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3 years ago

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If the number of atoms of each element on the reactant side of an equation is equal to the number of atoms of each element on th

e product side of the equation, the equation is _____.
A.)endothermic
B.)equal
C.)balanced
D.)exothermic

1 answer:

cricket20 [7]3 years ago

6 0

C. Is your answer hope you have a wonderful day

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Salt in crude oil must be removed before the oil undergoes processing in a refinery. The

irina1246 [14]

Answer:

$\large \boxed{0.64 \, \%}$

Explanation:

Assume you are using 1 L of water.

Then you are washing 4 L of salty oil.

1. Calculate the mass of the salty oil

Assume the oil has a density of 0.86 g/mL.

$\text{Mass of oil} = \text{4000 mL} \times \dfrac{\text{0.86 g}}{\text{1 mL}} = \text{3440 g}$

2. Calculate the mass of salt in the salty oil

$\text{Mass of salt} = \text{3440 g} \times \dfrac{\text{5 g salt}}{\text{100 g oil}} = \text{172 g salt}$

3. Calculate the mass of salt in the spent water

$\text{Mass of salt} = \text{1000 g water} \times \dfrac{\text{15 g salt}}{\text{100 g water}} = \text{150 g salt}$

4. Mass of salt remaining in washed oil

Mass = 172 g - 150 g = 22 g

5. Concentration of salt in washed oil

$\text{Concentration} = \dfrac{\text{22 g}}{\text{3440 g}} \times 100 \, \% = \mathbf{0.64 \, \%}\\\\\text{The concentration of salt in the washed oil is $\large \boxed{\mathbf{0.64 \, \%}}$}$

3 0

3 years ago

giving the incomplete equation 2N2O5 (g) which set of products completes and balances the incomplete equarion

a_sh-v [17]

Answer:

The complete question is as follows

Given the incomplete equation: 2 N2O5(g) ==> Which set of products completes and balances the incomplete equation?

A)2 N2(g) + 3 H2(g)

B)2 N2(g) + 2 O2(g)

C)4 NO2(g) + O2(g)

D)4 NO(g) + SO2(g)

The correct option is C) 4NO2(g) + O2(g)

Explanation:

Note that the products should be NO2 and O2 since the reactant is entirely made up of N and O. option A is not correct as hydrogen cannot emerge as a product in this reaction. Matter can never be created or be destroyed bu can only change in a chemical reaction. Option D is not also correct for the same reason.

Option B is not correct since it did not balance the number of atoms of O and N in the reactant side of the equation.

The option C) 4NO2(g) + O2(g) is therefore the right option since it balances both the elements and the number of atoms of the elements present.

7 0

3 years ago

Which statement describes what happens to the DNA in the process shown? A. Some of the DNA is destroyed, so each daughter cell h

kolbaska11 [484]

hhjjjbvhjbvb

hhmkn

hjkk

hhjj

7 0

3 years ago

When 7.085 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.71 grams of CO2 and 10.37 grams of H

Taya2010 [7]

Answer:

- Empirical:

$C_3H_7$

- Molecular:

$C_6H_{14}$

Explanation:

Hello,

In this case, based on the information regarding the combustion, the moles of carbon turn out:

$n_C=21.71gCO_2*\frac{1molCO_2}{44gCO_2}*\frac{1molC}{1molCO_2}=0.493molC$

Moreover, the moles of hydrogen:

$n_H=10.37gH_2O*\frac{1molH_2O}{18gH_2O}*\frac{2molH}{1molH_2O}=1.152molH$

Thus, the subscripts of carbon and hydrogen in the hydrocarbon turn out:

$C=\frac{0.4934}{0.4934}=1\\H=\frac{1.15222}{0.4934}=2.335\\CH_{2.335}$

Now, looking for a suitable whole number we obtain the following empirical formula as 2.335 times 3 is 7 for hydrogen:

$C_3H_7$

In such a way, that compound has a molar mass of 43 g/mol, thus, the whole compound's molar mass is 86.18 g/mol for which the molecular formula is twice the empirical one, therefore:

$C_6H_{14}$

Which is hexane.

Best regards.

6 0

3 years ago

What is the percent of hydrogen peroxide in the solution when 5.02g of H2O2 solution reacts to produce 0.153g of H2O2? 2H2O2 (l)

Murljashka [212]

<u>Given:</u>

Mass of H2O2 solution = 5.02 g

Mass of H2O2 = 0.153 g

<u>To determine: </u>

The % H2O2 in solution

<u>Explanation:</u>

Chemical reaction-

2H2O2(l) → 2H2O(l) + O2(g)

Mass % of a substance in a solution = (Mass of the substance/Mass of solution) * 100

In this case

% H2O2 = (Mass H2O2/Mass of solution)* 100 = (0.153/5.02)*100 = 3.05%

Ans: % H2O2 in the solution = 3.05%

5 0

3 years ago