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Luba_88 [7]
3 years ago
14

Drag the correct label to the pictures. Each label can be used more than once. Classify the materials based on their composition

.

Chemistry
1 answer:
marta [7]3 years ago
7 0

Answer:

I know, it's hard!!

Explanation:

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If have a volume of 18 L of a gas at a temperature of 272 K and a pressure of 90 atm, what will be the pressure of the gas if ra
Solnce55 [7]

Answer:

P₂ ≅ 100 atm (1 sig. fig. based on the given value of P₁ = 90 atm)

Explanation:

Given:

P₁ = 90 atm                    P₂ = ?

V₁ = 18 Liters(L)              L₂ = 12 Liters(L)      

=> decrease volume => increase pressure

=> volume ratio that will increase 90 atm is (18L/12L)                                                                  

T₁ = 272 Kelvin(K)          T₂ = 274 Kelvin(K)

=>  increase temperature => increase pressure

=> temperature ratio that will increase 90 atm is (274K/272K)

n₁ = moles = constant    n₂ = n₁ = constant

P₂ = 90 atm x (18L/12L) x (274K/272K) = 135.9926471 atm (calculator)

By rule of sig. figs., the final answer should be rounded to an accuracy equal to the 'measured' data value having the least number of sig. figs. This means P₂ ≅ 100 atm based on the given value of P₁ = 90 atm.

3 0
2 years ago
Calculate the number of grams of CO that can react with 0.400 kg of Fe2O3.
aleksandr82 [10.1K]

Answer:

mass of CO = 210.42 g

mass in three significant figures = 210. g

Explanation:

Given data:

mass of Fe2O3 = 0.400 Kg

mass of CO= ?

Solution:

chemical equation:

Fe2O3 + 3CO → 2Fe + 3CO2

Now we will calculate the molar mass of  Fe2O3 and CO.

Molar mass of  Fe2O3 = (55.845 × 2) + (16 × 3) = 159.69 g/mol

Molar mass of CO = 12+ 16 = 28 g/mol

now we will convert the kg of Fe2O3 in g.

mass of Fe2O3 = 0.400 kg × 1000 = 400 g

number of moles of Fe2O3  = 400 g/ 159.69 g/mol = 2.505 mol

mass of CO = moles of Fe2O3 × 3( molar mass of CO)

mass of CO = 2.505 mol × 84 g/mol

mass of CO = 210.42 g

mass in three significant figures = 210. g

5 0
3 years ago
Read 2 more answers
An astronaut in her spacesuit weighs 300 lb on earth. What would her weight be on the moon?
Phantasy [73]
She would be 150 on the moon because the moon has half the mass of earth
6 0
2 years ago
Read 2 more answers
Draw the structure of the bromohydrin formed when (Z)-3-hexene reacts with Br2/H2O. Use the wedge/hash bond tools to indicate st
Ipatiy [6.2K]

Answer:

(3R,4R)-4-bromohexan-3-ol

Explanation:

In this case, we have  reaction called <u>halohydrin formation</u>. This is a <u>markovnikov reaction</u> with <u>anti configuration</u>. Therefore the halogen in this case "Br" and the "OH" must have <u>different configurations</u>. Additionally, in this molecule both carbons have the <u>same substitution</u>, so the "OH" can go in any carbon.

Finally, in the product we will have <u>chiral carbons</u>, so we have to find the absolute configuration for each carbon. On carbon 3 we will have an "R" configuration on carbon 4 we will have also an "R" configuration. (See figure 1)

I hope it helps!

5 0
3 years ago
What is the pressure in millimeters of mercury of 0.0130 molmol of helium gas with a volume of 210. mLmL at 55 ∘C∘C? (Hint: You
juin [17]

Answer : The pressure of the helium gas is, 1269.2 mmHg

Explanation :

To calculate the pressure of the gas we are using ideal gas equation:

PV=nRT

where,

P = Pressure of He gas = ?

V = Volume of He gas = 210. mL = 0.210 L    (1 L = 1000 mL)

n = number of moles He = 0.0130 mole

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

T = Temperature of He gas = 55^oC=273+55=328K

Putting values in above equation, we get:

P\times 0.210L=0.0130mole\times (0.0821L.atm/mol.K)\times 328K

P=1.67atm=1269.2mmHg

Conversion used : (1 atm = 760 mmHg)

Thus, the pressure of the helium gas is, 1269.2 mmHg

4 0
3 years ago
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