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3 years ago

Claudia and her team of scientists develop a new car battery that recharges electric cars at a fast rate.

Chemistry

1 answer:

Doss [256]3 years ago

7 0

Answer: Waste Operators will handle less hazardous material.

Explanation: Since the electric car is electric it produces hazardous material and now that it doesn't it wont.

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Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly

Katen [24]

Answer:

We will produce 57.1 grams of silver sulfadiazine

Explanation:

Silver sulfadiazine burn-treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly into the wound. If 20.0 g of Ag2O is reacted with 40.0 of C10H10N4SO2, what mass of silver sulfadiazine (AgC10H9N4SO2) can be produced assuming 100% yield?

Step 1: Data given

Mass of Ag2O = 20.0 grams

Molar mass of Ag2O = 231.735 g/mol

Mass of C10H10N4SO2 = 40.0 grams

Molar mass of C10H10N4SO2 = 250.277 g/mol

Step 2: The balanced equation

Ag2O + 2C10H10N4SO2 → 2AgC10H9N4SO2 + H2O

Step 3: Calculate moles Ag2O

Moles Ag2O = mass Ag2O / molar mass Ag2O

Moles Ag2O = 20.0 grams / 231.735 g/mol

Moles Ag2O = 0.0863 moles

Step 4: Calculate moles C10H10N4SO2

Moles C10H10N4SO2 = 40.0 grams / 250.277 g/mol

Moles C10H10N4SO2 = 0.160 moles

Step 5: Calculate the limiting reactant

For 1 mol Ag2O we need 2 moles 2C10H10N4SO2 to produce 2 moles AgC10H9N4SO2 and 1 mol H2O

C10H10N4SO2 is the limiting reactant. There will react 0.160 moles.

Ag2O is in excess. There will react 0.160/ 2 = 0.080 moles

There will remain 0.0863 - 0.080 = 0.0063 moles Ag2O

Step 5: Calculate moles AgC10H9N4SO2

For 1 mol Ag2O we need 2 moles 2C10H10N4SO2 to produce 2 moles AgC10H9N4SO2 and 1 mol H2O

For 0.160 moles C10H10N4SO2 we'll have 0.160 moles AgC10H9N4SO2

Step 6: Calculate mass AgC10H9N4SO2

Mass AgC10H9N4SO2 = moles * molar mass

Mass AgC10H9N4SO2 = 0.160 moles * 357.137 g/mol

Mass AgC10H9N4SO2 = 57.1 grams

We will produce 57.1 grams of silver sulfadiazine

6 0

3 years ago

What type of matter is salt water?

algol13

Salt water is a Homogeneous Mixture......

8 0

3 years ago

PLEASE HELP. !!

scoray [572]

Answer:

Potential energy = 441 N

Explanation:

Given:

Mass M = 15 kg

Height = 3 m

Find:

Potential energy

Computation:

Potential energy = mgh

Potential energy = (15)(9.8)(3)

Potential energy = 441 N

8 0

3 years ago

What is the difference in concentration between a pH of 7 and 12?

Ratling [72]

Answer:

The pH of a solution is simply a measure of the concentration of hydrogen ions,

, which you'll often see referred to as hydronium cations,

More specifically, the pH of the solution is calculated using the negative log base

of the concentration of the hydronium cations.

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

−

log

(

[

]

)

∣

−−−−−−−−−−−−−−−−−−−−−−−−

Now, we use the negative log base

because the concentration of hydronium cations is usually significantly smaller than

As you know, every increase in the value of a log function corresponds to one order of magnitude.

Explanation:

4 0

3 years ago

Read 2 more answers

The metal content of iron in ores can be determined by a redox procedure in which the sample is first oxidized with Br2 to conve

coldgirl [10]

Answer:

80.27%

Explanation:

Let's consider the following balanced equation.

2 Fe³⁺(aq) + Sn²⁺(aq) ⇒ 2Fe²⁺(aq) + Sn⁴⁺(aq)

First, we have to calculate the moles of Sn²⁺ that react.

$\frac{0.1015molSn^{2+} }{1L} .13.28 \times 10^{-3} L=1.348\times 10^{-3}molSn^{2+}$

We also know the following relations:

According to the balanced equation, 1 mole of Sn²⁺ reacts with 2 moles of Fe³⁺.
1 mole of Fe³⁺ is oxidized from 1 mole of Fe.
The molar mass of Fe is 55.84 g/mol.

Then, for 1.348 × 10⁻3 moles of Sn²⁺:

$1.348\times 10^{-3}molSn^{2+}.\frac{2molFe^{3+} }{1molSn^{2+} } .\frac{1molFe}{1molFe^{3+} } .\frac{55.84gFe}{1molFe} =0.1505gFe$

If there are 0.1505 g of Fe in a 0.1875 g sample, the mass percentage of Fe is:

$\frac{0.1505g}{0.1875g} \times 100 \% = 80.27\%$

5 0

4 years ago