All categories

3 years ago

Please help me l don’t understand please !!!!!!

Chemistry

1 answer:

garik1379 [7]3 years ago

7 0

Answer: C

Explanation:

he never had evidence in the first place that was nearly enough.

You might be interested in

When chlorine is added to acetylene, 1, 1, 2, 2-tetrachloroethane is formed: 2cl2 (g) + c2h2 (g) → c2h4cl4 (l) how many liters o

Otrada [13]

Answer:
20 L of Cl₂

Solution:

The reaction is as follow,

H₂C₂ + 2 Cl₂ → H₂C₂Cl₄

According to equation,

167.84 g (1 mole) H₂C₂Cl₄ is produced by = 44.8 L (2 mole) of Cl₂
So,
75 g of H₂C₂Cl₄ will be produced by = X L of Cl₂

Solving for X,
X = (44.8 L × 75 g) ÷ 167.84 g

X = 20 L of Cl₂

7 0

4 years ago

The equation X + Y 2Z has the rate law equation shown below. Which of the following statements best describes the relationship o

andreyandreev [35.5K]

The order of the reaction with respect to X is 2.
The statements given ;
1. As Concentration of X is in the rate law equation , changing X will have an effect on the rate of the equation.
2. Rate is proportional to X^2
So if concentration of X is doubled, then rate proportional to (2X)^2 = 4X^2
Rate therefore quadruples when X is doubled
This statement is correct
3. If we divide X/2 then the effect to the rate is (X/2)^2 = X/4 . This will reduce the rate by quarter not half . This statement is wrong.
4. If we multiply by 3
Then rate proportional to (3X)^2 = 9X^2
Rate increases by 9 times. This statement is wrong

4 0

3 years ago

Which of the organisms in this food web gets energy from both producers and consumers?

4vir4ik [10]

Sand shrimp or Algae

8 0

3 years ago

A 23.0-mL volume of O2, collected over water at 752 torr and 22Â°C, is produced from the thermal decomposition of KClO3. The vap

arsen [322]

Answer:

$9.14\times 10^{-4}$ moles

Explanation:

We are given:

Vapor pressure of water = 19.8 torr

Total vapor pressure = 752 torr

Vapor pressure of oxygen gas = Total vapor pressure - Vapor pressure of water = (752 - 19.8) torr = 732.2 torr

To calculate the amount of oxygen gas collected, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 732.2 torr

The conversion of P(torr) to P(atm) is shown below:

$P(torr)=\frac {1}{760}\times P(atm)$

So,

Pressure = 732.2 / 760 atm = 0.9634 atm

V = Volume of the gas = 23 mL = 0.023 L

T = Temperature of the gas = $22^oC=[22+273]K=295K$

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

n = number of moles of oxygen gas = ?

Applying the equation as:

0.9634 atm × 0.023 L = n × 0.0821 L.atm/K.mol × 295.15 K

⇒n = $9.14\times 10^{-4}$ moles

3 0

4 years ago

The mole is a counting number that allows scientists to describe how individual molecules and atoms react. If one mole of atoms

larisa [96]

Answer:

$\large \boxed{1.503 \times 10^{23}\text{ molecules of Cu(OH)}_{2}}$}$

Explanation:

You must calculate the moles of Cu(OH)₂, then convert to molecules of Cu(OH)₂.

1. Moles of Cu(OH)₂ $\text{Moles of Cu(OH)}_{2} = \text{24.35 g Cu(OH)}_{2} \times \dfrac{\text{1 mol Cu(OH)}_{2}}{\text{97.562 g Cu(OH)}_{2}} = \text{0.2496 mol Cu(OH)}_{2}$

2. Molecules of Cu(OH)₂ $\text{No. of molecules} = \text{0.2496 mol Cu(OH)}_{2} \times \dfrac{6.022 \times 10^{23}\text{ molecules Cu(OH)}_{2}}{\text{1 mol Cu(OH)}_{2}}\\\\= \mathbf{1.503 \times 10^{23}}\textbf{ molecules Cu(OH)}_{2}\\\text{There are $\large \boxed{\mathbf{1.503 \times 10^{23}}\textbf{ molecules of Cu(OH)}_{2}}$}$

4 0

4 years ago