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3 years ago

Which of the following is NOT a chemical reaction?

Chemistry

1 answer:

Damm [24]3 years ago

6 0

Ice melting from water. Nothing has changed except the state of matter.

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A laboratory analysis of a sample finds it is composed of 38.8% carbon, 16.2% hydrogen, and 45.1% nitrogen. What is its empirica

Sladkaya [172]

Answer: The empirical formula for the given compound is $CH_5N$

Explanation : Given,

Percentage of C = 38.8 %

Percentage of H = 16.2 %

Percentage of N = 45.1 %

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

Mass of C = 38.8 g

Mass of H = 16.2 g

Mass of N = 45.4 g

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

Step 1: Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{38.8g}{12g/mole}=3.23moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{16.2g}{1g/mole}=16.2moles$

Moles of Nitrogen = $\frac{\text{Given mass of nitrogen}}{\text{Molar mass of nitrogen}}=\frac{45.4g}{14g/mole}=3.24moles$

Step 2: 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 3.23 moles.

For Carbon = $\frac{3.23}{3.23}=1$

For Hydrogen = $\frac{16.2}{3.23}=5.01\approx 5$

For Oxygen = $\frac{3.24}{3.23}=1.00\approx 1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H : N = 1 : 5 : 1

Hence, the empirical formula for the given compound is $C_1H_5N_1=CH_5N$

3 0

3 years ago

Which element could not form in the sun and would have to be formed in a supernova?.

sasho [114]

Uranium, most uranium does derive from a star. However, not from our sun.

7 0

2 years ago

Which of the following lists the relative strengths of the fundamental forces from strongest to weakest?

den301095 [7]

Answer:

D. Strong nuclear force, electrostatic force, weak nuclear force, gravitational force

7 0

3 years ago

Determine the empirical formula of the following compound if a sample contains 0.104 molK, 0.052 molC, and 0.156 molO;?

faltersainse [42]

Answer:

K₂CO₃

Explanation:

Given parameters:

Number of moles of K = 0.104mol

Number of moles of C = 0.052mol

Number of moles of O = 0.156mol

Method

From the given parameters, to calculate the empirical formula of the elements K, C and O, we reduce the given moles to the simplest fraction.

Empirical formula is the simplest formula of a compound and it differs from the molecular formula which is the actual formula of a compound.

Divide the given moles through by the smallest which is C, 0.052mol.
Then approximate values obtained to the nearest whole number of multiply by a factor to give a whole number ratio.
This is the empirical formula

Solution

Elements K C O

Number of moles 0.104 0.052 0.156

Dividing by the

smallest 0.104/0.052 0.052/0.052 0.156/0.052

2 1 3

The empirical formula is K₂CO₃

3 0

3 years ago

How would i calculate molecules of water produced in a reaction?

levacccp [35]

You would calculate them by dividing them and then multiplying to get the final answer

5 0

4 years ago