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3 years ago

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In a 4.00 L pressure cooker, water is brought to a boil. If the final temperature is 115 °C at 3.10 atm, how many moles of steam

are in the cooker?

1 answer:

Olenka [21]3 years ago

7 0

Answer: 0.39mol of the steam are in the cooker.

Explanation:Please see attachment for explanation

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The entropy change for a real, irreversible process is equal to:______.

taurus [48]

Answer:

The entropy change for a real, irreversible process is equal to <u>zero.</u>

The correct option is<u> 'c'.</u>

Explanation:

<u>Lets look around all the given options -:</u>

(a) the entropy change for a theoretical reversible process with the same initial and final states , since the entropy change is equal and opposite in reversible process , thus this option in not correct.

(b) equal to the entropy change for the same process performed reversibly ONLY if the process can be reversed at all. Since , the change is same as well as opposite too . Therefore , this statement is also not true .

(c) zero. This option is true because We generate more entropy in an irreversible process. Because no heat moves into or out of the surroundings during the procedure, the entropy change of the surroundings is zero.

(d) impossible to tell. This option is invalid , thus incorrect .

<u>Hence , the correct option is 'c' that is zero.</u>

8 0

2 years ago

How can I calculate the mass percent of carbon, nitrogen and oxygen in caffeine, C8H10N4O2.

Ahat [919]

You must first calculate the total weight of 1 mole of the substance. You do this by finding the molar weights on the periodic table of each of the elements in the compound:

$8(12.01g)+10(1.008g)+4(14.007g)+2(15.999g)=96.08g+10.08g+56.028g+31.998g=194.186g$

So now we take the amount of each element that is given in the compound and divide it by the total mass of the compound:

Carbon: 96.08g

$\frac{96.08g}{194.186g}= 0.49478=49.48$

Carbon = 49.48%

Nitrogen: 56.028g

$\frac{56.028g}{194.186g}=0.28853=28.85$

Nitrogen = 28.85%

Oxygen: 31.998g

$\frac{31.998g}{194.186g} =0.16478=16.48$

Oxygen = 16.48%

8 0

2 years ago

Read 2 more answers

How many moles are in 3.113 g of Au?Molar mass of Au=197 g/mol

SVEN [57.7K]

<h3>Answer:</h3>

0.0157 g Au

<h3>General Formulas and Concepts:</h3>

<u>Chemistry</u>

<u>Atomic Structure</u>

Reading a Periodic Table
Using Dimensional Analysis

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

Brackets
Parenthesis
Exponents
Multiplication
Division
Addition
Subtraction

Left to Right

<h3>Explanation:</h3>

<u>Step 1: Define</u>

3.113 g Au

<u>Step 2: Identify Conversions</u>

Molar Mass of Au - 197.87 g/mol

<u>Step 3: Convert</u>

<u /> $3.113 \ g \ Au(\frac{1 \ mol \ Au}{197.87 \ g \ Au} )$ = 0.015733 g Au

<u>Step 4: Check</u>

<em>We are given 3 sig figs. Follow sig fig rules and round.</em>

0.015733 g Au ≈ 0.0157 g Au

3 0

2 years ago

It didn't have science but the subject is science. A climate with short cool summers and long, bitterly cold winters is the

kvasek [131]

Hey there,

Question : <span>A climate with short cool summers and long, bitterly cold winters is the?

Answer : D, Tundra Climate

Hope this helps :))

<em>~Top♥</em>
</span>

6 0

2 years ago

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Use the equation 2Cu+O2-->2CuO, to find how many grams of copper react to produce 2.44 mol CuO.

Alexandra [31]

According to the equation, the ratio of the reactant Cu and product CuO is 2:2, thus 1:1. Therefore to produce 2.44 mol CuO, 2.44 mol Cu is required. The molecular weight of Cu is 64. So the mass of Cu that is required to produce 2.44mol CuO is 2.44mol * 64 g/mol = 156.16 g.

7 0

2 years ago

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