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Mazyrski [523]
3 years ago
14

Help please I don’t know the answer

Chemistry
2 answers:
scoray [572]3 years ago
8 0
I think is 3 dude but im not good at this so
Nostrana [21]3 years ago
6 0

The answer is 3 It is a body of knowledge gained using inquiry and experimentation. Hope this helped!

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A chemical engineer studying the properties of fuels placed 1.670 g of a hydrocarbon in the bomb of a calorimeter and filled it
tigry1 [53]

Answer:

856,68 J/gram

Explanation:

We know that the variaton of temperature of 1K is equal to 1°C

so if the ΔT is 3.55°C, it is 3.55K.

so

403 J - 1 K

x - 3.55K

X= 403 * 3.55 = 1430,65 J

1.670 g - 1430,65 J

1 g - y

y = \frac{1430,65}{1.670} = 856,68 J

7 0
3 years ago
What is the temperature of 0.5 moles of water vapor that occupies 120 dm3 and applies a pressure of 15,000 Pa to its container?
AleksandrR [38]

Answer:

The answer is C. 7.52 K

Explanation:

hope it helps

6 0
3 years ago
If 143.56 mL of 0.6653 M ammonium carbonate reacts with 175.37 mL of 0.8732 M chromium(III) sulfate in a double replacement reac
Cloud [144]
ANSWER=83.42%

EXPLANATION:

4 0
2 years ago
Read 2 more answers
Which has the higher percentage of aluminum, Al2O, or Al(NO3)3
Rzqust [24]

Al₂O  has a higher percentage of aluminium.

Explanation:

To solve this problem, we have to compare the molar mass of the aluminium in each compound to one another as percentage of the whole compound:

Molar mass of Al₂O = 2(27) + 16 = 70g/mol

Molar mass of Al(NO₃)₃ = 27 + 3[14 + 3(16)] = 213g/mol

Percentage by mass of Al in Al₂O = \frac{2x27}{70} x 100 = 77%

Percentage by mass of Al in  Al(NO₃)₃ = \frac{27}{213} x 100 = 12.7%

Al₂O  has a higher percentage of aluminium.

learn more:

Molar mass brainly.com/question/2861244

#learnwithBrainly

8 0
3 years ago
Hydroxylamine hydrochloride is a powerful reducing agent which is used as a polymerization catalyst. It contains 5.80 mass % H,
ludmilkaskok [199]

<u>Answer:</u> The empirical formula for the given compound is H_{4}O_1N_1Cl_1=H_4NOCl

<u>Explanation:</u>

We are given:

Percentage of H = 5.80 %

Percentage of O = 23.02 %

Percentage of N = 20.16 %

Percentage of Cl = 51.02 %

Let the mass of compound be 100 g. So, percentages given are taken as mass.

Mass of H = 5.80 g

Mass of O = 23.02 g

Mass of N = 20.16 g

Mass of Cl = 51.02 g

To formulate the empirical formula, we need to follow some steps:

  • <u>Step 1:</u> Converting the given masses into moles.

Moles of Hydrogen = \frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{5.80g}{1g/mole}=5.80moles

Moles of Oxygen = \frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{23.02g}{16g/mole}=1.44moles

Moles of Nitrogen = \frac{\text{Given mass of nitrogen}}{\text{Molar mass of nitrogen}}=\frac{20.16g}{14g/mole}=1.44moles

Moles of Chlorine = \frac{\text{Given mass of Chlorine}}{\text{Molar mass of Chlorine}}=\frac{51.02g}{35.5g/mole}=1.44moles

  • <u>Step 2:</u> Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 1.44 moles.

For Hydrogen = \frac{5.80}{1.44}=4.03\approx 4

For Oxygen = \frac{1.44}{1.44}=1

For Nitrogen = \frac{1.44}{1.44}=1

For Chlorine = \frac{1.44}{1.44}=1

  • <u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of H : O : N : Cl = 4 : 1 : 1 : 1

Hence, the empirical formula for the given compound is H_{4}O_1N_1Cl_1=H_4NOCl

3 0
3 years ago
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