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3 years ago

In Europe gasoline is often sold in liters. If a typical fill-up requires 11 gal of gas, how many liters are necessary?

Chemistry

1 answer:

egoroff_w [7]3 years ago

3 0

Answer:

41,64 liters

Explanation:

In order to change the units we need to know the equivalence of said units.

1 gal of gas equals to 3,78541 liters.

We can use cross-multiplication in order to convert it into liters:

$\frac{1 gal}{3.78541 L} = \frac{11 gal}{X} \\\\X= \frac{3.78541 L x 11 gal}{1 gal}$

A typical fill-up requires 41,64 liters.

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gregori [183]

Answer:

v = 16.49 m/s

Explanation:

Given that,

Length of the string, l = 1.15 m

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We know that, 1 turn = 6.28 rad

137 turns = 860.79 rad

1 min = 60 s

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We need to find the tangential velocity of the ball. It can be given by

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So, the tangential velocity of the ball is 16.49 m/s.

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3 years ago

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Answer:

FALSE

Explanation:

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3 years ago

Read 2 more answers

A possible mechanism for the gas phase reaction of NO and H2 is as follows: Step 1 2NO N2O2 Step 2 N2O2 + H2 N2O + H2O Step 3 N2

mel-nik [20]

Answer: Option (d) is the correct answer.

Explanation:

Steps involved for the given reaction will be as follows.

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Rate expression for step 1 is as follows.

Rate = k $[NO]^{2}$

Step 2: $N_{2}O_{2} + H_{2} \rightarrow N_{2}O + H_{2}O$

This step 2 is a slow step. Hence, it is a rate determining step.

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Here, $N_{2}O_{2}$ is intermediate in nature.

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Thus, we can conclude that the statement step 1 is the rate determining step, concerning this mechanism is not directly supported by the information provided.

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3 years ago

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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.

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