Suppose you wanted to make 100 grams of water. How many grams of hydrogen and oxygen will you need?

What particle is needed to complete the following equation?<br> 14/7N + ____ ---> 14/6C + 1/1H

yawa3891 [41]

Explanation:

The given reaction equation is as follows.

$^{14}_{7}N$ + ___ $\rightarrow ^{14}_{6}C + ^{1}_{1}H$

As there is release of one hydrogen which shows that mass number has increase by 1 on the product side.

Therefore, particle $^{1}_{0}n$ must be added in order to balance the given reaction equation.

Hence, the complete reaction equation will be as follows.

$^{14}_{7}N + ^{1}_{0}n \rightarrow ^{14}_{6}C + ^{1}_{1}H$

8 0

3 years ago

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What is hallucination

Sindrei [870]

Answer:

<h3>Hallucination is an experience involving the apparent perception of something not present .</h3>

Explanation:

<h3>Please mark my answer as a brainliest. Please follow me .❤❤❤❤</h3>

3 0

3 years ago

A 3.50 g sample of an unknown compound containing only C , H , and O combusts in an oxygen‑rich environment. When the products h

statuscvo [17]

Explanation:

First, calculate the moles of $CO_{2}$ using ideal gas equation as follows.

PV = nRT

or, n = $\frac{PV}{RT}$

= $\frac{1 atm \times 4.41 ml}{0.0821 Latm/mol K \times 293 K}$ (as 1 bar = 1 atm (approx))

= 0.183 mol

As, Density = $\frac{mass}{volume}$

Hence, mass of water will be as follows.

Density = $\frac{mass}{volume}$

0.998 g/ml = $\frac{mass}{3.26 ml}$

mass = 3.25 g

Similarly, calculate the moles of water as follows.

No. of moles = $\frac{mass}{\text{molar mass}}$

= $\frac{3.25 g}{18.02 g/mol}$

= 0.180 mol

Moles of hydrogen = $0.180 \times 2$ = 0.36 mol

Now, mass of carbon will be as follows.

No. of moles = $\frac{mass}{\text{molar mass}}$

0.183 mol = $\frac{mass}{12 g/mol}$

= 2.19 g

Therefore, mass of oxygen will be as follows.

Mass of O = mass of sample - (mass of C + mass of H)

= 3.50 g - (2.19 g + 0.36 g)

= 0.95 g

Therefore, moles of oxygen will be as follows.

No. of moles = $\frac{mass}{\text{molar mass}}$

= $\frac{0.95 g}{16 g/mol}$

= 0.059 mol

Now, diving number of moles of each element of the compound by smallest no. of moles as follows.

C H O

No. of moles: 0.183 0.36 0.059

On dividing: 3.1 6.1 1

Therefore, empirical formula of the given compound is $C_{3}H_{6}O$ .

Thus, we can conclude that empirical formula of the given compound is $C_{3}H_{6}O$ .

6 0

3 years ago

A 650.0 mL solution contains 125 grams of glucose (C6H12O6). If the molar mass of C6H12O6 is 180.16 g/mol, what is the molarity

Aleks [24]

Molarity of a solution is the molar concentration, which is the number of moles of solute in 1 L of solution.

the mass of glucose is - 125 g

number of moles of glucose - 125 g / 180.16 g/mol = 0.694 mol

the number of moles of glucose in 650.0 x 10⁻³ L - 0.694 mol

number of moles of glucose in 1 L - 0.694 mol / 650.0 x 10⁻³ L = 1.068 mol/L

molarity of glucose solution is 1.068 M

4 0

3 years ago

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How are an acid and a base define and describe the nature of each based on the strength, pH, and ion concentration?

Stels [109]

here are some notes i took on acids and bases and salts...i hope this helps

3 0

3 years ago