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Explain HOW this chemical reaction is NOT balanced correctly.

NeTakaya

Answer: there is more atoms of each element on the right.

Explanation:

On the left of the arrow you have:

Si-1

F-4

H-4

O-2

On the right of the arrow you have:

Si-3

F-6

H-8

O-4

A balanced equation always has the same amount of each element on the left of the arrow (the reactants) as the right (the products). This isn’t balanced because you have a lot more of each element on the right.

5 0

3 years ago

Read 2 more answers

The dopamine molecule has an intermediate hydrophobicity. Edit the dopamine molecule so that it is more hydrophobic.

yulyashka [42]

You should edit the dopamine molecule by tampering with its polar groups. Polar groups affect chemical's physical properties including hydrophobicity.

5 0

4 years ago

C) What volume of dilute HNO3 solution (0.150 mol/L) would be required

babymother [125]

Answer: 1.15L

Explanation:Please see attachment for explanation

5 0

3 years ago

Given the reaction represented by the balanced equation:

user100 [1]

Answer:

$mass of CHF_3 = 1/3 \times 9.47 \times 70 =220.97g$

Explanation:

$CH_4(g)+3F_2(g)->3HF(g)+CHF_3$

As given in the question that methane( $CH_4$ ) is taken excess amount

mass of $CHF_3$ depend only on mass of fluorine

mass of $F_2$ =180 g

mole of $F_2$ = $\frac{180}{19}$ =9.47

3 mole of $F_2$ gives 1 mole of $CHF_3$

so 1 mole will give $\frac{1}{3}$ mole of $CHF_3$

therefore,

9.47 mole of $F_2$ will give $\frac{1}{3} \times 9.47$ mole of $CHF_3$

$mass of CHF_3 = 1/3 \times 9.47 \times 70 =220.97g$

7 0

3 years ago

Percentage Yield

scoundrel [369]

Q.No. 1:

You have 20.0 g of CaCO₃. You decompose it by heat, and weigh the calcium oxide that remains. You have 10.3 grams. What is the % yield?

Answer:

%age Yield = 92.37 %

Solution:

The balance chemical equation for given decomposition reaction is;

CaCO₃ → CaO + CO₂

Step 1: Calculate Moles of CaCO₃:

Moles = Mass / M.Mass

Moles = 20.0 g / 100.08 g/mol

Moles = 0.199 moles of CaCO₃

Step 2: Calculate theoretical amount of CaO produced;

According to equation,

1 moles of CaCO₃ produced = 1 mole of CaO

So,

0.199 moles of CaCO₃ will produce = X moles of CaO

Solving for X,

X = 0.199 mol × 1 mol / 1 mol

X = 0.199 mol of CaO

Also,

Mass = Moles × M.Mass

Mass = 0.199 mol × 56.07 g/mol

Mass = 11.15 g of CaO

Step 3: Calculate %age Yield as;

%age Yield = Actual Yield / Theoretical Yield × 100

%age Yield = 10.3 g / 11.15 g × 100

%age Yield = 92.37 %

___________________________________________

Q.No. 2:

A student makes sodium chloride by buming 2.3 grams of sodium in chlorine gas. If the yield is 90%, how much sodium chloride is made?

Answer:

Actual Yield = 5.785 g of NaCl

Solution:

The balance chemical equation for given decomposition reaction is;

2 Na + Cl₂ → 2 NaCl

Step 1: Calculate Moles of Na:

Moles = Mass / M.Mass

Moles = 2.3 g / 23 g/mol

Moles = 0.10 moles of Na

Step 2: Calculate theoretical amount of NaCl produced;

According to equation,

2 moles of Na produced = 2 moles of NaCl

So,

0.10 moles of Na will produce = X moles of NaCl

Solving for X,

X = 0.10 mol × 2 mol / 2 mol

X = 0.10 mol of NaCl

Also,

Mass = Moles × M.Mass

Mass = 0.10 mol × 58.44 g/mol

Mass = 5.844 g of NaCl

Step 3: Calculate Actual Yield as;

%age Yield = Actual Yield / Theoretical Yield × 100

Or,

Actual Yield = %age Yield × Theoretical Yield ÷ 100

Actual Yield = 99 × 5.844 g ÷ 100

Actual Yield = 5.785 g of NaCl

___________________________________________

Q.No. 3:

For the chemical reaction Mg(s) + 2 HCl (aq) → H₂ (g) + MgCl₂ (aq) calculate the % yield if 100 grams of magnesium react with excess HCl to produce 310 grams of MgCl₂.

Answer:

%age Yield = 79.13 %

Solution:

The balance chemical equation for given decomposition reaction is;

Mg + 2 HCl → MgCl₂ + H₂

Step 1: Calculate Moles of Mg:

Moles = Mass / M.Mass

Moles = 100 g / 24.30 g/mol

Moles = 4.11 moles of Mg

Step 2: Calculate theoretical amount of MgCl₂ produced;

According to equation,

1 mole of Mg produced = 1 mole of MgCl₂

So,

4.11 moles of Mg will produce = X moles of MgCl₂

Solving for X,

X = 4.11 mol × 1 mol / 1 mol

X = 4.11 mol of MgCl₂

Also,

Mass = Moles × M.Mass

Mass = 4.11 mol × 95.21 g/mol

Mass = 391.73 g of MgCl₂

Step 3: Calculate %age Yield as;

%age Yield = Actual Yield / Theoretical Yield × 100

%age Yield = 310.0 g / 391.73 g × 100

%age Yield = 79.13 %

5 0

4 years ago