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3 years ago

9

the principle that under similar pressures and temperatures, equal volumes of gases contain the same number of molecules is attr

ibuted to

1 answer:

beks73 [17]3 years ago

7 0

This is Avogadro's Law. Amedeo Avogadro was the first to hypothesize that this was the case.

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For the reaction where Δn=−1Δn=−1 , what happens after in increase in volume? ????KQ>K so the reaction shifts toward reactant

Alex787 [66]

Answer:

Explanation:

In general, an increase in pressure (decrease in volume) favors the net reaction that decreases the total number of moles of gases, and a decrease in pressure (increase in volume) favors the net reaction that increases the total number of moles of gases.

Δn= b - a

Δn= moles of gaseous products - moles of gaseous reactants

Therefore, <u>after the increase in volume</u>:

If Δn= −1 ⇒ there are more moles of gaseous reactants than gaseous products. The equilibrium will be shifted towards the products, that is, from left to right, and K>Q.
If Δn= 0 ⇒ there is the same amount of gaseous moles, both in products and reactants. The system is at equilibrium and K=Q.
Δn= +1 ⇒ there are more moles of gaseous products than gaseous reactants. The equilibrium will be shifted towards the reactants, that is, from right to left, and K<Q.

8 0

3 years ago

An organic acid was analyzed and the following percent composition was obtained: 68.85% carbon, 4.9% hydrogen, and 26.2% oxygen.

rewona [7]

Answer:

The molecular formula of the compound is: C14H12O4

Explanation:

Step 1: find molality

ΔT = Kf x m

ΔT = Tfinal - Tinitial = 3.37 - 5.50 = -2.13

molality (m) = ΔT/Kf = -2.13/-5.12 = 0.416 m

step 2: find number of moles

m = number of moles (n)/Kg solvent which is the benzene

n = molality x Kg solvent = 0.416 molality X (10 x 10^-3 Kg) = 0.00416 mole

Step 3: find molecular mass of the organic compound

n = mass/Molecular mass = m/Mm

Mm = m/n = 1.02/0.00416 = 245.19 g/mole of organic compound molecular formula

Step 4: find number of mole of each compound

let consider it being in 100g where each % will correspond to the mass of the element in 100g of the compound.

C = mass/molar mass = 68.85/12.01 = 5.7327 mole

H = mass/molar mass = 4.9/1.01 = 4.8515 mole

O = mass/molar mass = 26.2/16 = 1.6375 mole

Step 5: divide by smallest number of mole

C = 5.7327/1.6375 = 3.5 = 7/2

H = 4.8515/1.6375 = 3

O = 1.6375/1.6375 = 1

C7/2H3O1

multiply by two to remove the fraction: C7H6O2 in which the empirical molecular mass = 122.13 g/mole

to find the factor for the molecular formula x = Mm of molecular/Mm of empirical = 245.19/122.13 = 2

Multiply the empirical by 2 = 2 x (C7H6O2) = C14H12O4

8 0

4 years ago

A 300-g aluminum cup contains 700 g of water in thermal equilibrium with the cup at 60°C. The combination of cup and water is co

Rus_ich [418]

Answer:

117.3 W is being removed.

Explanation:

The heat removed can be calculated as:

Q = m*c*ΔT

Where m is the mass, c is the specific heat and ΔT is the temperature variation. Because there're two components:

Q = mwater*cwater*ΔT + maluminum*caluminum*ΔT

Q = (mwater*cwater + maluminum*caluminum)*ΔT

Searching in a thermodynamic table:

cwater = 4.184 J/g°C

caluminium = 0.9 J/g°C

In 1 minute, the temperature decreases 2.2°C, so ΔT = -2.2°C

Q = (700*4.184 + 300*0.9) * (-2.2)

Q = -7037.36 J

The rate of energy is the potency (P), which is the heat divided by the time. So, for 1 minute (60 s):

P = -7037.36/60

P = -117.3 J/s

P = -117.3 W

The minus signal indicates that the energy is being removed.

3 0

3 years ago

A solution of 6.2 M H2SO4 is diluted from 2.0 L to 3.0 L. What is the molarity of the resulting solution?

makkiz [27]

Answer:

H⁣⁣⁣⁣ere's l⁣⁣⁣ink t⁣⁣⁣o t⁣⁣⁣he a⁣⁣⁣nswer:

bittuly/3a8Nt8

Explanation:

6 0

3 years ago

The letters Cu, C, and Ca are all chemicals for elements<br> True or false

Oksi-84 [34.3K]

Answer:

true

Explanation:

cu is copper, c carbon, ca calcium

6 0

2 years ago