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3 years ago

Which formulas represent compounds?

Chemistry

2 answers:

Nimfa-mama [501]3 years ago

6 0

The answer will be B

Alexxandr [17]3 years ago

5 0

Your answer is B. CO2 ; H2O

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A compound contains carbon and hydrogen this compound goes through a combustion reaction such that compound y is produced from t

Olegator [25]

Answer:

x is CO2

y is H2O

Explanation:

An organic compound that contains carbon and hydrogen is called a hydrocarbon.

When a hydrocarbon is burnt in air (combustion) only two products are obtained; carbon dioxide and water. The carbon dioxide comes from the carbon component of the molecule while the water comes from the hydrogen component of the molecule.

Therefore, for a hydrocarbon CxHy we obtain; xCO2 and (x + 1)H2O as products.

6 0

3 years ago

Diffusion occurs faster in gases than in liquids because _____.

zalisa [80]

Diffusion occurs faster in a gas than in liquids because in a liquid the molecules are closser together and in a gas they are farther appart

6 0

4 years ago

Read 2 more answers

What is the molarity of a solution that contains 12 moles of solute and 583 ml of solution?

frozen [14]

Answer:

21 M

Explanation:

Molarity = mol solute/ L solution = 12 mol/0.583 L ≈ 21 mol/L = 21 M

5 0

3 years ago

Suppose that 98.0g of a non electrolyte is dissolved in 1.00kg of water. The freezing point of this solution is found to be -0.4

Sholpan [36]

Answer:

$\large \boxed{\text{392 u}}$

Explanation:

1. Calculate the molal concentration

The formula for the freezing point depression by a nonelectrolyte is

$\Delta T_{f} = -K_{f}b\\b = -\dfrac{\Delta T_{f}}{ K_{f}} = -\dfrac{-0.465 \, ^{\circ}\text{C}}{\text{1.86 $\, ^{\circ}$C$\cdot$kg$\cdot$mol}^{-1}} = \text{0.250 mol/kg}$

2. Calculate the moles of solute

$\begin{array}{rcl}b & = & \dfrac{\text{moles of solute}}{\text{kilograms of solvent}}\\\\\text{moles of solute} & = & b \times {\text{kilograms of solvent}}\\n & = &\text{0.250 mol/kg} \times \text{1.00 kg}\\ & = & \text{0.250 mol}\\\end{array}$

3. Calculate the molecular mass

$\begin{array}{rcl}\text{Moles} & = &\dfrac{\text{mass}}{\text{molar mass}}\\\\\text{0.250 mol} & = & \dfrac{\text{98.0 g}}{MM}\\\\MM & = & \dfrac{\text{98.0 g }}{\text{0.250 mol}}\\\\& = &\textbf{392 g/mol}\\\end{array}\\\text{The molecular mass of the solute is $\large \boxed{\textbf{392 u}}$}$

3 0

3 years ago

What s thisssss oneeeeeee

ZanzabumX [31]

C
Explanation- equals 459

3 0

3 years ago