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2 years ago

Two cars that are identical except for their color are traveling on the same road.

Chemistry

2 answers:

Ray Of Light [21]2 years ago

7 0

B. The blue car has more kinetic energy than the red car

Bogdan [553]2 years ago

4 0

The answer would be B

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KF + 02 <br><br> Balance the equation

Paladinen [302]

Explanation:

this equation is balanced

if you look at it carefully

k=1

f=1

o=2

we do not have any opposing element

5 0

2 years ago

Read 2 more answers

What is the volume of stank of nitrogen that contains 17 moles of nitrogen at 34 C under 12,000Pa?

Otrada [13]

Answer:

3626.76dm³

Explanation:

Given parameters:

Number of moles of Nitrogen in tank = 17moles

Temperature of the gas = 34°C

Pressure on the gas = 12000Pa

Unkown:

Volume of the tank, V =?

Converting the parameters to workable units:

We take the temperature from °C to Kelvin

K = 273 + °C = 273 + 34 = 307k

Taking the pressure in Pa to atm:

101325Pa = 1atm

12000Pa = 0.118atm

Solution:

To solve this problem, we employ the use of the ideal gas equation. The ideal gas law combines three gas laws which are the Boyle's law, Charles's law and the Avogadro's law.

It is expressed as PV = nRT

The unknown is the Volume and we make it the subject of the formula

V = $\frac{nRT}{P}$

Where R is called the gas constant and it is given as 0.082atmdm³mol⁻¹K⁻¹

Therefore V = $\frac{17 x 0.082 x 307 }{0.118}$ = 3626.76dm³

3 0

3 years ago

Read 2 more answers

Balance the following chemical reaction:

mrs_skeptik [129]

Answer:

what the freak is thisnenejehey

7 0

3 years ago

Read 2 more answers

A charged rubber rod can pick up a small neutrally charged piece of paper by what process

seropon [69]

Ion induced dipole process

8 0

3 years ago

Create the Equation: What is the Percent Yield of Ammonia (NH3) if 11.8 g is recovered in a reaction with 7.02 x 10^23 molecules

insens350 [35]

Answer:

Explanation:

The first thing that you need to do here is to calculate the theoretical yield of the reaction, i.e. what you get if the reaction has a

100

yield.

The balanced chemical equation

(

)

(

)

→

(

)

tells you that every

mole of nitrogen gas that takes part in the reaction will consume

moles of hydrogen gas and produce

mole of ammonia.

In your case, you know that

mole of nitrogen gas reacts with

mole of hydrogen gas. Since you don't have enough hydrogen gas to ensure that all the moles of nitrogen gas can react

what you need

3 moles H (sub 2)

what you have

1 mole H (sub2)

you can say that hydrogen gas will act as a limiting reagent, i.e. it will be completely consumed before all the moles of nitrogen gas will get the chance to take part in the reaction.

So, the reaction will consume

mole of hydrogen gas and produce

mole H

⋅

2 moles NH

moles H

0.667 moles NH

100

yield. This represents the reaction's theoretical yield.

Now, you know that the reaction produced

0.50

moles of ammonia. This represents the reaction's actual yield.

In order to find the percent yield, you need to figure out how many moles of ammonia are actually produced for every

100

moles of ammonia that could theoretically be produced.

You know that

0.667

moles will produce

0.50

moles, so you can say that

100

moles NH

in theory

⋅

0.50 moles NH

actual

0.667

moles NH

in theory

75 moles NH

actual

Therefore, you can say that the reaction has a percent yield equal to

% yield = 75%

−−−−−−−−−−−−−

or 75 moles NH sub3

I'll leave the answer rounded to two sig figs.

5 0

2 years ago