $\frac{28,01g}{1mol}$ = 168,1 g

27,3% CH₄× $\frac{16,05g}{1mol}$ = 438,2 g

9,9% H₂× $\frac{2,02g}{1mol}$ = 20,0 g

44,8% N₂× $\frac{28g}{1mol}$ = 1254,4 g

The total mass of the gas mixture is:

528,1g + 168,1g + 438,2g + 20,0g + 1254,4g = 2408,8 g

Thus composition of the gas mixture in weight% is:

CO₂: $\frac{528,1g}{2408,8g}$ ×100 = 21,9%

CO: $\frac{168,1g}{2408,8g}$ ×100 = 7,0%

CH₄: $\frac{438,2g}{2408,8g}$ ×100 = 18,2%

H₂: $\frac{20,0g}{2408,8g}$ ×100 = 0,8%

N₂: $\frac{1254,4g}{2408,8g}$ ×100 = 52,1%

b) The average molecular weight of the gas mixture is determined with mole % composition, thus:

0,12×44,01g/mol + 0,06×28,01g/mol + 0,273×16,05g/mol + 0,099×2,02g/mol + 0,448×28g/mol = 24,09 g/mol

I hope it helps!

6 0

3 years ago

How many bonds can a hydrogen atom form? O A. 3 O B. 1 O c. 4 O D. 2

Slav-nsk [51]

Answer:

the right answer is b !!!

8 0

2 years ago

Read 2 more answers

A researcher placed 25.0 g of silver chloride, AgCl, in sunlight and allowed the substance to decompose completely to form silve

steposvetlana [31]

Answer:

A. The law of definite proportions states that all pure samples of a particular chemical compound contain the same elements combines in the same proportion by mass.

B. The law of conservation of mass states that during ordinary chemical reactions, matter can neither be created or destroyed.

Note: The full question is as follows;

A researcher placed 25.0 g of silver chloride, AgCl, in sunlight and allowed the substance to decompose completely to form silver, Ag, with the release of chlorine gas, Cl2. The gas was collected in a container during the decomposition. The researcher determined that the mass of the silver formed was 18.8 g, and the mass of the chlorine gas formed was 6.2 g. The equation for the reaction is:

2AgCl ----> 2Ag + Cl2

a. State the law of definite proportions. Then use the researcher's data to confirm the law of definite proportions. Show your calculations.

b. State the law of conservation of matter. Then use the researcher's data to confirm the conservation of matter. Show your calculations.

Explanation:

A. Mass of silver obtained from AgCl = 18.8g.

Percentage mass of silver in the chloride = (18.8/25.0) * 100 = 75.2 %

Mass of chlorine obtained from AgCl = 6.2

Percentage mass of chlorine = (6.2/25) * 100 = 24.8 %

In one mole of AgCl with a molar mass of 143.3 g/mol; mass of silver = 107.8, mass of Cl = 35.5

Percentage mass of Ag = (107.8/143.3) * 100 = 75.2%

Percentage mass of Cl = (35.5/143.3) * 100 = 24.8%

Since the percentages by mass of Ag and AgCl obtained from the sample is the same to that obtained from a mole of AgCl, the law of definite proportions which states that all pure samples of a particular chemical compound contain the same elements combined in the same proportion by mass is verified.

B. Mass of reactant; AgCl sample = 25.0

Mass of products; At = 18.8 g; Cl = 6.2 g

Sum of products masses = 18.8 + 6.2 = 25.0 g

Therefore mass of reactant = mass of products.

This is in accordance with the law of conservation of mass which states that during ordinary chemical reactions, matter is neither created nor destroyed.

8 0

3 years ago